Acids and Bases Flashcards
1
Q
Has a sour taste, neutralizes bases, and produces H+ ions in water.
A
Acid.
2
Q
Has a bitter or chalky taste, neutralizes acids, and produces OH- ions in water.
A
Base.
3
Q
True or False:
Both acids and bases are electrolytes.
A
True.
4
Q
HCl.
A
Hydrochloric acid.
5
Q
H2SO4.
A
Sulfuric acid.
6
Q
H2SO3.
A
Sulfurous acid.
7
Q
H2CO3.
A
Carbonic acid.
8
Q
HBr.
A
Hydrobromic acid.
9
Q
What is the correct formula for ammonium hydroxide?
A
NH4OH.
10
Q
Which statement concerning
Arrhenius acid-base theory is not correct?
A) All of these are correct.
B) An acid produces H+ ions in water.
C) A neutralization reaction produces water and a salt.
D) A base produces OH- ions in water.
A
A) All of these are correct.
11
Q
What is the conjugate base of HSO4-?
A
SO42-.
12
Q
What is the conjugate acid of HSO4-?
A
H2SO4.
13
Q
What is the conjugate acid of H2PO4-?
A
H3PO4.
14
Q
What is the conjugate base of H2PO4-?
A
HPO42-.
15
Q
Why is water the most common acid and base in the world?
A
It is very good at donating and accepting protons.
16
Q
True or False:
Bronsted-Lowry bases donate protons.
A
False.
They accept protons.
17
Q
When HCl is dissolved in water, the resulting products are:
A
H3O+ and Cl–.
18
Q
Which acid is responsible for reacting with limestone and eating away statues and buildings?
A
Sulfuric acid.
19
Q
Use the information below to determine which one of the following weak
acids is the strongest.
HCN (Ka = 4.9 × 10^-10)
HClO (Ka = 3.0 × 10^-8)
HNO2 (Ka = 4.5 × 10^-4)
HF (Ka = 6.8 × 10^-5)
A
HNO2 (Ka = 4.5 × 10^-4)
Ka values closer to 1 are stronger acids.
20
Q
Use the information below to determine which one of the following weak
acids is the weakest.
HCN (Ka = 4.9 × 10^-10)
HClO (Ka = 3.0 × 10^-8)
HNO2 (Ka = 4.5 × 10^-4)
HF (Ka = 6.8 × 10^-5)
A
HCN (Ka = 4.9 × 10^-10).
Weak acids have values farther away from 1.
21
Q
Use the information below to determine which of the following weak
acids has the strongest conjugate base.
HCN (Ka = 4.9 × 10^-10)
HClO (Ka = 3.0 × 10^-8)
HNO2 (Ka = 4.5 × 10^-4)
HF (Ka = 6.8 × 10^-5)
A
HCN (Ka = 4.9 × 10^-10).
The weakest acids have the strongest conjugate bases.
22
Q
Use the information below to determine which of the following weak
acids has the weakest conjugate base.
HCN (Ka = 4.9 × 10^-10)
HClO (Ka = 3.0 × 10^-8)
HNO2 (Ka = 4.5 × 10^-4)
HF (Ka = 6.8 × 10^-5)
A
HNO2 (Ka = 4.5 × 10^-4).
The strongest weak acid will have the weakest conjugate base.
23
Q
Match each solution below with whether it is acidic, basic or neutral:
- [H3O+] = 1.4 x 10^-9 M.
- [H3O+] = 2.0 x 10^-5 M.
- [H3O+] = 1.0 x 10^-7 M.
A
- Basic (because H3O+ is more than 10^7).
- Acidic (because H3O+ is less than 10^7).
- Neutral (because H3O+ = 10^7).
24
Q
Match each solution below with whether it is acidic, basic or neutral:
- [OH–] = 8.0 x 10^-3 M.
- [OH–] = 1.0 x 10^-7 M.
- [OH–] = 3.5 x 10^-10 M.
A
- Basic (because OH- is less than 10^7).
- Neutral (because OH- = 10^7).
- Acidic (because OH- is more than 10^7).
25
Vinegar has a [OH-] = 1.0 x 10^-11M. Calculate the [H3O+] of vinegar (assuming an aqueous solution).
[H3O+] = 1.0 x 10^-3 M.
26
Urine has a [OH-] = 2.0 x 10^-9M. Calculate the [H3O+] of urine (assuming an aqueous solution).
[H3O+] = 5.0 x 10^-6 M.
27
Ammonia has a [OH-] = 5.6 x 10^-3M. Calculate the [H3O+] of ammonia (assuming an aqueous solution).
[H3O+] = 1.8 x 10^-12 M.
28
Coffee has a [H3O+] = 1.0 x 10^-5 M. Calculate the [OH-] of coffee (assuming an aqueous solution).
[OH-] = 1.0 x 10^-9 M.
29
Soap has a [H3O+] = 1.0 x 10^-8 M. Calculate the [OH-] of soap (assuming an aqueous solution).
[OH-] = 1.0 x 10^-6 M.
30
Lemon juice has a [H3O+] = 2.5 x 10^-2 M. Calculate the [OH-] of lemon juice (assuming an aqueous solution).
[OH-] = 4.0 x 10^-13 M.
31
Match each solution below with whether it is acidic or basic:
1. Blood, pH = 7.38
2. Vinegar, pH = 2.8
1. Basic
2. Acidic
32
Match the given [H3O+] or [OH-] with the correct corresponding pH for that solution.
1. [H3O+] = 1 x 10^-4 M
2. [H3O+] = 3 x 10-9 M
3. [OH-] = 1 x 10-5 M
1. pH = 4.0
2. pH = 8.5
3. pH = 9.0
33
Find the the pH from the given [H3O+] or [OH-] for that solution.
1. [OH-] = 2.5 x 10-11M
2. [H3O+] = 6.7 x 10-8 M
3. [OH-] = 8.2 x 10-4 M
1. pH = 3.40
2. pH = 7.17
3. pH = 10.92
34
Calculate the hydrogen ion
concentration in a solution with pH = 6.35.
4.5 × 10-7 M.
35
Calculate the hydroxide ion concentration in a solution with pH = 6.35.
2.2 × 10-8 M.
36
What is the value of [H3O+] in a
solution with pH = 10.82?
1.5 × 10-11 M.
37
What is the value of [OH-] in a
solution with pH = 10.82?
6.7 × 10-4 M.
38
Urine has a [OH-] = 2.0 x 10-9M. Calculate the pH of urine (assuming an aqueous solution).
pH - 5.3
39
What is the hydrogen ion concentration
in a solution with pH = 2.34?
[H+] = 10^ -pH
4.6 x 10-3 M.
40
What is the hydroxide ion concentration
in a solution with pH = 2.34?
2.2 x 10-12 M.
41
What is the normality of a solution
containing 49 g of H2SO4 in enough water to make 400 mL of solution?
N = moles x acid or base # of ions/ liters of solution
2.5 N
42
What is the normality of a solution
containing 100 g HNO3 in 500 mL of solution?
3.17 N.
43
What is the normality of a solution
prepared by dissolving 37.5 g citric acid, a triprotic acid with molar mass of
192.14 g/mol, in water to make 250 mL solution?
2.34 N.
44
Which equation provides the correct balancing and products of the following:
ZnCO3 + HBr →
ZnCO3 + 2HBr → CO2 + H2O + ZnBr2
45
Which equation provides the correct balancing and products of the following:
Zn + HCl →
Zn + 2HCl → H2 + ZnCl2
46
Which equation provides the correct balancing and products of the following:
HCl + NaHCO3 →
HCl + NaHCO3 → CO2 + H2O + NaCl
47
Which equation provides the correct balancing and products of the following:
H2SO4 + Mg(OH)2 →
H2SO4 + Mg(OH)2 → 2H2O + MgSO4
48
Which is the correct balanced equation for the following neutralization reaction:
HCl + Mg(OH)2 → H2O + MgCl2
2HCl + Mg(OH)2 → 2H2O + MgCl2
49
Which is the correct balanced equation for the following neutralization reaction:
H3PO4 + LiOH → H2O + Li3PO4
H3PO4 + 3LiOH → 3H2O + Li3PO4
50
Which is the correct neutralization reaction for H2SO4 and NaOH?
H2SO4 + 2NaOH → 2H2O + Na2SO4
51
Which is the correct neutralization reaction for HCl and Fe(OH)3?
3HCl + Fe(OH)3 → 3H2O + FeCl3
52
Which is the correct neutralization reaction for H2CO3 and Mg(OH)2?
H2CO3 + Mg(OH)2 → 2H2O + MgCO3
53
What is the resulting molarity of an HCl solution if 5.00 mL is titrated with 28.6 mL of a 0.145 M NaOH solution?
0.830 M HCl solution
54
If 38.2 mL of a 0.163 M KOH solution is required to titrate 25.0 mL of a solution of H2SO4, what is the molarity of the H2SO4 solution?
H2SO4 + 2KOH → 2H2O + K2SO4
0.124 M H2SO4 solution
55
What defines a salt?
An ionic compound composed of the cation from the base and the anion from the acid.
56
Of the following four substances,
which would form a basic solution when dissolved in water:
1) NH4Cl
2) Cu(NO3)2
3) K2CO3
4) NaF
3 and 4.
57
True or False:
The following represents a buffer system: NaOH and NaCl.
False.
A buffer system is a weak acid and its conjugate base.
58
True or False:
The following represents a buffer system: H2CO3 and NaHCO3.
True.
59
True or False:
The following represents a buffer system: HF and KF.
True.
60
True or False: The following represents a buffer system: KCl and NaCl.
False.
61
Consider the buffer system of HF and its salt, NaF:
HF + H2O → H3O+ + F–
The purpose of this buffer system is to:
Maintain pH.
62
Consider the buffer system of HF and its salt, NaF:
HF + H2O → H3O+ + F–
The salt of the weak acid is needed to:
Provide the conjugate base and neutralize added H3O+.
63
Consider the buffer system of HF and its salt, NaF:
HF + H2O → H3O+ + F–
if OH- is added, it is neutralized by:
H3O+.
64
Consider the buffer system of HF and its salt, NaF:
HF + H2O → H3O+ + F–
when H3O+ is added, equilibrium shifts in the direction of the:
Reactants.
65
Why is the following solutions
a buffer?
a solution of acetic acid and sodium acetate
It has an acid and the conjugate base.
66
All of the following species are
involved in the blood buffer system except:
1. CO2
2. CO32-
3. They are all involved in the blood buffer system
4. H2CO3
They are all involved in the blood buffer system.
67
What is the concentration of an
acetic acid solution if a 10.0 mL sample required 26.4 mL of 0.950 M KOH for
neutralization?
2.51 M.
68
How many mL of 0.150 M NaOH are
needed to neutralize 50.00 mL of a 0.120 M solution of H2SO4?
80.0 mL.
69
How many mL of 0.241 M H2SO4 will be needed to neutralize a 50.0 mL sample
of 0.191 M KOH?
19.80 mL.
70
How many mL of 0.360 M HNO3 are needed to neutralize a 22.5 mL sample of
0.240 M KOH?
15.0 mL.
71
How many mL of 0.100 M NaOH are
needed to neutralize 50.00 mL of a 0.150 M solution of CH3CO2H, a
monoprotic acid?
75.00 mL.
72
The treatment for leukemia often includes the use of a radioisotope that contains 17 neutrons and has a mass number of 32. What is the chemical symbol for this radioisotope?
32/15 P.
73
When a patient receives a brain scan (used to diagnose brain tumors and aneurysms) , a radioisotope which contains 43 protons and 56 neutrons is used. Which element does this represent?
99/43 Tc.
74
One of the radioisotopes used in the treatment of cancer is 131/55 Cs. Which of the following statements about this radioisotope is NOT correct:
1. It has 55 neutrons.
2. It has an atomic number of 55.
3. It is the element cesium.
4. It has 55 electrons.
1. It has 55 neutrons.
It has 76 neutrons.
75
State each particles correct name:
1. 4/2 He.
2. 0/+1 Y.
3. 0/0 Y.
1. Alpha rays.
2. Positron.
3. Gamma rays.
76
Match the following statements with the type of rays:
1. Does not penetrate skin.
2. A neutron changes to a proton and an electron is emitted.
3. Shielding requires lead or thick concrete
1. Alpha particle.
2. Beta particle.
3. Gamma radiation.
77
Dr. Marie Curie's nationality is:
Polish.
78
Which 2 elements on the periodic table did Marie and Pierre Curie discover?
Polonium and radium.
79
True or False:
All of Marie Curie's belongings to this day must be stored in lead because they remain radioactive.
True.
80
Where was Marie Curie the first female professor?
She held the first female professorship at Sorbonne University in Paris.
81
True or False:
There are more stable than unstable isotopes in existence.
False.
82
True or False:
All elements beyond bismuth (#83) are radioactive.
True.
83
True or False:
Hydrogen has 3 known isotopes, but only 1 is stable.
False.
2/3 are stable.
84
Write a balanced nuclear reaction for the alpha decay of 208/84 Po.
208/84 Po → 204/82 Pb + 4/2 He.
85
Write a balanced nuclear reaction for the alpha decay of 232/90 Th.
232/90 Th → 228/88 Ra + 4/2 He.
Radium because it loses 2 protons. Protons = atomic number.
86
Write a balanced nuclear reaction for the beta decay of 20/8 O.
20/8 O → 20/9 F + 0/-1 e.
87
Write a balanced nuclear reaction for the beta decay of 92/38 Sr.
92/38 Sr → 92/39 Y + 0/-1 e.
88
Write a balanced nuclear reaction for the positron emission of 54/27 Co.
54/27 Co → 54/26 Fe + 0/+1 e.
89
Write a balanced nuclear reaction for the positron emission of 93/45 Rh.
93/45 Rh → 93/44 Ru + 0/+1 e.
90
Strontium-85, used for bone scans, has a half-life of 65 days. How long would it take for the radiation level of strontium-85 to drop to one quarter of its original level?
130 days.
91
Strontium-85, used for bone scans, has a half-life of 65 days. How long would it take for the radiation level of strontium-85 to drop to one eighth of its original level?
195 days.
92
Indicate the number of half-lives that have elapsed for the following statements:
1. Pb-103 with a half-life of 17 days, after 34 days.
2. C-11 with a half-life of 20 mins, after 20 mins.
3. At-211 with a half-life of 7 h, after 21 h.
1. 2 half-lives.
2. 1 half-life.
3. 3 half-lives.
93
Technetium-99 is an ideal radioisotope for scanning organs because it has a half-life of 6 h and is a pure gamma emitter. A lab technician prepared 80.0 mg of this radioisotope to use on patients for today. How many mg of technetium-99 would remain after 24h?
5.00 mg.
94
Technetium-99 is an ideal radioisotope for scanning organs because it has a half-life of 6 h and is a pure gamma emitter.
A lab technician prepared 80.0 mg of this radioisotope to use on patients for today. How many mg of technetium-99 would remain after 18 h?
10 mg.
95
Fluorine-18, which has a half-life of 110 mins, is used in PET scans. If 100.0 mg of F-18 is shipped at 8AM, how many mg of the sample are still active when the shipment arrives at the lab at 1:30PM.
12.5 mg.
96
Phosphorus-32, a radioisotope used in the treatment of leukemia, has a half-life of 14 days. How much of a sample of P-32 would remain after 3 months?
approx 1.5%.
97
I-131, a radioisotope used in the treatment of leukemia, has a half-life of 8 days. How much of a sample of this radioisotope would remain after 22 days?
Aapprox 15%.
98
True or False:
Ionizing radiation is massless.
True.
99
True or False:
Ionizing radiation has a greater impact on rapidly dividing cells.
True.
This is why it is used on cancer tumors.
100
True or False:
Gamma radiation passes through clothing, whereas alpha radiation does not.
True.
101
True or False:
Healthcare professionals protect themselves from radiation by wearing clothing that contains a layer of tungsten.
False.
Its a layer of lead.
102
True or False:
The effects of ionizing radiation are directly proportional to the distance an individual is from the source.
False.
The shorter (or smaller) the distance from the source, the greater the damage done.
103
2 technicians, Sanjay and Kim were accidentally exposed to radiation. Sanjay was exposed to 8mGy while Kim was exposed to 5 rad. Which technician received more radiation?
Kim.
1 Gy = 1000 mGy.
8/1000 x 100 rad = 0.8 rad.
104
Match each property with the correct unit of measurement.
1. Activity.
2. Absorbed dose.
3. Biological damage.
1. mCi.
2. rad.
3. rem.
105
The recommended dosage of iodine-131 is 4.20 μCi/kg of body mass. How many micorcuries of iodine-131 are needed for a 75 kg person with hyperthyroidism?
315 mcg.
106
Radioisotopes of this element are used in the treatment of thyroid disease.
Iodine.
107
Which of the following is NOT a symptom of radiation sickness?
a. Vomiting.
b. Fatigue.
c. Red blood cell lysis.
d. decreased white blood cell count.
c. Red blood cell lysis.
(RBC rupture and content leaks out).
108
A curie is?
The amount of radioactive substance that undergoes 3.7 × 10^10 disintegrations per second.
109
A unit used to measure the amount of radiation absorbed per gram of tissue is the...
rad, or Gy.
110
In artificial transmutation one of the products will be a:
1. Helium atom.
2. Helium ion.
3. Hydrogen atom.
4. Hydrogen ion.
1. Helium atom.
111
True or False:
Over 3000 radioisotopes occur naturally.
False.
3300 occur unnaturally.
112
True or False:
Smoke detectors utilize the radioisotope Am-241.
True.
Am-241 emits alpha particles and when smoke interrupts this process the alarm is triggered! Life-saving chemistry.
113
An artificial transmutation of N-14 by bombardment with a neutron would result in which product?
C-14.
When a neutron bombards a larger atom it causes nuclear fission and the atom splits into a smaller one.
114
The fission of an atom of uranium
(or an atom of greater atomic number) can be induced by bombarding it with:
Neutrons.
115
When a nucleus is bombarded with
particles and breaks into two similarly sized nuclei plus one or more small
particles, the process is called:
Fission.
This can be used to turn water into steam to be used as electrical power.
116
True or False:
When an atom undergoes nuclear fission, it splits into two larger atoms.
False.
It splits into 2 smaller atoms.
117
The minimum of radioactive material needed to sustain a nuclear chain reaction is known as the:
Critical mass.
118
True or False:
The reactions responsible for the sun's energy are nuclear fusion reactions.
True.
Smaller particles collide to create larger ones. This release a lot of energy and conditions to make this reaction happen are difficult to create on earth.
119
What is the conjugate base of water?
OH -
120
A positron is a partide emitted from the nudeus that has the same mass as a(n) __________.
Electron but has a positive charge.
121
Which of the followina descriptions or an electron is correct?
A. An electron surrounds the nucleus, has a negative charge and is virtually massless.
B. An electron is found inside the nucleus, has a positive charge and a mass of 1 amu.
C. An electron surrounds the nucleus, has a negative charge and a mass of 1 amu
D. An electron surrounds the nucleus, has no charge and is virtuallv massless.
E. An electron is found inside the nucleus, has a negative charge and a mass of 1 amu.
A. An electron surrounds the nucleus, has a negative charge and is virtually massless.
122
An unstable isotope generally has:
A. Low neutron to proton ratio.
B. Change in the charge of the nucleus.
C. Equal number of protons and electrons.
D. High neutron to proton ratio.
E. Equal number of protons and neutrons.
A. Low neutron to proton ratio.
