Analytical Chemistry Flashcards by Abi Peralta

The pH of 10-4 gm hydrogen ion per liter of a solution is
A. 7
B. 8
C. 5
D. 4

D. 4

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A certain aqueous solution at 25ºC has [OH] = 6.2 E -5 M. Calculate the pH of the solution.
A. 4.21
B. 5.80
C. 8.20
D. 9.79

D. 9.79

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Assuming complete ionization, the pH of 0.01 M HCl solution would be
A. 1
B. 2
C. 3
D. 4

B. 2

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The pH of a solution is 6.38. Find the concentration of hydrogen ion in moles per liter.
A. 4.17E-7 M
B. 2.23E-7 M
C. 1.22E-6 M
D. 3.20E-6 M

A. 4.17E-7 M

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The hydrogen ion concentration of a solution is a thousand times greater than the hydroxide ion concentration. Find the pH of the solution.
A. 8.5
B. 7.5
C. 5.5
D. 6.5

C. 5.5

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If the solution X has a pH of 6 and solution Y has a hydronium ion concentration twice that of solution X, the approximate pH of solution Y is
A. 12.0
B. 3.0
C. 5.7
D. 9.0

C. 5.7

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Calculate the percent ionization of 0.05 M acetic acid. Ka = 1.8E-5
A. 6.7%
B. 4.5%
C. 2.4%
D. 1.9%

D. 1.9%

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A 0.01 M weak acid (contains one replaceable hydrogen) is 4.17% ionized. What is the ionization constant?
A. 1.8E-5
B. 1.2E-4
C. 3.6E-5
D. 1.2E-5

A. 1.8E-5

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What is the concentration of an HCN solution which is 0.02% ionized? Ka = 4E-10.
A. 0.001 M
B. 0.01 M
C. 0.1 M
D. 1 M

B. 0.01 M

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What is the pH of a 0.10 M solution of nitous acid (HNO2)? Ka = 7.2E-4
A. 1.43
B. 4.24
C. 2.09
D. 2.85

C. 2.09

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Calculate the pH of 0.10 M NH3(aq). K = 1.8E-5
A. 2.9
B. 11.1
C. 3.4
D. 10.6

B. 11.1

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What is the pH of 7.0E- 8 M acetic acid?
A. 6.85
B. 4.76
C. 8.90
D. 5.76

A. 6.85

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A 0.1 M solution of HAc has been buffered by the addition of NaAc. The H+ ion concentration is found to be 0.000025 M. What is the concentration of the acetate ion?
A. 0.072 M
B. 0.72 M
C. 0.045 M
D. 0.45 M

A. 0.072 M

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Find the hydrogen ion concentration in a liter of solution that contains 12.0 grams of acetic acid and 8.2 grams of sodium acetate.
A. 3.6 E-5 M
B. 6.3 E-5 M
C. 3.6 E-6 M
D. 6.3 E-6 M

A. 3.6 E-5 M

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The pH of an acetic acid-sodium acetate buffer whose salt to acid ration is 2 is
A. 4.74
B. 5.05
C. 6.95
D. 8.95

B. 5.05

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Find the hydrogen ion concentration in a solution containing 0.1 mole of HOCN and 0.1 mole of NaOCN per liter of solution.
A. 2E-4 M
B. 2E-5 M
C. 1.5E-6 M
D. 1.5E-3 M

A. 2E-4 M

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If 100 mL of 0.1 M NH4Cl solution is added to 150 mL of 0.1 M NH4OH solution, what is the hydroxide ion concentration in the resulting solution? Kb(NH4OH) = 1.8E-5.
A. 2.7 E-5 M
B. 2.7 E-4 M
C. 6.2 E-4 M
D. 6.2 E-5 M

A. 2.7 E-5 M

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Silver chromate, Ag2CrO4, is soluble to the extent of 0.0259 mole per liter. Calculate the solubility product constant. (6.9E-5 M3)
A. 1.9E-12
B. 1.9E-11
C. 1.9E-10
D. 1.9E-9

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Calculate the solubility of SrSO4 in grams per 100 mL of solution from its solubility product constant, Ksp = 7.6 E-7.
A. 0.016 g/100mL
B. 0.202 g/100mL
C. 0.152 g/100mL
D. 0.406 g/100mL

A. 0.016 g/100mL

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Calculate the solubility of Mg(OH)2 in grams per liter from the solubility product constant. Ksp = 8.9 E-12.
A. 0.0021 g/L
B. 0.0076 g/L
C. 0.187 g/L
D. 0.561 g/L

B. 0.0076 g/L

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To increase the solubility of sugar in water, you must
A. stir the solution vigorously
B. pulverize the sugar particles before adding them to the water
C. heat the solution
D. evaporate the water

C. heat the solution

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A certain organic monoacidic base with an ionization constant of 2.0 E 8 serves as an indicator in a neutralization titration. An intermediate shade of color is obtained at pH = 6. What percentage of the indicator has been converted to the ions at this point?
A. 67%
B. 70%
C. 60%
D. 55%

A. 67%

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A 0.1 M solution of sodium bicarbonate has a pH value of :
A. 7
B. 8.4
C. 5.6
D. 4.0

B. 8.4

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A certain organic base of the general formula ROH serves as an indicator in the neutralization titration. Its change of color is found to take place when it is one-quarter converted to ionic form. At this point the pH value of the solution is 5.6. What is the ionization constant of the indicator?
A. 1.3 E-9
B. 1.3 E-8
C. 1.3 E-7
D. 1.3 E-6

A. 1.3 E-9

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Calculate the hydronium-ion concentration of an aqueous, 0.150 M acetic acid solution. The Ka for acetic acid is 1.76 E -5.
A. 1.62 E-3 M
B. 1.62 E-2 M
C. 2.45 E-2 M
D. 2.45 E-3 M

A. 1.62 E-3 M

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What is the proof of a “wine cooler” that is 5% alcohol volume?
A. 2.5 proof
B. 5 proof
C. 10 proof
D. 50 proof

C. 10 proof

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What is the pH of a 1 E -8 M solution of HCl?
A. 6.98
B. 7.02
C. 5.76
D. 8.95

A. 6.98

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What is the ratio of the concentration of acetic acid to sodium acetate in a buffer whose pH is 5?
A. 0.56
B. 1.2
C. 1.8
D. 3.1

A. 0.56

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Calculate the solubility product constant of AgI solution if its solubility is 2.15 E-10 grams per 100 mL of solution.
A. 5.2 E-13
B. 8.4 E-17
C. 5.2 E-17
D. 8.4 E-13

B. 8.4 E-17

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What is the solubility product of barium fluoride if 1.3 grams of barium fluoride dissolve in a liter?
A. 1.2 E-6
B. 1.2 E-7
C. 1.7 E-6
D. 1.7 E-7

C. 1.7 E-6

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The hydrogen ion concentration of a solution is 5 E-6 M. Find pH.
A. 2.1
B. 3.2
C. 4.5
D. 5.3

D. 5.3

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The acidity constant for acetic acid is 1.8 E-5. Find pKa.
A. 3.6
B. 4.2
C. 4.7
D. 5.4

C. 4.7

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The pH of a solution is 6.38. Find the concentration of hydroxide ion in moles per liter.
A. 1.2 E-6
B. 2.4 E-8
C. 2.4 E-6
D. 1.2 E-8

B. 2.4 E-8

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The hydrogen ion concentration of a solution is 5E-6 M. Find pOH.
A. 5.3
B. 8.7
C. 4.8
D .9.2

B. 8.7

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What is the pH of 0.01 M solution HCl?
A. 3.5
B. 4.1
C. 3.9
D. 2.0

D. 2.0

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Calculate the pOH of a 0.020 M HCl solution.
A. 1.7
B. 12.3
C. 2.8
D. 11.2

B. 12.3

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In a 0.1 molar solution, cyanic acid is 4.4 percent dissociated. Find Ka.
A. 2.0 E-4
B. 2.0 E-5
C. 2.0 E-6
D. 2.0 E-7

A. 2.0 E-4

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Calculate the OHin 0.1 molar ammonium hydroxide solution. Kb = 1.8 E-5
A. 1.34 E- 2
B. 1.34 E-3
C. 4.2 E-4
D. 4.2 E-2

B. 1.34 E-3

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If 0.1 mole of solid NaOH solution is added to 150 mL 0.2 M HAc solution. Calculate the final H+
ion concentration.
A. 1.5 E-4 M
B. 2.6 E-4 M
C. 5.9 E-4 M
D. 4.6 E-6 M

D. 4.6 E-6 M

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100 mL of 0.1 M NaOH solution is added to 150 mL of 0.2 M HAc solution. Calculate the final H+ ion concentration.
A. 3.2 E-4 M
B. 3.7 E-5 M
C. 3.2 E-5 M
D. 3.7 E-6 M

B. 3.7 E-5 M

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Calculate the ionization constant of HAc if 0.1 M HAc is 1.34% ionized.
A. 1.2 E-4
B. 1.8 E-5
C. 2.6 E-4
D. 2.6 E-5

B. 1.8 E-5

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What is the pH of 0.256 M NH4Cl? Kb = 1.8 E-5
A. 2.64
B. 9.90
C. 11.36
D. 4.92

C. 11.36

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Phenol is monobasic acid with and ionization constant at 25ºC of 1.3 E-10. What is the pH value of a 1 M solution?
A. 1.2
B. 6.44
C. 3.45
D. 9.06

D. 9.06

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A 0.20 M solution of weak acid HA is 0.6% ionized. What is the value of ionization constant, Ka, for this acid?
A. 7.2 E-6
B. 7.2 E-7
C. 7.9 E-6
D. 7 E-5

A. 7.2 E-6

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A 4.2% ionized 0.01 M ammonia solution is prepared from ammonium hydroxide. Calculate the pH.
A. 10.62
B. 3.38
C. 8.55
D. 5.45

A. 10.62

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The ionization constant for acetic acid is 1.82 E-5. What is the hydrogen ion concentration for a 0.2 M solution?
A. 2.2 E-4 M
B. 7.7 E-5 M
C. 7.9 E-6 M
D. 7 E-5 M

C. 7.9 E-6 M

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Calculate the pH of an aqueous buffer solution which contains 0.100 mol/L NH3 and 0.200 mol/L NH4Cl.
A. 9
B. 8.5
C. 7.0
D. 10

A. 9

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Five mL of 3 M HAc is added to 50 ml of 1 M NaAc solution. Find the hydrogen ion concentration.
A. 5.4 E-6
B. 6.7 E-4
C. 1.2 E-8
D. 1.8 E-5

A. 5.4 E-6

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What is the pH of a solution containing 0.01 M acetic acid and 0.01 M sodium acetate?
A. 9.26
B. 4.74
C. 3.25
D. 10.75

B. 4.74

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The solubility of barium sulfate is 0.0091 g/L at 25ºC. What is the value of the solubility product constant of barium sulfate? The molar weight if the barium sulfate is 233 g/mol.
A. 1.52 E-9 mole2/L2
B. 8.63 E-7 mole2/L2
C. 4.24 E-8 mole2/L2
D. 2.98 E-6 mole2/L2

A. 1.52 E-9 mole2/L2

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The solubility of PbCl2 in water is 1.6 E-2 mole/L. What is the Ksp of PbCl2?
A. 5 E-4
B. 4.1 E-6
C. 3.1 E-7
D. 1.6 E-5

D. 1.6 E-5

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A saturated solutions of Ag2SO4, is soluble to the extent of 0.0259 mole per liter. Calculate the solubility product constant.
A. 6.26 E-6
B. 6.25 E- 4
C. 1.5626 E- 6
D. 3.125 E-6

A. 6.26 E-6

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Silver chromate, Ag2CrO4, is soluble to the extent of 0.0259 mole per liter. Calculate the solubility product constant.
A. 6.9 E-5
B. 6.9 E-6
C. 1.9 E-6
D. 1.9E-5

A. 6.9 E-5

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What is the concentration of the Ag+ ion in a saturated solution og AgCl? Ksp = 1.7 E-10
A. 1.7 E-10 M
B. 3.4 E-10 M
C. 1.3 E-5 M
D. 2.6 E-5 M

C. 1.3 E-5 M

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The solubility of CaF2 is 2 E-4 mol/liter. Its solubility product is
A. 2.0 E- 4
B. 4.0 E-8 M
C. 8.0 E-12 M
D. 3.2 E- 11 M

D. 3.2 E- 11 M

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What is the pH of buffer solution consisting of 0.20 M NH3 and 0.10 M NH4NO3 at 25ºC K for ammonia is 1.8 E-5
A. 5.6
B. 7.9
C. 13.2
D. 9.5

D. 9.5

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Calculate the ionization constant for0.1 M nitrous acid that is 6.5 % ionized.
A. 5.6 E-2
B. 1.8 E-5
C. 4.5 E-6
D. 1.8 E-5

C. 4.5 E-6

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Potassium hydroxide ionizes completely in water. What is the pH og 0.05 M KOH?
A. 1.3
B. 11.5
C. 2.5
D. 12.7

D. 12.7

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The pH of solution is 5.0. Its hydrogen ion concentration is decreased hundred times. Then the solution will be
A. more acidic
B. neutral
C. basic
D. of the same acidit

B. neutral

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Calculate the pH of a solution of 0.080 M HNO3.
A. 8.0
B. 5.4
C. 3.2
D. 1.1

D. 1.1

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The solubility product constant of Mg(OH)2 in water is 1.2 E-11. If the Mg2+ concentration in an acid solution is 1.2 E-5 mol/L, what is the pH at which Mg(OH)2 just begins to precipitate?
A. 3
B. 4
C. 11
D. 12

C. 11

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A solution of acetic acid whose analytical concentration was 0.100 M was found to have a hydrogen ion concentration of 1.32 E-3 M. Calculate the equilibrium constant for the dissociation of this acid.
A. 1.76 E-5
B. 2.01 E-4
C. 2.01 E-5
D. 1.76 E-4

A. 1.76 E-5

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A chemical compound is made up of
A. a mixture of compounds
B. noble gases bonded together
C. atoms with complete valence shells which are then bonded to become incomplete
D. two or more atoms joined through bonding

D. two or more atoms joined through bonding

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When two hydrogen atoms are brought together
A. the electrons, which are negative, attract each other
B. the positive electron of each atom repels the other atom
C. the negative electron of each atom is attracted by the positive nucleus of the other atom
D. the negative electron of each atom is attracted by the neutral nucleus of the other atom

C. the negative electron of each atom is attracted by the positive nucleus of the other atom

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In HCl, the chlorine attracts the electrons more than the hydrogen does largely because
A. chlorine has more electrons than hydrogen
B. chlorine has more protons in its nucleus than hydrogen does
C. chlorine has more neutrons in its nucleus than hydrogen does
D. HCl is polar covalent molecule

B. chlorine has more protons in its nucleus than hydrogen does

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ons are formed when
A. one or more electrons are shared
B. at least two nonpolar bond are created
C. electrons are transferred from one atom to another
D. neutral atoms are created

B. at least two nonpolar bond are created

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When an atom loses on or more electrons during oxidation
A. a cation is formed
B. an anion is formed
C. the atom always becomes neutral
D. the atom undergoes reduction

A. a cation is formed

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An ionic bond
A. forms when two atoms gain or lose a pair of electrons
B. results from oxidation
C. forms when two nonmetals chemically combine
D. results from the attraction between cations and anions

D. results from the attraction between cations and anions

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When magnesium and chlorine reacts, they form
A. Mg2Cl
B. Mg3Cl2
C. Mg2Cl3
D. MgCl2

D. MgCl2

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Which statement about a compound is true?
A. it consist of two or more distinct substances
B. it has no definite composition
C. its components cannot be physically separated
D. the properties of the individual components are retained

C. its components cannot be physically separated

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During a chemical reaction, there is a
A. conversion of mass to energy
B. loss of energy
C. change of energy from one form to another
D. gain of energy because all reactions give off hea

C. change of energy from one form to another

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When a state of equilibrium is reached
A. the rate of the forward reactions equals the rate of the reverse reaction
B. the forward and reverse reaction stops
C. the rate of the forward reaction is greater than the rate of the reverse reaction
D. the rate of the reverse reaction is greater than the rate of the forward reaction

A. the rate of the forward reactions equals the rate of the reverse reaction

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Which of the following is true of our understanding of the nature of the atom?
A. it has undergone little, but significant change and is now complete
B. it has undergone change and will likely continue to do so
C. it is just as the ancients originally described it
D. it has undergone such major changes it is returning to the ancient model

B. it has undergone change and will likely continue to do so

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Which of the following would not come from a radioactive source?
A. gamma rays
B. laser beam
C. alpha particles
D. high-speed electrons from nuclear decay

B. laser beam

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Which of the following radiation will be stopped by a piece of paper?
A. alpha
B. neutron
C. gamma ray
D. x-ray

A. alpha

Which rule or principle delineates the placement of additional electrons in the unfilled orbital of lowest energy?
A. Avogadro
B. Aufbau
C. Hund
D. Pauli

B. Aufbau

Spectral lines are produced
A. when electrons are knocked out of their energy level
B. when electrons interact with protons
C. when electrons move up to higher energy levels
D. when electrons return to their energy level

D. when electrons return to their energy level

Which of the following is not a source of the potential energy a substance has in a chemical reaction?
A. composition
B. mass number
C. structure
D. bond type

B. mass number

When a chemical bond is broken,
A. energy is absorbed
B. energy is released
C. there is no energy change
D. an exothermic reaction has occurred

A. energy is absorbed

Chemical change will occur if they lead to
A. bond formation
B. endothermia
C. exothermia
D. lower energy condition

A. bond formation

The transfer of electrons from one atom to another forms
A. isotopes
B. allotropes
C. ions
D. molecules

C. ions

Which of the following is not a way to express the formula of a compound
A. structural
B. molecular
C. empirical
D. metallic

D. metallic

Which of the following compounds always end in –ide?
A. binary
B. polyatomic
C. covalent
D. ionic

A. binary

Van der waals forces accounts for the formation of
A. water molecules
B. ionic solids
C. conjugate bases
D. liquid helium

D. liquid helium

The modern periodic table is based on
A. atomic radius
B. atomic mass
C. atomic number
D. atomic charge

C. atomic number

The properties of the atoms depend on their
A. mass
B. number
C. radius
D. structure

D. structure

The periods on the periodic table are represented by
A. columns
B. rows
C. metallic elements
D. inert gas members

B. rows

Metals tend to ____ electrons
A. lose
B. gain
C. share
D. combine

A. lose

Nonmetals tend to ____ electrons in combination with metals
A. lose
B. gain
C. share
D. combine

B. gain

Which if the following is not true of the metals?
A. have relative low ionization energies
B. usually have low electrical conductivity
C. are malleable
D. have high thermal conductivity

B. usually have low electrical conductivity

When an atom gains or loses electrons, it tends to
A. become chemically unstable
B. become neutral
C. increase its oxidation number
D. change its size

D. change its size

Nonmetals, in the solid phase, tend to
A. have the same size
B. conduct electricity
C. lack metallic luster
D. all of the above

C. lack metallic luster

Nonmetals do not generally
A. possess high ionization energy
B. gain electrons
C. have high electronegativities
D. tend to be malleable

Metalloids tend to have characteristics of
A. metals
B. nonmetals
C. both metals and nonmetals
D. inert gases

C. both metals and nonmetals

Elements within a group have
A. similar number of valence electron
B. the same number of energy levels
C. the same atomic radii
D. similar masses

A. similar number of valence electron

In the “A” groups, as the atomic number increases,
A. the electronegativity increases
B. the same number of energy levels
C. the atomic radius decreases
D. the elements tend to have fewer metallic propertie

B. the same number of energy levels

In each period, as the atomic number increases,
A. the raiuds of the atom increases
B. ther is a transition from negative to positive oxidation states
C. the electronegativity increases
D. the ionization energy decreases

C. the electronegativity increases

Sulfur is ____ oxygen
A. smaller than
B. less reactive than
C. equally as reactive as
D. an ion of

B. less reactive than

The type of chemical bond form between carbon and hydrogen in polymers
A. ionic
B. covalent
C. metallic
D. hydrogen

B. covalent

Which of the following is an acid found in milk?
A. lactic acid
B. tartaric acid
C. malic acid
D. citric acid

A. lactic acid

It is a substance that will slow down the speed of chemical reaction
A. catalyst
B. inhibitor
C. positive catalyst
D. substrate

B. inhibitor

A solution containing 25.3 mL of 0.1065 N HCl is added to one containing 92.2 mL of 0.2715 M H2SO4, and 50 mL of 1.00 N KOH are added. Is the solution acid or alkaline?
A. alkaline
B. cannot be determined
C. acid
D. none of the above

C. acid

How many milliliters of 6 M H2SO4 would be required to neutralize 100 mL of 3 M NaOH solution?
A. 25 mL
B. 40 mL
C. 50 mL
D. 75 mL

A. 25 mL

How many drops of 0.1 M HNO3 solution are required to neutralize 15 drops of 0.2 M Ba(OH)2 solution?
A. 40
B. 50
C.60
D. 70

C.60

What volume of 0.125 M H2SO4 is required to neutralize 2.50 g of Ca(OH)2 ?
A. 0.270 mL
B. 0.135 mL
C. 135 mL
D. 270 mL

D. 270 mL

A 0.5000 g sample of pure CaCO3 is dissolved in water to which 50.00 mL of HCl solution have been added. The solution then requires 6.20 mL of NaOH solution which 1.000 mL = 1.010 mL of the HCl. What is the normality of the HCl solutions?
A. 0.2307
B. 0.2284
C. 0.3125
D. 0.3540

B. 0.2284

What is the percentage of total acid expressed as acetic acid in sample of vinegar if 3.000 g of the vinegar require 20.50 mL of 0.1150 N KOH solution for an end point with phenolphthalein indicator?
A. 3.21%
B. 4.33%
C. 4.72%
D. 5.21%

C. 4.72%

In the analysis of a 2.00 g sample of lime by titration with H2SO4, what must be the normality of the acid so that the percentage of Ca may be found by dividing the net volume of the acid by 4?
A. 0.15 N
B. 0.20 N
C. 0.25 N
D. 0.30 N

C. 0.25 N

A mixture of Na2CO3 and BaCO3 weighing 0.2000 g requires 30.00 mL of 0.1000 N acid for complete neutralization. What is the percentage of Na2CO3 in the sample?
A. 55.7%
B. 44.3%
C. 50.5%
D. 49.5%

A. 55.7%

What weight of BaCO3 should be added to 1.000 g of Li2CO3 so that the mixture will require the same volume of standard acid for neutralization as would the same weight of CaCO3?
A. 0.714 g
B. 0.450 g
C. 1.005 g
D. 0.985 g

A. 0.714 g

A sample consisting of Na2CO3, NaOH and inert gas matter weighs 1.179 grams. It is titrated with 0.3000 N HCl with phenolphthalein as the indicator, and the solution became colorless after the addition of 48.16 mL. Methyl orange is then added and 24.08 mL more of the acid are needed for the color change. What is the percentage of Na2CO3 in the sample?
A. 24.51%
B. 64.95%
C. 4.06%
D. 76.15%

B. 64.95%

Nicotine is a compound that contains carbon, hydrogen and nitrogen. If a 2.50 g of a sample of nicotine is burned in oxygen 6.78 g of CO2, 1.94 g of H2O and 0.432 g of N2 are the products of combustion. What is the purity of the sample?
A. 99.87%
B. 98.20%
C. 95.2%
D. 89.90%

A. 99.87%

A 5.82 g silver coin is dissolved in nitric acid. When sodium chloride is added to the solution, all the silver precipitated as AgCl. The AgCl precipitate weighs 7.20 g. Determine the percentage of silver in the coin.
A. 90.5%
B. 91.2%
C. 92.3%
D. 93.1%

A. 90.5%

A sample of an oxide of lead (oxide A) weighing 4.7840 g is heated to drive off oxygen to form oxide B weighing 4.5704 g. Further heating at high temperature removes more oxygen to give oxide C weighing 4.4639 g and containing 92.8% of lead. The empirical formula of oxide A is
A. PbO
B. PbO2
C. Pb2O3
D. Pb3O4

B. PbO2

D. Pb3O4

A. PbO

A mixture contains Na2CO3, NaOH and inert matter. A sample weighing 1.500 g requires 28.85 mL of 0.5000 N HCl to reach a phenolphthalein end point, and an additional 23.85 mL to reach methyl orange end point. What is the percentage of NaOH in the sample?
A. 84.27%
B. 50.68%
C. 20.56%
D. 6.67%

D. 6.67%

What volume of 0.125 M H2SO4 solution is required to neutralize 25.21 mL of 0.540 M NaOH?
A. 109 mL
B. 54.4 mL
C. 5.84 mL
D. 11.7 mL

B. 54.4 mL

In standardizing a solution of HCl, it is found that 47.26 mL of the acetic acid are equivalent to 1.216 g of pure Na2CO3. What is the normality of the acid?
A. 0.4855 N
B. 0.3540 N
C. 0.5020 N
D. 0.3902 N

A. 0.4855 N

A metal with water the evolution of hydrogen and formation of its hydroxide. One gram atom of the metals was allowed to react completely with water. The hydroxide solution was made up to one liter. One hundred milliliters of this solution required 110 mL of 0.9091 N hydrochloric acid for neutralization. The chloride metal was found to contain 13.7% of chlorine. The volume of hydrogen gas liberated at S.T.P is
A. 22.4 L
B. 44.8 L
C. 11.2 L
D. 5.6 L

C. 11.2 L

A metal with water the evolution of hydrogen and formation of its hydroxide. One gram atom of the metals was allowed to react completely with water. The hydroxide solution was made up to one liter. One hundred milliliters of this solution required 110 mL of 0.9091 N hydrochloric acid for neutralization. The chloride metal was found to contain 13.7% of chlorine. The atomic weight of the metals is
A. 297
B. 197
C. 224
D. 226

C. 224

A metal with water the evolution of hydrogen and formation of its hydroxide. One gram atom of the metals was allowed to react completely with water. The hydroxide solution was made up to one liter. One hundred milliliters of this solution required 110 mL of 0.9091 N hydrochloric acid for neutralization. The chloride metal was found to contain 13.7% of chlorine. Since the solution of the hydroxide of the metal is normal, the valency of the metal is
A. 1
B. 2
C. 3
D. 4

A. 1

A 15.10 g sample of an unstable hydrated salt, Na2SO4-xH2O, was found to contain 7.05 g of water. Determine the empirical formula of the salt.
A. Na2SO4-3H2O
B. Na2SO4-4H2O
C. Na2SO4-6H2O
D. Na2SO4-7H2O

D. Na2SO4-7H2O

A taconite ore consisted of 35% Fe3O4 and the balance siliceous impurities. How many tons of the ore must be processed in order to recover one tone of metallic iron?
A. 3.75
B. 3.95
C. 4.15
D. 4.45

B. 3.95

A sample of poly styrene prepared by heating styrerne with tribromobenzoyl peroxide in the absence of air has the formula Br3C6H3(C8H8)N. the number n varies with the conditions of preparation. One sample of polystyrene prepared in this manner was found to contain 10.46% bromine. What is the v alue of N?
A. 19
B. 18
C. 17
D. 16

A. 19

Calculate the percentage of CaO in CaCO3.
A. 42.7%
B. 45.6%
C. 52.0%
D. 56.0%

D. 56.0%

How many milliliters of 0.1000 N Ba(OH)2 are theoretically required to titrate 0.3000 g of H3AsO4 to the formation of Ba(H2AsO4)2?
A. 16.4 mL
B. 17.6 mL
C. 18.9 mL
D. 21.14 mL

D. 21.14 mL

What is the normality of a solution of KOH if 45.18 mL are required to neutralize 0.300 g of pure oxalic acid (H2C2O4H2O)?
A. 0.1053
B. 0.1153
C. 0.2135
D. 0.3125

A. 0.1053

Calculate the alkaline strength of pearl ash(impure potassium carbonate) in terms of percent K2O from the following date: Sample=0.3500 g; HCl used=48.03 mL; NaOH used for back titration=2.02 mL; 1.000 mL HCl=0.005300 g Na2CO3; 1.000 mL NaOH=0.02192 g KHC2O4 H2O
A. 45.2%
B. 54.0%
C. 60.5%
D. 65.8%

C. 60.5%

What weight of a sample of impure oxalic acid should be taken for titration by 0.5000 N NaOH so that the percentage of H2C2O4 - 2H2O will be twice the burette reading?
A. 1.576 g
B. 1.892 g
C. 2.007 g
D. 2.280 g

A. 1.576 g

What volume of a 1 M solution of hydrochloric acid is required to neutralize 80 mL of 0.5 M NaOH solution?
A. 320 mL
B. 160 mL
C. 80 mL
D. 40 mL

D. 40 mL

How many mL of 0.200 M NaOH will completely neutralize 100 mL of 0.250 M H2SO4?
A. 125
B. 175
C. 225
D. 250

D. 250

When 50 mL of a nitric acid solution was titrated with 0.334 M NaOH, it required 42.80 mL of the base to achieve the equivalence point. What is the molarity of the nitric acid solution?
A. 0.286
B. 0.826
C. 0.682
D. 0.628

A. 0.286

A 0.250 g sample of solid acid was dissolved in water and exactly neutralized by 40.0 mL of 0.125 N base. What is the equivalence weight of the acid?
A. 40
B. 44
C. 48
D. 50

D. 50

A 48.4 mL sample of HCl solution requires 1.240 g of pure CaCO3 for complete neutralization. Calculate the normality of the acid.
A. 0.512
B. 0.476
C. 0.412
D. 0.386

A. 0.512

A 25 mL sample of 0.025 M HBr is mixed with 25.0 mL of 0.023 M KOH. What is the pH of the resulting mixture?
A. 1.00
B. 3.00
C. 7.00
D. 11.00

B. 3.00

A student is titrating 50 mL of 0.2 N HCl solution with a solution of 0.2 N KOH. He accidentally adds one mL too much titrant. What is the pH of the resulting solution?
A. 10.3
B. 11.3
C. 2.7
D. 7.3

B. 11.3

A sample of impure sulfide ore contains 42.43% Zn. Find the percentage of the pure ZnS in the sample.
A. 67.10%
B. 63.10%
C. 56.05%
D. 52.15%

B. 63.10%

A sample of impure cuprite Cu2O contains 66.6% copper. What is the percentage of pure Cu2O in the sample?
A. 45%
B. 55%
C. 65%
D. 75%

D. 75%

The “roasting” of 100 g of a copper ore yielded 75.4 g of 89.5% pure copper. If the ore composed of Cu2S and CuS with 11.0% inert impurity, calculate the percent of Cu2S in the ore.
A. 62%
B. 38%
C. 74%
D. 28%

A. 62%

A 1.2048 g sample of impure NaCO3 is dissolved and allowed to react with a solution of CaCl2. The resulting CaCO3, after precipitation, filtration, and drying, was found to weight 1.0362 g. Assuming that the impurities do not contribute to the weight of the precipitate, calculate the percent purity of the Na2CO3.
A. 86.2%
B. 88.9%
C. 91.1%
D. 93.2%

C. 91.1%

Hydrogen peroxide maybe oxidized to O2 or it may be reduced to H2O. Which of the following represents the milliequivalent weight of H2O2 as an oxidizing agent and as a reducing agent?
A. 0.03402
B. 0.01134
C. 0.00851
D. 0.01701

D. 0.01701

A solid metallic element burns in oxygen to produce an oxide which dissolves in water to give the hydroxide of the metal. The hydroxide obtained from 1 gram of metal neutralizes 111.2 mL of normal hydrochloric acid. The specific heat of the metal is 0.228 cal/g-ºC. What is the valency of the metal?
A. 1
B. 2
C. 3
D. 4

C. 3

B. 8.992

Calculate the normality of NaOH if 10 mL of NaOH reacts with 20 mL of 0.4 M sulfuric acid.
A. 1.6 N
B. 0.8 N
C. 2.6 N
D. 3.2 N

A. 1.6 N

A. 1.576 g

What volume of a 1 M solution of hydrochloric acid is required to neutralize 80 mL of 0.5 M NaOH solution?
A. 320 mL
B. 160 mL
C. 80 mL
D. 40 mL

D. 40 mL

What volume of 0.0224 N adipic acid solution would be used in the titration of 1.022 cm3 of 0.0317 N Ba(OH)2?
A. 1.20 mL
B. 1.45 mL
C. 2.05 mL
D. 3.60 mL

B. 1.45 mL

What is the equivalent weight of an acid 1.243 g of which required 31.72 cm3 of 0.1923 N standard base for neutralization?
A. 180
B. 194
C. 204
D. 210

C. 204

What volume of 0.115 M HClO4 solution is required to neutralize 50.00 mL of 0.0875 M NaOH?
A. 0.115 mL
B. 38.0 L
C. 38.0 mL
D. 50.0 mL

C. 38.0 mL

What volume of 0.128 M HCl is required to neutralize 2.87 g of Mg(OH)2?
A. 0.0126 L
B. 0.385 L
C. 0.769 L
D. 22.4 L

C. 0.769 L

Tartaric acid (H2C4H4O6), has two acidic hydrogens. The acid is often present in wines and precipitates from solution as the wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 22.62 mL of 2.000 M NaOH solution to titrate both acidic protons in 40.00 mL of tartaric acid solution. Calculate the molarity of the tartaric acid.
A. 0.02262 M
B. 0.04524 M
C. 0.5655 M
D. 1.131 M

C. 0.5655 M

Mayonnaise and milk are examples of
A. emulsion
B. suspension
C. colloid
D. mixture

C. colloid

Which of the following units represents the largest amount of energy?
A. calorie
B. joule
C. erg
D. electron-volt

A. calorie

Whose rule or principle delineates the placement of additional electron in the unfilled orbital of lowest energy?
A. Avogadro
B. Aufbau
C. Hund
D. Paul

B. Aufbau

An exothermic reaction is one which
A. takes place only on heating
B. is accompanied by absorption of heat
C. is accompanied by a flame
D. is accompanied by evolution of heat

D. is accompanied by evolution of heat

An element obtained commercially from sea water and salt brines is
A. aluminum
B. beryllium
C. potassium
D. magnesium

D. magnesium

The major problem in exploiting nuclear fusion as an energy source is
A. the high radioactivity of reactants
B. the high radioactivity of the products
C. the lack of appropriate reactants
D. the high activation energy that is required for the reaction

D. the high activation energy that is required for the reaction

Which of the following is not a normal characteristic of a metal?
A. conduction of electricity
B. low electron affinity
C. malleability
D. high ionization energy

D. high ionization energy

An amphoteric substance
A. can be dissolved by an acid
B. reacts with both an acid and a base
C. can be neutralized by an acid
D. is insoluble in a base but dissolved in an acid

B. reacts with both an acid and a base

The electrolysis of water yields
A. equal volumes of hydrogen and oxygen
B. equal masses of hydrogen and oxygen
C. two volumes of hydrogen for each volume
D. twice the mass of hydrogen as of oxygen

B. equal masses of hydrogen and oxygen

The quantity known as specific heat is
A. any temperature reported on the more specific absolute temperature scale
B. the energy needed to increase the temperature of 1 gram of a substance by 1 degree Celsius
C. any temperature of a 1 kg sample reported in degrees Celsius
D. the heat needed to increase the temperature of any size sample by 1 degree Celsius

A. any temperature reported on the more specific absolute temperature scale

The heat transfer that takes place by energy moving directly from molecule is called
A. conduction
B. convection
C. radiation
D. none of these

C. radiation

The heat transfer that does not require matter is
A. conduction
B. convection
C. radiation
D. impossible, for matter is always required

Styrofoam is a good insulating material because
A. it is plastic material that conducts heat poorly
B. it contains many tiny pockets of air
C. of the structure of the molecules making up it
D. it is not very dense

A. it is plastic material that conducts heat poorly

The transfer of heat that takes place because of density difference in fluids is
A. conduction
B. convection
C. radiation
D. none of these

B. convection

When a solid, liquid, or gas changes from one physical state to another, the change is called
A. melting
B. entropy
C. a phase change
D. sublimation

C. a phase change

Latent heat is “hidden” because it
A. goes into or comes out of internal potential energy
B. is a fluid (caloric) that cannot be sensed
C. does not actually exist
D. is form of internal kinetic energy

D. is form of internal kinetic energy

As a solid undergoes a phase change to a liquid state, it
A. releases heat while remaining at a constant temperature
B. absorbs heat while remaining at constant temperature
C. releases heat as the temperature decreases
D. absorbs heat as the temperature increases

B. absorbs heat while remaining at constant temperature

The condensation of water vapor actually
A. warms the surroundings
B. cools the surroundings
C. sometimes warms and sometimes cools the surroundings
D. neither warms nor cools the surroundings

A. warms the surroundings

A wave is
A. the movement of material from one place to another place
B. a travelling disturbance that carries energy
C. a wavy line that moves through materials
D. all of the above

D. all of the above

A longitudinal mechanical wave causes particles of a material to move
A. back and forth in the same direction the wave is moving
B. perpendicular to the direction the wave is moving
C. in a circular motion in the direction the wave is moving
D. In a circular motion opposite the direction the wave is moving

A. back and forth in the same direction the wave is moving

A transverse mechanical wave causes particles of a material to move
A. back and forth in the same direction the wave is moving
B. perpendicular to the direction the wave is moving
C. in a circular motion in the direction the wave is moving
D. In a circular motion opposite the direction the wave is moving

B. perpendicular to the direction the wave is moving

Transverse mechanical waves will move only through
A. solids
B. liquids
C. gases
D. all of these

D. all of these

Longitudinal mechanical waves will move only through
A. solids
B. liquids
C. gases
D. all of these

D. all of these

The sky appears to be blue when the sun is in the sky because
A. blue is the color of air, water, and other fluids in large amounts
B. red light is scattered more than blue
C. blue light more than the other colors
D. none of the above

C. blue light more than the other colors

The photoelectric effect proved to be a problem for a wave model of light because
A. the number of electrons ejected varied directly with the intensity of light
B. the light intensity had no effect on the energy of the ejected electrons
C. the energy of the ejected electrons varied inversely with the intensity of light
D. the energy of the ejected electrons varied directly with the intensity of light

B. the light intensity had no effect on the energy of the ejected electrons

Max Planck made the revolutionary discovery that the energy of vibrating molecules involved in blackbody radiation existed only in
A. multiples of certain amounts
B. amounts that smoothly graded one into next
C. the same, constant amount of energy in all situations
D. amounts that were never consistent from one experiment to the next

A. multiples of certain amounts

Einstein applied Planck’s quantum discovery to light and found
A. a direct relationship between the energy and frequency of light
B. that the energy of a photon divided by the frequency of the photon always equaled a constant known as Planck’s constant
C. that the energy of a photon divided by the Planck’s constant always equaled the frequency
D. all of the above

D. all of the above

Today, light is considered to be
A. tiny particles of matter that move through space, having no wave properties
B. electromagnetic waves only, with properties of particle
C. a small-scale phenomenon without a sharp distinction between particle and wave properties
D. something that is completely unknown

C. a small-scale phenomenon without a sharp distinction between particle and wave properties

The electron was discovered through experiments with
A. radioactivity
B. light
C. matter waves
D. electricity

B. light

Thomson was convinced that he had discovered a subatomic particle, the electron, from the evidence that
A. the charge-to-mass ratio was the same for all materials
B. cathode rays could move through a vacuum
C. electrons were attached towards a negatively charge plate
D. the charge was always 1.60 E-19 coulomb

A. the charge-to-mass ratio was the same for all materials

The existence of a tiny, massive, and positively charged nucleus was deduced from the observation that
A. fast, massive and positively charged alpha particles all move straight through the metal foil
B. alpha particles were deflected by a magnetic field
C. some alpha particles were deflected by the metal foil
D. none of the above

A. fast, massive and positively charged alpha particles all move straight through the metal foil

According to the Rutherford’s calculations the volume of an atom is mostly
A. occupied by neutrons and protons
B. filled with electrons
C. occupied by tightly bound protons, electrons, and neutrons
D. empty space

D. empty space

The main problem with solar system model of the atom is that
A. electrons move in circular, not elliptical orbit
B. the electrons should lose energy since they are accelerating
C. opposite charges should attract one another
D. the mass ratio of the nucleus to the electron is wrong

B. the electrons should lose energy since they are accelerating

The energy of a photon
A. varies inversely with the frequency
B. varies directly with velocity, not frequency
C. is directly proportional to the frequency
D. is inversely proportional to the velocity

C. is directly proportional to the frequency

The lines of color in a line spectrum from a given element
A. change colors with changes in the temperature
B. are always the same, with a regular spacing pattern
C. are randomly spaced, having no particular pattern
D. have the same colors, with a spacing pattern that varies with temperature

B. are always the same, with a regular spacing pattern

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