Question 1

For HClO2,Ka = 1.2 × 10-2.What is the pH of an aqueous solution in which [NaClO2] = 0.193 M and [HClO2] = 0.203 M?

Accepted Answer

A)  3.32
B)  0.11
C)  1.92
D)  1.94
E)  1.90F) B) and D)
G) B) and C)

Question 2

What will the pH at the neutralization point of 0.00812 M Ba(OH) 2(aq) be when titrated with HCl(aq) ?

Accepted Answer

A)  7.0
B)  12.2
C)  8.0
D)  9.0
E)  6.0F) A) and B)
G) A) and C)

Question 3

What is the hydronium ion concentration in an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L-1 HCN with 50.00 mL of 0.010 mol L-1 NaCN? Assume that the volumes of the solutions are additive and that Ka = -1 HCN with 50.00 mL of 0.010 mol L-1 NaCN? Assume that the volumes of the solutions are additive and that Ka =   A) 4.9 × 10-11 mol L-1 B) 4.9 × 10-10 mol L-1 C) 4.9 × 10-9 mol L-1 D) 7.0 × 10-6 mol L-1" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  4.9 × 10-11 mol L-1
B)  4.9 × 10-10 mol L-1
C)  4.9 × 10-9 mol L-1
D)  7.0 × 10-6 mol L-1E) None of the above
F) B) and D)

Question 4

If 30.0 mmol HCl(g) is added to 1.00 L of a buffer that is 0.340 M NH3(aq) and 0.290 M NH4Cl(aq) ,what are the final concentrations of NH3(aq) and NH4Cl(aq) ,respectively? Assume no volume change.

Accepted Answer

A)  0.310 M and 0.320 M
B)  0.310 M and 0.290 M
C)  0.370 M and 0.290 M
D)  0.370 M and 0.320 ME) B) and D)
F) A) and D)

Question 5

The Henderson-Hasselbach equation,used to calculate the pH of simple conjugate-pair buffer systems,would be expressed for an ammonia/ammonium chloride buffer,for which Kb(NH3) is 1.8 × 10-5,as:

Accepted Answer

A)  pH = 4.74 + log([NH3]/[NH4+]) 
B)  pH = 4.74 + log([NH4+]/[NH3]) 
C)  pH = 9.25 + log([NH3]/[NH4+]) 
D)  pH = 9.25 + log([NH4+]/[NH3]) 
E)  pH = 14.0 - log(1.8 × 10-5) F) A) and C)
G) C) and D)

Question 6

What is the pH of a buffer that is 0.88 M HCN(aq) and 0.53 M NaCN(aq) ? The Ka of HCN is 6.2 × 10-10.

Accepted Answer

A)  8.99
B)  9.21
C)  9.43
D)  4.79E) A) and B)
F) None of the above

Question 7

Which of the following can act as buffer solutions?
I.0.1 M HC2H3O2/0.1 M NaC2H3O2
II.0.1 M NH3/0.1 M NH4Cl
III.0.1 M HNO3/0.1 M NaNO3 
IV.0.1 M H2SO3/0.1 M NaHSO3 
V.0.1 M KHSO4/ 0.1 M H2SO4

Accepted Answer

A)  I,II,and III
B)  II,IIIand IV
C)  IIIand IV
D)  I,IIand IV
E)  III,IVand VF) C) and E)
G) B) and C)

Question 8

The buffer capacity of a solution may be defined as the number of moles of H+ that will change the pH of 1.00 L of the buffer by 1.00 pH units.What is the buffer capacity of an aqueous solution which is 0.10 M in acetic acid (Ka = 1.8 × 10-5) and 0.30 M in sodium acetate,in units of mol (H+) per liter?

Accepted Answer

A)  0.20
B)  0.10
C)  0.087
D)  0.009
E)  zeroF) C) and D)
G) None of the above

Question 9

For the following titration,determine whether the solution at the equivalence point is acidic,basic or neutral and why:
KOH(aq) is titrated with HI(aq)

Accepted Answer

A)  basic because of hydrolysis of K+ 
B)  basic because of hydrolysis of KOH
C)  acidic because of hydrolysis of OH- 
D)  acidic because of hydrolysis of HI
E)  neutral salt of strong acid and strong baseF) A) and E)
G) A) and C)

Question 10

Formic acid (HCOOH,Ka = 1.8 × 10-4) is the principal component in the venom of stinging ants.What is the molarity of a formic acid solution if 25.00 mL of the aqueous formic acid solution requires 29.80 mL of 0.0567 mol L-1 NaOH(aq) to reach the equivalence point?

Accepted Answer

A)  0.0134 mol L-1
B)  0.0476 mol L-1
C)  0.0567 mol L-1
D)  0.0676 mol L-1E) A) and B)
F) None of the above

Question 11

For the following titration,determine whether the solution at the equivalence point is acidic,basic or neutral and why:
HCl(aq) is titrated with NH3(aq)

Accepted Answer

A)  acidic because of hydrolysis of NH4+ 
B)  basic because of hydrolysis of NH3 
C)  acidic because of hydrolysis of Cl- 
D)  acidic because of hydrolysis of HCl
E)  neutral salt of strong acid and strong baseF) A) and D)
G) C) and D)

Question 12

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.266 mol L-1 in nitrous acid -1 in nitrous acid   And 0.112 mol L-1 in potassium nitrite (   ) .The acid dissociation constant of nitrous acid is   A) 29.6 B) 0.402 C) 11.2 D) 1.34 ×   E) 1.55" class="answers-bank-image d-inline" rel="preload" > And 0.112 mol L-1 in potassium nitrite ( -1 in nitrous acid   And 0.112 mol L-1 in potassium nitrite (   ) .The acid dissociation constant of nitrous acid is   A) 29.6 B) 0.402 C) 11.2 D) 1.34 ×   E) 1.55" class="answers-bank-image d-inline" rel="preload" > ) .The acid dissociation constant of nitrous acid is -1 in nitrous acid   And 0.112 mol L-1 in potassium nitrite (   ) .The acid dissociation constant of nitrous acid is   A) 29.6 B) 0.402 C) 11.2 D) 1.34 ×   E) 1.55" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  29.6
B)  0.402
C)  11.2
D)  1.34 × -1 in nitrous acid   And 0.112 mol L-1 in potassium nitrite (   ) .The acid dissociation constant of nitrous acid is   
A)  29.6 
B)  0.402 
C)  11.2 
D)  1.34 ×   
E)  1.55" class="answers-bank-image d-inline" rel="preload" >
E)  1.55F) B) and E)
G) A) and B)

Question 13

Twenty-five milliliters of 0.10 M HCl(aq) is titrated with 0.10 M NaOH(aq) .What is the pH before any NaOH(aq) is added?

Accepted Answer

A)  0.40
B)  2.5
C)  0.1
D)  1.0
E)  25F) A) and C)
G) B) and E)

Question 14

25 mL of 0.10 M aqueous acetic acid is titrated with 0.10 M NaOH(aq) .What is the pH after 30 mL of NaOH have been added? Ka for acetic acid = 1.8 × 10-5.

Accepted Answer

A)  12.0
B)  2.0
C)  12.2
D)  8.7
E)  12.3F) B) and D)
G) B) and C)

Question 15

Determine the pH of the following aqueous solution.Initial concentrations are given.
[HF] = 1.296 M,[NaF] = 1.045 M,Ka for HF is 6.6 × 10-4

Accepted Answer

A)  10.73
B)  3.27
C)  3.18
D)  3.09
E)  11.91F) A) and D)
G) C) and D)

Question 16

An aqueous solution containing equimolar amounts of a weak acid with Ka = 10-5 and its sodium salt has:

Accepted Answer

A)  pH > 7
B)  pH 
C)  pH = 7
D)  pH dependent on concentration ratios
E)  pH dependent on the nature of the acid anionF) D) and E)
G) A) and B)

Question 17

Acid-base indicators have two forms: an acid of one color and a base of another color.

Accepted Answer

A) True 
 B)False

Question 18

A buffer was prepared by adding 2.4 g of ammonium nitrate to 100.0 mL of 0.30 M aqueous ammonia (Kb = 1.8 × 10-5) .To this solution was then added 10.0 mL of 0.30 M aqueous sodium hydroxide,which caused a pH change of ________.

Accepted Answer

A)  3.0 pH units
B)  0.30 pH units
C)  0.90 pH units
D)  0.09 pH units
E)  zeroF) A) and B)
G) A) and C)

Question 19

How will addition of sodium acetate to an aqueous acetic acid solution affect the pH?

Accepted Answer

A)  It will lower the pH.
B)  The pH will not change.
C)  The solution becomes hotter.
D)  The pH cannot be measured.
E)  It will raise the pH.F) A) and D)
G) A) and C)

Question 20

An aqueous solution is prepared by dissolving 0.23 mol of nitrous acid and 0.27 mol of sodium nitrite in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly.The pH does not decrease drastically because the HCl reacts with the ________ present in the buffer solution.The -3. A)    O B)    C) nitrite ion D) nitrous acid E) This is a buffer solution: the pH does not change at all upon addition of acid or base." class="answers-bank-image d-inline" rel="preload" >
Of nitrous acid is 1.36 × 10-3.

Accepted Answer

A)   -3. 
A)     O 
B)     
C)  nitrite ion 
D)  nitrous acid 
E)  This is a buffer solution: the pH does not change at all upon addition of acid or base." class="answers-bank-image d-inline" rel="preload" > O
B)   -3. 
A)     O 
B)     
C)  nitrite ion 
D)  nitrous acid 
E)  This is a buffer solution: the pH does not change at all upon addition of acid or base." class="answers-bank-image d-inline" rel="preload" >
C)  nitrite ion
D)  nitrous acid
E)  This is a buffer solution: the pH does not change at all upon addition of acid or base.F) A) and E)
G) C) and D)

Exam 17: Additional Aspects of Acidbase Equilibria

Which of the following can act as buffer solutions? I.0.1 M HC₂H₃O₂/0.1 M NaC₂H₃O₂ II.0.1 M NH₃/0.1 M NH₄Cl III.0.1 M HNO₃/0.1 M NaNO₃ IV.0.1 M H₂SO₃/0.1 M NaHSO₃ V.0.1 M KHSO₄/ 0.1 M H₂SO₄

Correct Answer
verified

The Henderson-Hasselbach equation,used to calculate the pH of simple conjugate-pair buffer systems,would be expressed for an ammonia/ammonium chloride buffer,for which K_b(NH₃) is 1.8 × 10^-5,as:

Correct Answer
verified

If 30.0 mmol HCl(g) is added to 1.00 L of a buffer that is 0.340 M NH₃(aq) and 0.290 M NH₄Cl(aq) ,what are the final concentrations of NH₃(aq) and NH₄Cl(aq) ,respectively? Assume no volume change.

Correct Answer
verified

Correct Answer
verified

What will the pH at the neutralization point of 0.00812 M Ba(OH) ₂(aq) be when titrated with HCl(aq) ?

Correct Answer
verified

25 mL of 0.10 M aqueous acetic acid is titrated with 0.10 M NaOH(aq) .What is the pH after 30 mL of NaOH have been added? K_a for acetic acid = 1.8 × 10^-5.

Correct Answer
verified

Determine the pH of the following aqueous solution.Initial concentrations are given. [HF] = 1.296 M,[NaF] = 1.045 M,K_a for HF is 6.6 × 10^-4

Correct Answer
verified

An aqueous solution containing equimolar amounts of a weak acid with K_a = 10^-5 and its sodium salt has:

Correct Answer
verified

What is the pH of a buffer that is 0.88 M HCN(aq) and 0.53 M NaCN(aq) ? The K_a of HCN is 6.2 × 10^-10.

Correct Answer
verified

Acid-base indicators have two forms: an acid of one color and a base of another color.

Correct Answer
verified

For the following titration,determine whether the solution at the equivalence point is acidic,basic or neutral and why: HCl(aq) is titrated with NH₃(aq)

Correct Answer
verified

Twenty-five milliliters of 0.10 M HCl(aq) is titrated with 0.10 M NaOH(aq) .What is the pH before any NaOH(aq) is added?

Correct Answer
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For HClO₂,K_a = 1.2 × 10^-2.What is the pH of an aqueous solution in which [NaClO₂] = 0.193 M and [HClO₂] = 0.203 M?

Correct Answer
verified

How will addition of sodium acetate to an aqueous acetic acid solution affect the pH?

Correct Answer
verified

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.266 mol L^-1 in nitrous acid And 0.112 mol L^-1 in potassium nitrite ( ) .The acid dissociation constant of nitrous acid is

Correct Answer
verified

For the following titration,determine whether the solution at the equivalence point is acidic,basic or neutral and why: KOH(aq) is titrated with HI(aq)

Correct Answer
verified

Formic acid (HCOOH,K_a = 1.8 × 10^-4) is the principal component in the venom of stinging ants.What is the molarity of a formic acid solution if 25.00 mL of the aqueous formic acid solution requires 29.80 mL of 0.0567 mol L^-1 NaOH(aq) to reach the equivalence point?

Correct Answer
verified

A buffer was prepared by adding 2.4 g of ammonium nitrate to 100.0 mL of 0.30 M aqueous ammonia (K_b = 1.8 × 10^-5) .To this solution was then added 10.0 mL of 0.30 M aqueous sodium hydroxide,which caused a pH change of ________.

Correct Answer
verified

Correct Answer
verified

What is the hydronium ion concentration in an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 HCN with 50.00 mL of 0.010 mol L^-1 NaCN? Assume that the volumes of the solutions are additive and that K_a =

Correct Answer
verified

Exam 17: Additional Aspects of Acidbase Equilibria

Which of the following can act as buffer solutions? I.0.1 M HC2H3O2/0.1 M NaC2H3O2 II.0.1 M NH3/0.1 M NH4Cl III.0.1 M HNO3/0.1 M NaNO3 IV.0.1 M H2SO3/0.1 M NaHSO3 V.0.1 M KHSO4/ 0.1 M H2SO4

Correct AnswerverifiedShow Answer

The Henderson-Hasselbach equation,used to calculate the pH of simple conjugate-pair buffer systems,would be expressed for an ammonia/ammonium chloride buffer,for which Kb(NH3) is 1.8 × 10-5,as:

Correct AnswerverifiedShow Answer

If 30.0 mmol HCl(g) is added to 1.00 L of a buffer that is 0.340 M NH3(aq) and 0.290 M NH4Cl(aq) ,what are the final concentrations of NH3(aq) and NH4Cl(aq) ,respectively? Assume no volume change.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

What will the pH at the neutralization point of 0.00812 M Ba(OH) 2(aq) be when titrated with HCl(aq) ?

Correct AnswerverifiedShow Answer

25 mL of 0.10 M aqueous acetic acid is titrated with 0.10 M NaOH(aq) .What is the pH after 30 mL of NaOH have been added? Ka for acetic acid = 1.8 × 10-5.

Correct AnswerverifiedShow Answer

Determine the pH of the following aqueous solution.Initial concentrations are given. [HF] = 1.296 M,[NaF] = 1.045 M,Ka for HF is 6.6 × 10-4

Correct AnswerverifiedShow Answer

An aqueous solution containing equimolar amounts of a weak acid with Ka = 10-5 and its sodium salt has:

Correct AnswerverifiedShow Answer

What is the pH of a buffer that is 0.88 M HCN(aq) and 0.53 M NaCN(aq) ? The Ka of HCN is 6.2 × 10-10.

Correct AnswerverifiedShow Answer

Acid-base indicators have two forms: an acid of one color and a base of another color.

Correct AnswerverifiedShow Answer

For the following titration,determine whether the solution at the equivalence point is acidic,basic or neutral and why: HCl(aq) is titrated with NH3(aq)

Correct AnswerverifiedShow Answer

Twenty-five milliliters of 0.10 M HCl(aq) is titrated with 0.10 M NaOH(aq) .What is the pH before any NaOH(aq) is added?

Correct AnswerverifiedShow Answer

For HClO2,Ka = 1.2 × 10-2.What is the pH of an aqueous solution in which [NaClO2] = 0.193 M and [HClO2] = 0.203 M?

Correct AnswerverifiedShow Answer

How will addition of sodium acetate to an aqueous acetic acid solution affect the pH?

Correct AnswerverifiedShow Answer

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.266 mol L-1 in nitrous acid And 0.112 mol L-1 in potassium nitrite ( ) .The acid dissociation constant of nitrous acid is

Correct AnswerverifiedShow Answer

For the following titration,determine whether the solution at the equivalence point is acidic,basic or neutral and why: KOH(aq) is titrated with HI(aq)

Correct AnswerverifiedShow Answer

Formic acid (HCOOH,Ka = 1.8 × 10-4) is the principal component in the venom of stinging ants.What is the molarity of a formic acid solution if 25.00 mL of the aqueous formic acid solution requires 29.80 mL of 0.0567 mol L-1 NaOH(aq) to reach the equivalence point?

Correct AnswerverifiedShow Answer

A buffer was prepared by adding 2.4 g of ammonium nitrate to 100.0 mL of 0.30 M aqueous ammonia (Kb = 1.8 × 10-5) .To this solution was then added 10.0 mL of 0.30 M aqueous sodium hydroxide,which caused a pH change of ________.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

What is the hydronium ion concentration in an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L-1 HCN with 50.00 mL of 0.010 mol L-1 NaCN? Assume that the volumes of the solutions are additive and that Ka =

Correct AnswerverifiedShow Answer

Which of the following can act as buffer solutions? I.0.1 M HC₂H₃O₂/0.1 M NaC₂H₃O₂ II.0.1 M NH₃/0.1 M NH₄Cl III.0.1 M HNO₃/0.1 M NaNO₃ IV.0.1 M H₂SO₃/0.1 M NaHSO₃ V.0.1 M KHSO₄/ 0.1 M H₂SO₄

Correct Answer
verified

The Henderson-Hasselbach equation,used to calculate the pH of simple conjugate-pair buffer systems,would be expressed for an ammonia/ammonium chloride buffer,for which K_b(NH₃) is 1.8 × 10^-5,as:

Correct Answer
verified

If 30.0 mmol HCl(g) is added to 1.00 L of a buffer that is 0.340 M NH₃(aq) and 0.290 M NH₄Cl(aq) ,what are the final concentrations of NH₃(aq) and NH₄Cl(aq) ,respectively? Assume no volume change.

Correct Answer
verified

Correct Answer
verified

What will the pH at the neutralization point of 0.00812 M Ba(OH) ₂(aq) be when titrated with HCl(aq) ?

Correct Answer
verified

25 mL of 0.10 M aqueous acetic acid is titrated with 0.10 M NaOH(aq) .What is the pH after 30 mL of NaOH have been added? K_a for acetic acid = 1.8 × 10^-5.

Correct Answer
verified

Determine the pH of the following aqueous solution.Initial concentrations are given. [HF] = 1.296 M,[NaF] = 1.045 M,K_a for HF is 6.6 × 10^-4

Correct Answer
verified

An aqueous solution containing equimolar amounts of a weak acid with K_a = 10^-5 and its sodium salt has:

Correct Answer
verified

What is the pH of a buffer that is 0.88 M HCN(aq) and 0.53 M NaCN(aq) ? The K_a of HCN is 6.2 × 10^-10.

Correct Answer
verified

Correct Answer
verified

For the following titration,determine whether the solution at the equivalence point is acidic,basic or neutral and why: HCl(aq) is titrated with NH₃(aq)

Correct Answer
verified

Correct Answer
verified

For HClO₂,K_a = 1.2 × 10^-2.What is the pH of an aqueous solution in which [NaClO₂] = 0.193 M and [HClO₂] = 0.203 M?

Correct Answer
verified

Correct Answer
verified

Calculate the percent ionization of nitrous acid in an aqueous solution that is 0.266 mol L^-1 in nitrous acid And 0.112 mol L^-1 in potassium nitrite ( ) .The acid dissociation constant of nitrous acid is

Correct Answer
verified

Correct Answer
verified

Formic acid (HCOOH,K_a = 1.8 × 10^-4) is the principal component in the venom of stinging ants.What is the molarity of a formic acid solution if 25.00 mL of the aqueous formic acid solution requires 29.80 mL of 0.0567 mol L^-1 NaOH(aq) to reach the equivalence point?

Correct Answer
verified

A buffer was prepared by adding 2.4 g of ammonium nitrate to 100.0 mL of 0.30 M aqueous ammonia (K_b = 1.8 × 10^-5) .To this solution was then added 10.0 mL of 0.30 M aqueous sodium hydroxide,which caused a pH change of ________.

Correct Answer
verified

Correct Answer
verified

What is the hydronium ion concentration in an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 HCN with 50.00 mL of 0.010 mol L^-1 NaCN? Assume that the volumes of the solutions are additive and that K_a =

Correct Answer
verified