Question 1

Which of the following mathematical equations corresponds to the acid dissociation constant (Ka)?

Accepted Answer

A)  $K_{\mathrm{a}}=\frac{\left[\mathrm{H}^{+}\right]\left[\mathrm{OH}^{-}\right]}{[\mathrm{HB}]}$ 
B)  $K_{\mathrm{a}}=\frac{\left[\mathrm{H}^{+}\right][\mathrm{HB}]}{\left[\mathrm{B}^{-}\right]}$ 
C)  $K_{\mathrm{a}}=\frac{[\mathrm{HB}]\left[\mathrm{B}^{-}\right]}{\left[\mathrm{H}^{+}\right]}$ 
D)  $K_{\mathrm{a}}=\frac{\left[\mathrm{B}^{-}\right][\mathrm{HB}]}{\left[\mathrm{H}^{+}\right]}$ 
E)  $K_{\mathrm{a}}=\frac{\left[\mathrm{H}^{+}\right]\left[\mathrm{B}^{-}\right]}{[\mathrm{HB}]}$ 
A)  $K_{\mathrm{a}}=\frac{\left[\mathrm{H}^{+}\right]\left[\mathrm{OH}^{-}\right]}{[\mathrm{HB}]}$ 
B)  $K_{\mathrm{a}}=\frac{\left[\mathrm{H}^{+}\right][\mathrm{HB}]}{\left[\mathrm{B}^{-}\right]}$ 
C)  $K_{\mathrm{a}}=\frac{[\mathrm{HB}]\left[\mathrm{B}^{-}\right]}{\left[\mathrm{H}^{+}\right]}$ 
D)  $K_{\mathrm{a}}=\frac{\left[\mathrm{B}^{-}\right][\mathrm{HB}]}{\left[\mathrm{H}^{+}\right]}$ 
E)  $K_{\mathrm{a}}=\frac{\left[\mathrm{H}^{+}\right]\left[\mathrm{B}^{-}\right]}{[\mathrm{HB}]}$ E

Question 2

Hydrogen sulfate ion,HSO4−,has an acid dissociation constant of 1.0 × 10−2.What is the pH of 0.45 M hydrogen sulfate?

Accepted Answer

A)  0.35 
B)  1.21 
C)  2.00 
D)  2.19 
E)  3.03 
A)  0.35 
B)  1.21 
C)  2.00 
D)  2.19 
E)  3.03 B

Question 3

Seawater has a hydroxide ion concentration of 2.0 × 10−6 M.What is the pH of seawater?

Accepted Answer

A)  −8.30 
B)  5.70 
C)  6.99 
D)  7.53 
E)  8.30 
A)  −8.30 
B)  5.70 
C)  6.99 
D)  7.53 
E)  8.30 E

Question 4

What is the correct expression for the calculation of pH?

Accepted Answer

A)  pH = log[1.0 × 10−14] 
B)  pH = −log([H+][OH−]) 
C)  pH = log[OH−] 
D)  pH = −log[OH−] 
E)  pH = −log[H+] 
A)  pH = log[1.0 × 10−14] 
B)  pH = −log([H+][OH−]) 
C)  pH = log[OH−] 
D)  pH = −log[OH−] 
E)  pH = −log[H+]

Question 5

What is the pH of 1.0 M sulfurous acid? (Ka1 = 1.7 × 10−2,Ka2 = 6.0 × 10−8)

Accepted Answer

A)  −0.88 
B)  0.00 
C)  0.12 
D)  0.13 
E)  0.91 
A)  −0.88 
B)  0.00 
C)  0.12 
D)  0.13 
E)  0.91

Question 6

If the pH of a solution is greater than 7,the solution is

Accepted Answer

A)  acidic. 
B)  basic. 
C)  amphiprotic. 
D)  neutral. 
E)  in equilibrium. 
A)  acidic. 
B)  basic. 
C)  amphiprotic. 
D)  neutral. 
E)  in equilibrium.

Question 7

A solution of 0.10 M aluminum nitrate has a pH close to 3.0.Which chemical equation explains the acidic pH of the solution?

Accepted Answer

A)  Al3+(aq)+ 3OH?(aq)  ? Al(OH)3(s)+ 3H3O+(aq) 
B)  Al(H2O)63+(aq)+ H2O(l)  ? Al(H2O)5(OH)2+(aq)+ H3O+(aq) 
C)  Al(NO3)3(s)+ 3H2O(l)  ? Al(OH)3(s)+ 3HNO3(s) 
D)  HNO3(aq)+ H2O(l)  ? NO3?(aq)+ H3O+(aq) 
E)  NO3?(aq)+ H2O(l)  ? H2O + HNO3(aq) 
A)  Al3+(aq)+ 3OH?(aq)  ? Al(OH)3(s)+ 3H3O+(aq) 
B)  Al(H2O)63+(aq)+ H2O(l)  ? Al(H2O)5(OH)2+(aq)+ H3O+(aq) 
C)  Al(NO3)3(s)+ 3H2O(l)  ? Al(OH)3(s)+ 3HNO3(s) 
D)  HNO3(aq)+ H2O(l)  ? NO3?(aq)+ H3O+(aq) 
E)  NO3?(aq)+ H2O(l)  ? H2O + HNO3(aq)

Question 8

What is the conjugate acid of potassium hydrogen phosphate,K2HPO4?

Accepted Answer

A)  H3PO4 
B)  H2PO4− 
C)  HPO42− 
D)  K+ 
E)  OH− 
A)  H3PO4 
B)  H2PO4− 
C)  HPO42− 
D)  K+ 
E)  OH−

Question 9

A solution of 0.25 mol HF diluted to 1.0 L has a hydronium ion concentration of 1.3 × 10−2 M.What is the percent ionization of HF?

Accepted Answer

A)  0.80 % 
B)  1.3% 
C)  4.2% 
D)  5.2% 
E)  31% 
A)  0.80 % 
B)  1.3% 
C)  4.2% 
D)  5.2% 
E)  31%

Question 10

What is the pH of a solution prepared by diluting 0.40 mol HNO3(aq)to a volume of 225 mL?

Accepted Answer

A)  −0.25 
B)  0.25 
C)  0.40 
D)  2.75 
E)  7.50 
A)  −0.25 
B)  0.25 
C)  0.40 
D)  2.75 
E)  7.50

Question 11

An aqueous solution with a pH of 2.00 is diluted from 1.0 L to 3.0 L.What is the pH of the diluted solution?

Accepted Answer

A)  0.67 
B)  2.00 
C)  2.48 
D)  4.33 
E)  6.00 
A)  0.67 
B)  2.00 
C)  2.48 
D)  4.33 
E)  6.00

Question 12

What is the pH of 0.26 M ammonium ion? 
NH4+(aq)+ H2O(l)  ? NH3(aq)+ H3O+(aq)
Ka = 5.6 × 10?10

Accepted Answer

A)  3.87 
B)  4.33 
C)  4.75 
D)  4.92 
E)  9.25 
A)  3.87 
B)  4.33 
C)  4.75 
D)  4.92 
E)  9.25

Question 13

At 50°C,the water ionization constant,Kw,is 5.48 × 10-14.What is the H3O+ concentration in neutral water at this temperature?

Accepted Answer

A)  3.00 × 10-27 M 
B)  2.74 × 10-14 M 
C)  5.48 × 10-14 M 
D)  2.34 × 10-7 M 
E)  1.01 × 10-7 M 
A)  3.00 × 10-27 M 
B)  2.74 × 10-14 M 
C)  5.48 × 10-14 M 
D)  2.34 × 10-7 M 
E)  1.01 × 10-7 M

Question 14

Identify from the following list of molecules and ions those which behave as Lewis acids: NH3,BCl3,Fe3+.

Accepted Answer

A)  NH3 only 
B)  NH3 and BCl3 
C)  Fe3+ only 
D)  BCl3,and Fe3+ 
E)  NH3,BCl3,and Fe3+ 
A)  NH3 only 
B)  NH3 and BCl3 
C)  Fe3+ only 
D)  BCl3,and Fe3+ 
E)  NH3,BCl3,and Fe3+

Question 15

The pH of 0.350 M benzoic acid,HC7H5O2,is 2.32.What is the pKa for this acid?

Accepted Answer

A)  0.350 
B)  1.38 
C)  1.79 
D)  2.32 
E)  4.18 
A)  0.350 
B)  1.38 
C)  1.79 
D)  2.32 
E)  4.18

Question 16

A Lewis acid is defined as a(n)

Accepted Answer

A)  electron pair acceptor. 
B)  proton acceptor. 
C)  electron pair donor. 
D)  spectator ion. 
E)  proton acceptor.. 
A)  electron pair acceptor. 
B)  proton acceptor. 
C)  electron pair donor. 
D)  spectator ion. 
E)  proton acceptor..

Question 17

All of the following species are strong bases EXCEPT

Accepted Answer

A)  NaOH. 
B)  KOH. 
C)  Mg(OH)2. 
D)  Sr(OH)2. 
E)  RbOH. 
A)  NaOH. 
B)  KOH. 
C)  Mg(OH)2. 
D)  Sr(OH)2. 
E)  RbOH.

Question 18

What is the conjugate base of HClO2?

Accepted Answer

A)  H+ 
B)  H− 
C)  ClO2+ 
D)  ClO+ 
E)  ClO2− 
A)  H+ 
B)  H− 
C)  ClO2+ 
D)  ClO+ 
E)  ClO2−

Question 19

All of the following statements concerning diprotic acids and bases are incorrect EXCEPT

Accepted Answer

A)  Ka2 is larger than Ka1. 
B)  Ka1 is larger than Ka2. 
C)  Ka1 is equal to Kb2. 
D)  Ka1 + Kb2 equals Kw. 
E)  Ka1 + Ka2 equals Kw. 
A)  Ka2 is larger than Ka1. 
B)  Ka1 is larger than Ka2. 
C)  Ka1 is equal to Kb2. 
D)  Ka1 + Kb2 equals Kw. 
E)  Ka1 + Ka2 equals Kw.

Question 20

Given the following equilibrium constants, Ka (HSO4-)= 1.2 × 10-2
Kb (CH3CO2-)= 5.6 × 10-10
Kw = 1.00 × 10-14
determine the equilibrium constant for the reaction below at 25°C.
HSO4-(aq)+ CH3CO2-(aq)  ? SO42-(aq)+ CH3CO2H(aq)

Accepted Answer

A)  6.7 × 10-12 
B)  2.1 × 10-7 
C)  1.5 × 10-3 
D)  6.7 × 102 
E)  2.1 × 107 
A)  6.7 × 10-12 
B)  2.1 × 10-7 
C)  1.5 × 10-3 
D)  6.7 × 102 
E)  2.1 × 107

Exam 13: Acids and Bases

Which of the following mathematical equations corresponds to the acid dissociation constant (Ka)?

Hydrogen sulfate ion,HSO4−,has an acid dissociation constant of 1.0 × 10−2.What is the pH of 0.45 M hydrogen sulfate?

Seawater has a hydroxide ion concentration of 2.0 × 10−6 M.What is the pH of seawater?

What is the correct expression for the calculation of pH?

What is the pH of 1.0 M sulfurous acid? (Ka1 = 1.7 × 10−2,Ka2 = 6.0 × 10−8)

If the pH of a solution is greater than 7,the solution is

A solution of 0.10 M aluminum nitrate has a pH close to 3.0.Which chemical equation explains the acidic pH of the solution?

What is the conjugate acid of potassium hydrogen phosphate,K2HPO4?

A solution of 0.25 mol HF diluted to 1.0 L has a hydronium ion concentration of 1.3 × 10−2 M.What is the percent ionization of HF?

What is the pH of a solution prepared by diluting 0.40 mol HNO3(aq)to a volume of 225 mL?

An aqueous solution with a pH of 2.00 is diluted from 1.0 L to 3.0 L.What is the pH of the diluted solution?

What is the pH of 0.26 M ammonium ion? NH4+(aq)+ H2O(l) ? NH3(aq)+ H3O+(aq) Ka = 5.6 × 10?10

At 50°C,the water ionization constant,Kw,is 5.48 × 10-14.What is the H3O+ concentration in neutral water at this temperature?

Identify from the following list of molecules and ions those which behave as Lewis acids: NH3,BCl3,Fe3+.

The pH of 0.350 M benzoic acid,HC7H5O2,is 2.32.What is the pKa for this acid?

A Lewis acid is defined as a(n)

All of the following species are strong bases EXCEPT

What is the conjugate base of HClO2?

All of the following statements concerning diprotic acids and bases are incorrect EXCEPT

Given the following equilibrium constants, Ka (HSO4-)= 1.2 × 10-2 Kb (CH3CO2-)= 5.6 × 10-10 Kw = 1.00 × 10-14 determine the equilibrium constant for the reaction below at 25°C. HSO4-(aq)+ CH3CO2-(aq) ? SO42-(aq)+ CH3CO2H(aq)

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Filters

Which of the following mathematical equations corresponds to the acid dissociation constant (K_a)?

Hydrogen sulfate ion,HSO₄−,has an acid dissociation constant of 1.0 × 10−².What is the pH of 0.45 M hydrogen sulfate?

Seawater has a hydroxide ion concentration of 2.0 × 10−⁶ M.What is the pH of seawater?

What is the pH of 1.0 M sulfurous acid? (K_a1 = 1.7 × 10−²,K_a2 = 6.0 × 10−⁸)

What is the conjugate acid of potassium hydrogen phosphate,K₂HPO₄?

A solution of 0.25 mol HF diluted to 1.0 L has a hydronium ion concentration of 1.3 × 10−² M.What is the percent ionization of HF?

What is the pH of a solution prepared by diluting 0.40 mol HNO₃(aq)to a volume of 225 mL?

What is the pH of 0.26 M ammonium ion? NH₄⁺(aq)+ H₂O(l) ? NH₃(aq)+ H₃O⁺(aq) K_a = 5.6 × 10?¹⁰

At 50°C,the water ionization constant,K_w,is 5.48 × 10^-14.What is the H₃O⁺ concentration in neutral water at this temperature?

Identify from the following list of molecules and ions those which behave as Lewis acids: NH₃,BCl₃,Fe³⁺.

The pH of 0.350 M benzoic acid,HC₇H₅O₂,is 2.32.What is the pK_a for this acid?

What is the conjugate base of HClO₂?

Given the following equilibrium constants, K_a (HSO₄^-)= 1.2 × 10^-2K_b (CH₃CO₂^-)= 5.6 × 10^-10 K_w = 1.00 × 10^-14determine the equilibrium constant for the reaction below at 25°C. HSO₄^-(aq)+ CH₃CO₂^-(aq) ? SO₄^2-(aq)+ CH₃CO₂H(aq)