Question 1

A sample of a monoprotic acid (HA)  weighing 0.384 g is dissolved in water and the solution is titrated with aqueous NaOH. If 30.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the molar mass of HA?

Accepted Answer

A)   37.0 g/mol
B)   81.0 g/mol
C)   128 g/mol
D)   20.3 g/mol
E)   211 g/molF) A) and E)
G) A) and B)

Question 2

What volume of 0.200 M KOH must be added to 17.5 mL of 0.135 M H3PO4 to reach the third equivalence point?

Accepted Answer

A)   3.94 mL
B)   11.8 mL
C)   17.5 mL
D)   23.6 mL
E)   35.4 mLF) B) and E)
G) B) and D)

Question 3

At the equivalence point in an acid-base titration

Accepted Answer

A)   the [H3O+] equals the Ka of the acid.
B)   the [H3O+] equals the Ka of the indicator.
C)   the amounts of acid and base which have been combined are in their stoichiometric ratio.
D)   the pH is 7.0.
E)   the pH has reached a maximum.F) A) and E)
G) A) and C)

Question 4

A 25.0-mL sample of 0.10 M C2H3NH2 (ethylamine)  is titrated with 0.15 M HCl. What is the pH of the solution after 9.00 mL of acid have been added to the amine? Kb = 6.5 × 10-4

Accepted Answer

A)   11.08
B)   10.88
C)   10.74
D)   10.55
E)   10.49F) B) and C)
G) B) and E)

Question 5

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

Accepted Answer

A)   3.67
B)   3.78
C)   3.81
D)   3.85
E)   3.95F) B) and E)
G) B) and C)

Question 6

Which of the following substances has the greatest solubility in water?

Accepted Answer

A)   PbI2, Ksp = 7.9 × 10-9
B)   BaF2, Ksp = 1.5 × 10-6
C)   Ca(OH) 2, Ksp = 6.5 × 10-6
D)   Zn(IO3) 2, Ksp = 3.9 × 10-6
E)   Ag2SO4, Ksp = 1.5 × 10-5F) B) and D)
G) B) and C)

Question 7

Write the ion product expression for calcium phosphate, Ca3(PO4) 2.

Accepted Answer

A)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)   None of the above is the correct ion product expression." class="answers-bank-image d-inline" rel="preload" >
B)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)   None of the above is the correct ion product expression." class="answers-bank-image d-inline" rel="preload" >
C)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)   None of the above is the correct ion product expression." class="answers-bank-image d-inline" rel="preload" >
D)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)   None of the above is the correct ion product expression." class="answers-bank-image d-inline" rel="preload" >
E)   None of the above is the correct ion product expression.F) C) and D)
G) All of the above

Question 8

Make a clear distinction between buffer range and buffer capacity.

Accepted Answer

Buffer range is the range of pH over whi...

Question 9

The solubility of lead(II)  chloride is 0.45 g/100 mL of solution. What is the Ksp of PbCl2?

Accepted Answer

A)   4.9 × 10-2
B)   1.7 × 10-5
C)   8.5 × 10-6
D)   4.2 × 10-6
E)   -6F) A) and C)
G) A) and D)

Question 10

The pH of blood is 7.35. It is maintained in part by the buffer system composed of carbonic acid (H2CO3)  and the bicarbonate (hydrogen carbonate, HCO3-)  ion. What is the ratio of [bicarbonate]/[carbonic acid] at this pH? For carbonic acid, Ka1 = 4.2 × 10-7.

Accepted Answer

A)   [bicarbonate]/[carbonic acid] = 0.11
B)   [bicarbonate]/[carbonic acid] = 0.38
C)   [bicarbonate]/[carbonic acid] = 2.65
D)   [bicarbonate]/[carbonic acid] = 9.4
E)   None of the above ratios is correct.F) B) and C)
G) None of the above

Question 11

Formic acid is a monoprotic acid with a Ka value of 1.8 × 10-4 at 25°C.
a. Calculate the pH of a 0.200 mol L-1 solution of the acid, making any reasonable approximations.
b. If 0.0050 mol of NaOH is added to 100. mL of the solution in (a), calculate the pH of the resultant buffer.

Accepted Answer

Question 12

For a diprotic acid H2A, the relationship Ka1 > Ka2 is always true.

Accepted Answer

A) True 
 B)False

Question 13

When a weak acid is titrated with a weak base, the pH at the equivalence point

Accepted Answer

A)   is greater than 7.0.
B)   is equal to 7.0.
C)   is less than 7.0.
D)   is determined by the sizes of Ka and Kb.
E)   is no longer affected by addition of base.F) All of the above
G) C) and D)

Question 14

Calculate the solubility of magnesium sulfate, MgSO4, when placed into a 0.10 M MgCl2 solution. Ksp = 5.9 × 10-3

Accepted Answer

A)   4.2 × 10-2 M
B)   5.9 × 10-2 M
C)   7.7 × 10-2 M
D)   3.5 × 10-5 M
E)   3.5 × 10-6 MF) A) and B)
G) B) and E)

Question 15

What will be the effect of adding 0.5 mL of 0.1 M NaOH to 100 mL of an acetate buffer in which [CH3COOH] = [CH3COO-] = 0.5 M?

Accepted Answer

A)   The pH will increase slightly.
B)   The pH will increase significantly.
C)   The pH will decrease slightly.
D)   The pH will decrease significantly.
E)   Since it is a buffer solution, the pH will not be affected.F) C) and E)
G) A) and D)

Question 16

Citric acid has an acid dissociation constant of 8.4 × 10-4. It would be most effective for preparation of a buffer with a pH of

Accepted Answer

A)   2.
B)   3.
C)   4.
D)   5.
E)   6.F) A) and E)
G) C) and E)

Question 17

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate, Cd(NO3) 2. Which of the following statements is correct? Ksp = 6.44 × 10-3 for CdF2.

Accepted Answer

A)   Cadmium fluoride precipitates until the solution is saturated.
B)   The solution is unsaturated and no precipitate forms.
C)   The solubility of cadmium fluoride is increased by the presence of additional fluoride ions.
D)   One must know Ksp for cadmium nitrate to make meaningful predictions on this system.
E)   The presence of NaF will raise the solubility of Cd(NO3) 2.F) B) and E)
G) C) and D)

Question 18

Calculate the solubility of silver phosphate, Ag3PO4, in pure water. Ksp = 2.6 × 10-18

Accepted Answer

A)   4.0 × 10-5 M
B)   1.8 × 10-5 M
C)   4.0 × 10-6 M
D)   1.5 × 10-6 M
E)   -6 MF) D) and E)
G) B) and E)

Question 19

The solubility of calcium chromate is 1.56 × 10-3 g/100 mL of solution. What is the Ksp for CaCrO4?

Accepted Answer

A)   2.4 × 10-4
B)   1.5 × 10-5
C)   7.6 × 10-6
D)   1.0 × 10-8
E)   -8F) A) and B)
G) A) and C)

Exam 19: Ionic Equilibria in Aqueous Systems

When a weak acid is titrated with a weak base, the pH at the equivalence point

Correct Answer
verified

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

Correct Answer
verified

Write the ion product expression for calcium phosphate, Ca₃(PO₄) ₂.

Correct Answer
verified

What will be the effect of adding 0.5 mL of 0.1 M NaOH to 100 mL of an acetate buffer in which [CH₃COOH] = [CH₃COO^-] = 0.5 M?

Correct Answer
verified

Which of the following substances has the greatest solubility in water?

Correct Answer
verified

Calculate the solubility of silver phosphate, Ag₃PO₄, in pure water. K_sp = 2.6 × 10^-18

Correct Answer
verified

For a diprotic acid H₂A, the relationship K_a1 > K_a2 is always true.

Correct Answer
verified

At the equivalence point in an acid-base titration

Correct Answer
verified

What volume of 0.200 M KOH must be added to 17.5 mL of 0.135 M H₃PO₄to reach the third equivalence point?

Correct Answer
verified

Formic acid is a monoprotic acid with a K_a value of 1.8 × 10^-4 at 25°C. a. Calculate the pH of a 0.200 mol L^-1 solution of the acid, making any reasonable approximations. b. If 0.0050 mol of NaOH is added to 100. mL of the solution in (a), calculate the pH of the resultant buffer.

Correct Answer
verified

A 25.0-mL sample of 0.10 M C₂H₃NH₂(ethylamine) is titrated with 0.15 M HCl. What is the pH of the solution after 9.00 mL of acid have been added to the amine? K_b = 6.5 × 10^-4

Correct Answer
verified

The pH of blood is 7.35. It is maintained in part by the buffer system composed of carbonic acid (H₂CO₃) and the bicarbonate (hydrogen carbonate, HCO₃^-) ion. What is the ratio of [bicarbonate]/[carbonic acid] at this pH? For carbonic acid, K_a1 = 4.2 × 10^-7.

Correct Answer
verified

Calculate the solubility of magnesium sulfate, MgSO₄, when placed into a 0.10 M MgCl₂solution. K_sp = 5.9 × 10^-3

Correct Answer
verified

Citric acid has an acid dissociation constant of 8.4 × 10^-4. It would be most effective for preparation of a buffer with a pH of

Correct Answer
verified

A sample of a monoprotic acid (HA) weighing 0.384 g is dissolved in water and the solution is titrated with aqueous NaOH. If 30.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the molar mass of HA?

Correct Answer
verified

Make a clear distinction between buffer range and buffer capacity.

Correct Answer
verified
Buffer range is the range of pH over whi...
View Answer

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the K_sp of PbCl₂?

Correct Answer
verified

The solubility of calcium chromate is 1.56 × 10^-3 g/100 mL of solution. What is the K_sp for CaCrO₄?

Correct Answer
verified

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate, Cd(NO₃) ₂. Which of the following statements is correct? K_sp = 6.44 × 10^-3 for CdF₂.

Correct Answer
verified

Exam 19: Ionic Equilibria in Aqueous Systems

When a weak acid is titrated with a weak base, the pH at the equivalence point

Correct AnswerverifiedShow Answer

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

Correct AnswerverifiedShow Answer

Write the ion product expression for calcium phosphate, Ca3(PO4) 2.

Correct AnswerverifiedShow Answer

What will be the effect of adding 0.5 mL of 0.1 M NaOH to 100 mL of an acetate buffer in which [CH3COOH] = [CH3COO-] = 0.5 M?

Correct AnswerverifiedShow Answer

Which of the following substances has the greatest solubility in water?

Correct AnswerverifiedShow Answer

Calculate the solubility of silver phosphate, Ag3PO4, in pure water. Ksp = 2.6 × 10-18

Correct AnswerverifiedShow Answer

For a diprotic acid H2A, the relationship Ka1 > Ka2 is always true.

Correct AnswerverifiedShow Answer

At the equivalence point in an acid-base titration

Correct AnswerverifiedShow Answer

What volume of 0.200 M KOH must be added to 17.5 mL of 0.135 M H3PO4 to reach the third equivalence point?

Correct AnswerverifiedShow Answer

Formic acid is a monoprotic acid with a Ka value of 1.8 × 10-4 at 25°C. a. Calculate the pH of a 0.200 mol L-1 solution of the acid, making any reasonable approximations. b. If 0.0050 mol of NaOH is added to 100. mL of the solution in (a), calculate the pH of the resultant buffer.

Correct AnswerverifiedShow Answer

A 25.0-mL sample of 0.10 M C2H3NH2 (ethylamine) is titrated with 0.15 M HCl. What is the pH of the solution after 9.00 mL of acid have been added to the amine? Kb = 6.5 × 10-4

Correct AnswerverifiedShow Answer

The pH of blood is 7.35. It is maintained in part by the buffer system composed of carbonic acid (H2CO3) and the bicarbonate (hydrogen carbonate, HCO3-) ion. What is the ratio of [bicarbonate]/[carbonic acid] at this pH? For carbonic acid, Ka1 = 4.2 × 10-7.

Correct AnswerverifiedShow Answer

Calculate the solubility of magnesium sulfate, MgSO4, when placed into a 0.10 M MgCl2 solution. Ksp = 5.9 × 10-3

Correct AnswerverifiedShow Answer

Citric acid has an acid dissociation constant of 8.4 × 10-4. It would be most effective for preparation of a buffer with a pH of

Correct AnswerverifiedShow Answer

A sample of a monoprotic acid (HA) weighing 0.384 g is dissolved in water and the solution is titrated with aqueous NaOH. If 30.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the molar mass of HA?

Correct AnswerverifiedShow Answer

Make a clear distinction between buffer range and buffer capacity.

Correct AnswerverifiedBuffer range is the range of pH over whi...View AnswerShow Answer

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the Ksp of PbCl2?

Correct AnswerverifiedShow Answer

The solubility of calcium chromate is 1.56 × 10-3 g/100 mL of solution. What is the Ksp for CaCrO4?

Correct AnswerverifiedShow Answer

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate, Cd(NO3) 2. Which of the following statements is correct? Ksp = 6.44 × 10-3 for CdF2.

Correct AnswerverifiedShow Answer

Correct Answer
verified

Correct Answer
verified

Write the ion product expression for calcium phosphate, Ca₃(PO₄) ₂.

Correct Answer
verified

What will be the effect of adding 0.5 mL of 0.1 M NaOH to 100 mL of an acetate buffer in which [CH₃COOH] = [CH₃COO^-] = 0.5 M?

Correct Answer
verified

Correct Answer
verified

Calculate the solubility of silver phosphate, Ag₃PO₄, in pure water. K_sp = 2.6 × 10^-18

Correct Answer
verified

For a diprotic acid H₂A, the relationship K_a1 > K_a2 is always true.

Correct Answer
verified

Correct Answer
verified

What volume of 0.200 M KOH must be added to 17.5 mL of 0.135 M H₃PO₄to reach the third equivalence point?

Correct Answer
verified

Formic acid is a monoprotic acid with a K_a value of 1.8 × 10^-4 at 25°C. a. Calculate the pH of a 0.200 mol L^-1 solution of the acid, making any reasonable approximations. b. If 0.0050 mol of NaOH is added to 100. mL of the solution in (a), calculate the pH of the resultant buffer.

Correct Answer
verified

A 25.0-mL sample of 0.10 M C₂H₃NH₂(ethylamine) is titrated with 0.15 M HCl. What is the pH of the solution after 9.00 mL of acid have been added to the amine? K_b = 6.5 × 10^-4

Correct Answer
verified

The pH of blood is 7.35. It is maintained in part by the buffer system composed of carbonic acid (H₂CO₃) and the bicarbonate (hydrogen carbonate, HCO₃^-) ion. What is the ratio of [bicarbonate]/[carbonic acid] at this pH? For carbonic acid, K_a1 = 4.2 × 10^-7.

Correct Answer
verified

Calculate the solubility of magnesium sulfate, MgSO₄, when placed into a 0.10 M MgCl₂solution. K_sp = 5.9 × 10^-3

Correct Answer
verified

Citric acid has an acid dissociation constant of 8.4 × 10^-4. It would be most effective for preparation of a buffer with a pH of

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
Buffer range is the range of pH over whi...
View Answer

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the K_sp of PbCl₂?

Correct Answer
verified

The solubility of calcium chromate is 1.56 × 10^-3 g/100 mL of solution. What is the K_sp for CaCrO₄?

Correct Answer
verified

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate, Cd(NO₃) ₂. Which of the following statements is correct? K_sp = 6.44 × 10^-3 for CdF₂.

Correct Answer
verified