Question 1

Which of the following solutions is acidic

Accepted Answer

A)  [OH-] = 1.0 x 10-7 M 
B)  [OH-] > 1.0 x 10-7 M 
C)  [OH-] = 1.0 x 10-10 M 
D)  [H3O+] = 1.0 x 10-10 M 
E)  [H3O+] -7 M 
A)  [OH-] = 1.0 x 10-7 M 
B)  [OH-] > 1.0 x 10-7 M 
C)  [OH-] = 1.0 x 10-10 M 
D)  [H3O+] = 1.0 x 10-10 M 
E)  [H3O+] -7 M

Question 2

Lime is used in farming to reduce the acidity of the soil. The chemical name for lime is calcium oxide. When water in the soil reacts with lime, the formula of the base formed is Ca(OH)2.

Accepted Answer

A) True 
 B)False

Question 3

Which one of these statements about strong acids is true

Accepted Answer

A)  All strong acids have H atoms bonded to electronegative oxygen atoms. 
B)  Strong acids are 100% ionized in water. 
C)  The conjugate base of a strong acid is itself a strong base. 
D)  Strong acids are very concentrated acids. 
E)  Strong acids produce solutions with a higher pH than weak acids. 
A)  All strong acids have H atoms bonded to electronegative oxygen atoms. 
B)  Strong acids are 100% ionized in water. 
C)  The conjugate base of a strong acid is itself a strong base. 
D)  Strong acids are very concentrated acids. 
E)  Strong acids produce solutions with a higher pH than weak acids.

Question 4

Suppose that ammonia, applied to a field as a fertilizer, is washed into a farm pond containing 3.0 * 106 L of water. If the pH of this pond is found to be 9.81, what volume of liquid ammonia found its way into the pond? [Given: Kb(NH3) = 1.8 * 10-5; the density of liquid ammonia is 0.771 g/cm3]

Accepted Answer

A)  15 L 
B)  25 L 
C)  11 L 
D)  19 L 
E)  320 L 
A)  15 L 
B)  25 L 
C)  11 L 
D)  19 L 
E)  320 L

Question 5

Given the following Ka values, which anion is the strongest base $\begin{array}{|l|l|}
\hline \text { Acid } & \mathrm{K}_{\mathrm{a}} \
\hline \mathrm{HF} & 7.1 \times 10^{-4} \
\hline \mathrm{HCOOH} & 1.7 \times 10^{-4} \
\hline \mathrm{HCN} & 4.9 \times 10^{-10} \
\hline \mathrm{HNO}_{2} & 4.5 \times 10^{-4} \
\hline \mathrm{CH}_{3} \mathrm{COOH} & 1.8 \times 10^{-5} \
\hline
\end{array}$

Accepted Answer

A)  F- 
B)  HCOO- 
C)  CN- 
D)  NO2- 
E)  CH3COO- 
A)  F- 
B)  HCOO- 
C)  CN- 
D)  NO2- 
E)  CH3COO-

Question 6

Which one of these salts will form an acidic solution upon dissolving in water

Accepted Answer

A)  LiBr 
B)  NaF 
C)  NH4Br 
D)  KOH 
E)  NaCN 
A)  LiBr 
B)  NaF 
C)  NH4Br 
D)  KOH 
E)  NaCN

Question 7

What mass of sodium cyanide must be added to 250. mL of water in order to obtain a solution having a pH of 10.50? [Ka(HCN) = 4.9 * 10-10]

Accepted Answer

A)  240 g 
B)  0.032 g 
C)  0.059 g 
D)  0.94 g 
E)  0.24 g 
A)  240 g 
B)  0.032 g 
C)  0.059 g 
D)  0.94 g 
E)  0.24 g

Question 8

Calculate the pH of a carbonated beverage in which the hydrogen ion concentration is 3.4 * 10-4 M.

Accepted Answer

A)  2.34 
B)  3.47 
C)  6.01 
D)  7.99 
E)  10.53 
A)  2.34 
B)  3.47 
C)  6.01 
D)  7.99 
E)  10.53

Question 9

Predict the direction in which the equilibrium will lie for the reaction C6H5COO- + HF $\leftrightharpoons$ C6H5COOH + F-.Ka(C6H5COOH) = 6.5 * 10-5; Ka(HF) = 7.1 * 10-4

Accepted Answer

A)  to the right 
B)  to the left 
C)  in the middle 
A)  to the right 
B)  to the left 
C)  in the middle

Question 10

Given the following Kb values, which cation is the strongest acid $\begin{array}{|l|l|}
\hline \text { Base } & \mathrm{K}_{\mathrm{b}} \
\hline \mathrm{NH}_{3} & 1.8 \times 10^{-5} \
\hline \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{2} & 5.6 \times 10^{-4} \
\hline \mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N} & 1.7 \times 10^{-9} \
\hline \mathrm{C}_{8} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{O}_{2} & 5.3 \times 10^{-14} \
\hline\left(\mathrm{NH}_{2}\right)_{2} \mathrm{CO} & 1.5 \times 10^{-14} \
\hline
\end{array}$

Accepted Answer

A)  NH4+ 
B)  C2H5NH3+ 
C)  C5H6N+ 
D)  [C8H11N4O2]+ 
E)  [NH2NH3CO]+ 
A)  NH4+ 
B)  C2H5NH3+ 
C)  C5H6N+ 
D)  [C8H11N4O2]+ 
E)  [NH2NH3CO]+

Question 11

The formula for the conjugate base of H3PO4 is H2PO4-.

Accepted Answer

A) True 
 B)False

Question 12

Which of the following does not fit the definition of a Brønsted Acid

Accepted Answer

A)  H3PO4 
B)  H2PO4- 
C)  H2O 
D)  NH4+ 
E)  CO2 
A)  H3PO4 
B)  H2PO4- 
C)  H2O 
D)  NH4+ 
E)  CO2

Question 13

A 5.5 L sample of a 0.25 M HNO3 solution is mixed with 1.2 L of a 0.34 M HCl solution. What is the pH of the mixture

Accepted Answer

A)  0.23 
B)  0.57 
C)  1.07 
D)  0.50 
E)  0.84 
A)  0.23 
B)  0.57 
C)  1.07 
D)  0.50 
E)  0.84

Question 14

If the pH of liquid bleach is 12.0, what is the hydroxide ion concentration in this solution

Accepted Answer

A)  1 * 10-2 M 
B)  1 * 10-3 M 
C)  1 * 10-4 M 
D)  1 * 10-5 M 
E)  None of the above 
A)  1 * 10-2 M 
B)  1 * 10-3 M 
C)  1 * 10-4 M 
D)  1 * 10-5 M 
E)  None of the above

Question 15

Which of the following is not a conjugate acid-base pair

Accepted Answer

A)  H3PO4 and H2PO4- 
B)  H2PO4- and HPO42- 
C)  H3PO4 and HPO42- 
D)  HPO42- and PO43- 
E)  H2O and H3O+ 
A)  H3PO4 and H2PO4- 
B)  H2PO4- and HPO42- 
C)  H3PO4 and HPO42- 
D)  HPO42- and PO43- 
E)  H2O and H3O+

Question 16

Which one of these salts will form a basic solution on dissolving in water

Accepted Answer

A)  NaCl 
B)  KCN 
C)  NaNO3 
D)  NH4NO3 
E)  FeCl3 
A)  NaCl 
B)  KCN 
C)  NaNO3 
D)  NH4NO3 
E)  FeCl3

Question 17

The equilibrium expression for the hydrolysis of a weak base, A-, in water is:

Accepted Answer

A)  Kb = [A-]/[OH-][H3O+] 
B)  Kb = [OH-][H3O+]/[A-] 
C)  Kb = [OH-][HA]/[A-] 
D)  Kb = [OH-][A-]/[HA] 
E)  Kb = [OH-][HA]/[A-][H3O+] 
A)  Kb = [A-]/[OH-][H3O+] 
B)  Kb = [OH-][H3O+]/[A-] 
C)  Kb = [OH-][HA]/[A-] 
D)  Kb = [OH-][A-]/[HA] 
E)  Kb = [OH-][HA]/[A-][H3O+]

Question 18

The OH- concentration in a 1.0 * 10-3 M Ba(OH)2 solution is

Accepted Answer

A)  0.50 * 10-3 M. 
B)  1.0 * 10-3 M. 
C)  2.0 * 10-3 M. 
D)  1.0 * 10-2 M. 
E)  0.020 M. 
A)  0.50 * 10-3 M. 
B)  1.0 * 10-3 M. 
C)  2.0 * 10-3 M. 
D)  1.0 * 10-2 M. 
E)  0.020 M.

Question 19

What is the pH of a 0.080 M solution of the weak base pyridine (C5H5N; Kb = 1.7 x 10-9)

Accepted Answer

A)  8.77 
B)  5.23 
C)  4.93 
D)  12.90 
E)  9.07 
A)  8.77 
B)  5.23 
C)  4.93 
D)  12.90 
E)  9.07

Question 20

Which one of these salts will form a basic solution upon dissolving in water

Accepted Answer

A)  NaCl 
B)  NaNO2 
C)  NH4NO3 
D)  KBr 
E)  AlCl3 
A)  NaCl 
B)  NaNO2 
C)  NH4NO3 
D)  KBr 
E)  AlCl3

Exam 15: Acids and Bases

Which of the following solutions is acidic

Lime is used in farming to reduce the acidity of the soil. The chemical name for lime is calcium oxide. When water in the soil reacts with lime, the formula of the base formed is Ca(OH)2.

Which one of these statements about strong acids is true

Suppose that ammonia, applied to a field as a fertilizer, is washed into a farm pond containing 3.0 * 106 L of water. If the pH of this pond is found to be 9.81, what volume of liquid ammonia found its way into the pond? [Given: Kb(NH3) = 1.8 * 10-5; the density of liquid ammonia is 0.771 g/cm3]

Given the following Ka values, which anion is the strongest base Acid 7.1\times1 1.7\times1 4.9\times1 4.5\times1 1.8\times1

Which one of these salts will form an acidic solution upon dissolving in water

What mass of sodium cyanide must be added to 250. mL of water in order to obtain a solution having a pH of 10.50? [Ka(HCN) = 4.9 * 10-10]

Calculate the pH of a carbonated beverage in which the hydrogen ion concentration is 3.4 * 10-4 M.

Predict the direction in which the equilibrium will lie for the reaction C6H5COO- + HF ⇋\leftrightharpoons⇋ C6H5COOH + F-.Ka(C6H5COOH) = 6.5 * 10-5; Ka(HF) = 7.1 * 10-4

Given the following Kb values, which cation is the strongest acid Base 1.8\times1 5.6\times1 1.7\times1 5.3\times1 1.5\times1

The formula for the conjugate base of H3PO4 is H2PO4-.

Which of the following does not fit the definition of a Brønsted Acid

A 5.5 L sample of a 0.25 M HNO3 solution is mixed with 1.2 L of a 0.34 M HCl solution. What is the pH of the mixture

If the pH of liquid bleach is 12.0, what is the hydroxide ion concentration in this solution

Which of the following is not a conjugate acid-base pair

Which one of these salts will form a basic solution on dissolving in water

The equilibrium expression for the hydrolysis of a weak base, A-, in water is:

The OH- concentration in a 1.0 * 10-3 M Ba(OH)2 solution is

What is the pH of a 0.080 M solution of the weak base pyridine (C5H5N; Kb = 1.7 x 10-9)

Which one of these salts will form a basic solution upon dissolving in water

Chemistry: The Study of Change

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Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

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Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

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Chemical Equilibrium

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

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Chemistry in the Atmosphere

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Filters

Lime is used in farming to reduce the acidity of the soil. The chemical name for lime is calcium oxide. When water in the soil reacts with lime, the formula of the base formed is Ca(OH)₂.

Given the following K_a values, which anion is the strongest base Acid 7.1\times1 1.7\times1 4.9\times1 4.5\times1 1.8\times1

What mass of sodium cyanide must be added to 250. mL of water in order to obtain a solution having a pH of 10.50? [K_a(HCN) = 4.9 * 10^-10]

Calculate the pH of a carbonated beverage in which the hydrogen ion concentration is 3.4 * 10^-4 M.

Predict the direction in which the equilibrium will lie for the reaction C₆H₅COO^- + HF $\leftrightharpoons$ C₆H₅COOH + F^-.K_a(C₆H₅COOH) = 6.5 * 10^-5; K_a(HF) = 7.1 * 10^-4

Given the following K_b values, which cation is the strongest acid Base 1.8\times1 5.6\times1 1.7\times1 5.3\times1 1.5\times1

The formula for the conjugate base of H₃PO₄ is H₂PO₄^-.

A 5.5 L sample of a 0.25 M HNO₃ solution is mixed with 1.2 L of a 0.34 M HCl solution. What is the pH of the mixture

The equilibrium expression for the hydrolysis of a weak base, A^-, in water is:

The OH^- concentration in a 1.0 * 10^-3 M Ba(OH)₂ solution is

What is the pH of a 0.080 M solution of the weak base pyridine (C₅H₅N; K_b = 1.7 x 10^-9)