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Chem > Unit 5-Solubility > Flashcards

Unit 5-Solubility Flashcards

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1
Q

1. Which statement is false

A. carbon dioxide is a major component(by volume)is a solution of air
B. an unsaturated solution will have Qsp<Ksp
C. an alloy consists of two or more solid elements
D. Ksp depends on temperature
E. Polar solutions tend to dissolve in polar solvents

A

A

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2
Q

2. Sugar is an example of a

A. strong electrolyte
B. weak electrolyte
C. nonelectrolyte

A

C

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3
Q
  1. Spectator ions are explicitly written in the

A. complete ionic equation
B. net ionic equation
C. molecular equation
D. neutralization equation

A

A

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4
Q
  1. For a saturated solution, which statement is true?
    A. All dissolving has stopped.
    B. A rapid temperature changes occurs.
    C. An equilibrium has been established.
    D. The solute is exceeding its solubility.
    E. The entropy of the system is continually decreasing.
A

C

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5
Q
  1. When a seed crystal was added to an unstable solution, the crystal seemed to grow in size immediately. In what condition was the solution just before the seed crystal was added ?
    A. concentrated B.saturated C. unsaturated D. supersaturated
A

D

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6
Q
  1. Potassium Carbonate is an example of a
    A. strong electrolyte B. weak electrolyte C. nonelectrolyte
A

A

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7
Q
  1. For the majority of ionic solids, as temperature increases, solubility in water
    A. increases
    B. decreases
    C. remains constant
A

A

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8
Q
  1. For the majority of inorganic gases, at a fixed pressure, as temperature increases, olubility in water
    A. increases B. decreases C. remains constant
A

B

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9
Q

As the pressure exerted on an aqueous solution ecreases, the solubility of a gas in that solution usually
A. increases
B. decreases
C. remains constant

A

B

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10
Q
  1. Which of the following sets of units is not commonly used to describe solubility:
    A. grams of solute/ 100 grams of water
    B. grams of solute/ 100mL of water
    C. moles of solute/ L of solution
    D. grams of solute/100 cm3 of solution
    E. grams of solute/ moles of water
A

A

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11
Q

At 15C, ionic compound AB has a solubility of 0.0035 moles of AB/100 grams of water and ionic compond CD has a solubility of 0.0018 moles of CD/ 100 grams of water. Which of the following statements is true?
A. At 15C, Ksp(AB) is greater than Ksp(CD)
B. At 15C, Ksp(AB) is less than Ksp(CD)
C. At 15C Ksp(AB) equals Ksp(CD)
D. Not enough information is given to compare the two solubility product constants.

A

A

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12
Q
  1. At 23C, the solubility of potassium Chlorate in water is 7.4g KCIO3/ 100g of H2O. How many grams of KCIO3 must be dissolved in 0.5kg of H2O tome saturated solution?
    A. 3.7
    B. 0.3
    C. 14.8
    D. 37.0
    E. 1.5
A

D

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13
Q
  1. Qualitatively, at 25C which of the following ionic compounds is MOST soluble in water?
    A.BaSO4
    B. PbSO4
    C. MgSO4
A

B

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14
Q

Qualitatively, at 25C, which of the following ionic compounds is the LEAST soluble in water?
A. naI
B. MgI2
C. KI
D. CdI2
E. AgI

A

E

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15
Q
  1. At 28C, kSP(AgF)=1.9x10^-10. What is the molar concentration of F- (aq) in a one litre saturated solution of silver fluoride at the temperature?
    A. 0.44X10^-5
    B. 0.95X10^-5
    C. 1.38X10^-5
    D. 0.95X10^-10
    E. 3.81X10^-10
A

C

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16
Q
  1. The Ksp for MgS is 3.6x10^-29 at 18C. The concentration of magnesium cation in a saturated solution of MgS at this temperature, in moles per litre, is
    A. 3.6x10^-39
    B. 1.4x10^-5
    C. 1.4x10^-6
    D. 6.0x10^-15
    E. 6.0x10^-14
A

D

17
Q
  1. The solubility of PbF2 IS 0.49g/L of H2O at 18C. What is the Ksp for lead fluoride at this temperature? (molar mass of PbF2 is 245.2 g/mole)
    A. 0.002
    B. 4.0x10^-6
    C. 8.0x10^-6
    D. 7.5x10^-7
    E. 3.2x10^-8
A

E

18
Q
  1. A saturated solution of barium sulphate at 27C contains 3.9x10^-5 M Ba2+ ions. What is the Ksp of this salt at this temperature?
    A. 3.9X10^-5
    B. 3.9X10^-6
    C. 2.1X10^-7
    D. 1.5x10^-8
    E. 1.5x10^-9
A

E

19
Q
  1. If one-tenth of a mole of sodium sulphate was added to the solution described in question 18. What would happen to the barium ion concentration?
    A. increase
    B. decrease
    C. remain the same
A

B

20
Q
  1. At room temperature, 10mL of 0.01 M Na2S and 10mL of 0.01 M AgNO3 are poured together. What event is most likely to occur?
    A. NaNO3 will precipitate out of solution
    B. Ag2S will precipitate out of solution
    C. hydrogen gas will be evolved
    D. AgS will precipitate out of solution
    E. NaAg will precipitate out of solution
A

B

21
Q
  1. At 20C, the solubility of AgCl is BLANK in the presence of solution of AgNO3 than it is in pure water.
    A. greater
    B. less
    C. the same
A

B

22
Q
  1. What does the sp stand for in Ksp.
    A. special
    B. solubility product
    C. solubility pair
    D. solubility process
    E. solubility precipitate
A

B

23
Q
  1. A 1:1 sparingly soluble salt has Ksp=9x10^-9. The solubility (in mol/litre) of the salt is closest to the value.
    A. 3x10^-3
    B. 1.8x10^-8
    C. 9.5x10^-5
    D. 8.1x10^-17
A

C

24
Q
  1. In general, ionic solids containing ions of which group will likely to be the most soluble?
    A. coinage metals
    B. alkali metals
    C. chalcogens
    D. halogens
    E. alkaline-earth metals
A

B

25
Q

If sparingly soluble salt has a molar mass of 2000g/mol and a solubility of 0.005 moles/ L of solution, calculate its solubility in grams/ 100mL of solution.
A. 2x10^4
B. 1
C. 5x10^-5
D. 0.1
E. 10

A

D

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