Question 1

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C6H5COOH) is added 1.00 mL of 12.0 M HCl. What is the percentage ionization of the benzoic acid in the resulting solution? [Ka(C6H5COOH) = 6.5 * 10-5]

Accepted Answer

A)  3.3%
B)  12%
C)  1.3%
D)  0.52%
E)  0.065%F) A) and D)
G) D) and E)

Question 2

Acid dissociation constants for phosphoric acid are given below. 3PO4 and NaH2PO4. B) NaH2PO4 and Na2HPO4. C) Na2HPO4 and Na3PO4. D) only NaH2PO4. E) only Na2HPO4." class="answers-bank-image d-inline" rel="preload" > A buffer with a pH = 7.4 can best be made by using

Accepted Answer

A)  H3PO4 and NaH2PO4.
B)  NaH2PO4 and Na2HPO4.
C)  Na2HPO4 and Na3PO4.
D)  only NaH2PO4.
E)  only Na2HPO4.F) B) and D)
G) None of the above

Question 3

A mixture made from 10 mL of 1 M HCl and 20 mL of 1 M CH3COONa would be classified as a buffer solution.

Accepted Answer

A) True 
 B)False

Question 4

All indicators are weak acids that are one color in acidic solution and another color in basic solution.

Accepted Answer

A) True 
 B)False  False

Question 5

Will a precipitate of magnesium fluoride form when 300. mL of 1.1 * 10-3 M MgCl2 are added to 500. mL of 1.2 * 10-3 M NaF? [Ksp (MgF2) = 6.9 * 10-9]

Accepted Answer

A)  Yes, Q > Ksp
B)  No, Q sp
C)  No, Q = Ksp
D)  Yes, Q spE) B) and D)
F) A) and D)

Question 6

Calculate the minimum concentration of Cr3+ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride. (For CrF3 , Ksp = 6.6 * 10-11.)

Accepted Answer

A)  0.023 M
B)  0.032 M
C)  7.7 * 10-8 M
D)  2.9 * 10-9 M
E)  6.9 * 10-10 MF) A) and E)
G) A) and C)

Question 7

Will a precipitate of AgCl form when 0.050 mol NaCl(s)and 0.050 mol AgNO3(s)are dissolved in 500. mL of 3.0 M NH3? [Kf for Ag(NH3)2+ is 1.5 * 107; Ksp(AgCl)= 1.6 * 10-10]

Accepted Answer

The answer of Will a precipitate of AgCl form when...

Question 8

Write an equation showing the net reaction that occurs when a strong base is added to a CO32-/HCO3-  buffer solution (for carbonic acid, Ka1 = 4.2 * 10-7, Ka2 = 2.4 * 10-8):

Accepted Answer

HCO<sub>3</sub><sup>...

Question 9

Describe how to prepare 500. mL of a cyanic acid (HCNO)/sodium cyanate (NaCNO)buffer having a pH of 4.80. [Ka(HCNO)= 2.0 * 10-4]

Accepted Answer

Dissolve amounts of the two compounds eq...

Question 10

Describe how to make a sodium formate (HCOONa)/formic acid (HCOOH)buffer that has a pH of 4.77.

Accepted Answer

Prepare a solution h...

Question 11

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution. [Ka(HCNO) = 2.0 * 10-4]

Accepted Answer

A)  0.97
B)  3.10
C)  4.40
D)  3.70
E)  4.30F) None of the above
G) D) and E)

Question 12

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na2CrO4 are added to 250 mL of 0.12 M AgNO3? [Ksp(Ag2CrO4) = 1.1 * 10-12] What is the concentration of the silver ion remaining in solution?

Accepted Answer

A)  Yes, [Ag+] = 2.9 * 10-6 M.
B)  Yes, [Ag+] = 0.060 M.
C)  Yes, [Ag+] = 1.3 * 10-4 M.
D)  No, [Ag+] = 0.060 M.
E)  No, [Ag+] = 0.105 M.F) B) and D)
G) C) and E) A

Question 13

Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH3 (Kb = 1.8 * 10-5) .

Accepted Answer

A)  2.87
B)  4.98
C)  5.12
D)  7.00
E)  11.12F) B) and C)
G) A) and D) C

Question 14

Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 * 10-10) solution.

Accepted Answer

A)  5.15
B)  8.71
C)  5.85
D)  9.91
E)  13.0F) A) and E)
G) A) and C)

Question 15

Calculate the concentration of chloride ions in a saturated lead(II) chloride (Ksp = 2.4 * 10-4) solution.

Accepted Answer

A)  2.4 * 10-4 M
B)  4.8 * 10-4 M
C)  3.9 * 10-2 M
D)  1.2 * 10-1 M
E)  7.8 * 10-2 MF) A) and B)
G) None of the above

Question 16

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCN (Ka = 4.9 * 10-10) with 0.10 M NaOH?

Accepted Answer

A)  3.0
B)  6.0
C)  7.0
D)  11.0
E)  12.0F) A) and B)
G) A) and C)

Question 17

The solubility of strontium carbonate is 0.0011 g/100 mL at 20oC. Calculate the Ksp value for this compound.

Accepted Answer

A)  7.5 * 10-5
B)  1.5 * 10-4
C)  5.6 * 10-9
D)  7.5 * 10-6
E)  1.5 * 10-3F) A) and D)
G) C) and E)

Question 18

The solubility product for chromium(III) fluoride is Ksp = 6.6 * 10-11. What is the molar solubility of chromium(III) fluoride?

Accepted Answer

A)  1.6 * 10-3 M
B)  1.2 * 10-3 M
C)  6.6 * 10-11 M
D)  2.2 * 10-3 M
E)  1.6 * 10-6 MF) A) and B)
G) A) and C)

Question 19

The solubility of Ba(NO3)2 is 130.5 g/L at 0oC. How many moles of dissolved salt are present in 4.0 L of a saturated solution of Ba(NO3)2 at 0oC?

Accepted Answer

Question 20

You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONa) . What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [Ka = 1.8 * 10-5]

Accepted Answer

A)  4.41
B)  4.74
C)  4.56
D)  4.92
E)  5.07F) B) and D)
G) A) and E)

Exam 17: Acid-Base Equilibria and Solubility Equilibria

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C6H5COOH) is added 1.00 mL of 12.0 M HCl. What is the percentage ionization of the benzoic acid in the resulting solution? [Ka(C6H5COOH) = 6.5 * 10-5]

Correct AnswerverifiedShow Answer

Acid dissociation constants for phosphoric acid are given below. A buffer with a pH = 7.4 can best be made by using

Correct AnswerverifiedShow Answer

A mixture made from 10 mL of 1 M HCl and 20 mL of 1 M CH3COONa would be classified as a buffer solution.

Correct AnswerverifiedShow Answer

All indicators are weak acids that are one color in acidic solution and another color in basic solution.

Correct AnswerverifiedFalse

Will a precipitate of magnesium fluoride form when 300. mL of 1.1 * 10-3 M MgCl2 are added to 500. mL of 1.2 * 10-3 M NaF? [Ksp (MgF2) = 6.9 * 10-9]

Correct AnswerverifiedShow Answer

Calculate the minimum concentration of Cr3+ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride. (For CrF3 , Ksp = 6.6 * 10-11.)

Correct AnswerverifiedShow Answer

Will a precipitate of AgCl form when 0.050 mol NaCl(s)and 0.050 mol AgNO3(s)are dissolved in 500. mL of 3.0 M NH3? [Kf for Ag(NH3)2+ is 1.5 * 107; Ksp(AgCl)= 1.6 * 10-10]

Correct AnswerverifiedShow Answer

Write an equation showing the net reaction that occurs when a strong base is added to a CO32-/HCO3- buffer solution (for carbonic acid, Ka1 = 4.2 * 10-7, Ka2 = 2.4 * 10-8):

Correct AnswerverifiedHCO3...View AnswerShow Answer

Describe how to prepare 500. mL of a cyanic acid (HCNO)/sodium cyanate (NaCNO)buffer having a pH of 4.80. [Ka(HCNO)= 2.0 * 10-4]

Correct AnswerverifiedDissolve amounts of the two compounds eq...View AnswerShow Answer

Describe how to make a sodium formate (HCOONa)/formic acid (HCOOH)buffer that has a pH of 4.77.

Correct AnswerverifiedPrepare a solution h...View AnswerShow Answer

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution. [Ka(HCNO) = 2.0 * 10-4]

Correct AnswerverifiedShow Answer

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na2CrO4 are added to 250 mL of 0.12 M AgNO3? [Ksp(Ag2CrO4) = 1.1 * 10-12] What is the concentration of the silver ion remaining in solution?

Correct AnswerverifiedA

Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH3 (Kb = 1.8 * 10-5) .

Correct AnswerverifiedC

Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 * 10-10) solution.

Correct AnswerverifiedShow Answer

Calculate the concentration of chloride ions in a saturated lead(II) chloride (Ksp = 2.4 * 10-4) solution.

Correct AnswerverifiedShow Answer

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCN (Ka = 4.9 * 10-10) with 0.10 M NaOH?

Correct AnswerverifiedShow Answer

The solubility of strontium carbonate is 0.0011 g/100 mL at 20oC. Calculate the Ksp value for this compound.

Correct AnswerverifiedShow Answer

The solubility product for chromium(III) fluoride is Ksp = 6.6 * 10-11. What is the molar solubility of chromium(III) fluoride?

Correct AnswerverifiedShow Answer

The solubility of Ba(NO3)2 is 130.5 g/L at 0oC. How many moles of dissolved salt are present in 4.0 L of a saturated solution of Ba(NO3)2 at 0oC?

Correct AnswerverifiedShow Answer

You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONa) . What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [Ka = 1.8 * 10-5]

Correct AnswerverifiedShow Answer

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C₆H₅COOH) is added 1.00 mL of 12.0 M HCl. What is the percentage ionization of the benzoic acid in the resulting solution? [K_a(C₆H₅COOH) = 6.5 * 10^-5]

Correct Answer
verified

Correct Answer
verified

A mixture made from 10 mL of 1 M HCl and 20 mL of 1 M CH₃COONa would be classified as a buffer solution.

Correct Answer
verified

Correct Answer
verified
False

Will a precipitate of magnesium fluoride form when 300. mL of 1.1 * 10^-3 M MgCl₂ are added to 500. mL of 1.2 * 10^-3 M NaF? [K_sp (MgF₂) = 6.9 * 10^-9]

Correct Answer
verified

Calculate the minimum concentration of Cr³⁺ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride. (For CrF₃, K_sp = 6.6 * 10^-11.)

Correct Answer
verified

Will a precipitate of AgCl form when 0.050 mol NaCl(s)and 0.050 mol AgNO₃(s)are dissolved in 500. mL of 3.0 M NH₃? [K_fforAg(NH₃)₂⁺is 1.5 * 10⁷; K_sp(AgCl)= 1.6 * 10^-10]

Correct Answer
verified

Write an equation showing the net reaction that occurs when a strong base is added to a CO₃^2-/HCO₃^- buffer solution (for carbonic acid, K_a1 = 4.2 * 10^-7, K_a2 = 2.4 * 10^-8):

Correct Answer
verified
HCO₃^...
View Answer

Describe how to prepare 500. mL of a cyanic acid (HCNO)/sodium cyanate (NaCNO)buffer having a pH of 4.80. [K_a(HCNO)= 2.0 * 10^-4]

Correct Answer
verified
Dissolve amounts of the two compounds eq...
View Answer

Correct Answer
verified
Prepare a solution h...
View Answer

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution. [K_a(HCNO) = 2.0 * 10^-4]

Correct Answer
verified

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na₂CrO₄ are added to 250 mL of 0.12 M AgNO₃? [K_sp(Ag₂CrO₄) = 1.1 * 10^-12] What is the concentration of the silver ion remaining in solution?

Correct Answer
verified
A

Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH₃ (K_b = 1.8 * 10^-5) .

Correct Answer
verified
C

Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (K_a = 4.9 * 10^-10) solution.

Correct Answer
verified

Calculate the concentration of chloride ions in a saturated lead(II) chloride (K_sp = 2.4 * 10^-4) solution.

Correct Answer
verified

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCN (K_a = 4.9 * 10^-10) with 0.10 M NaOH?

Correct Answer
verified

The solubility of strontium carbonate is 0.0011 g/100 mL at 20^oC. Calculate the K_sp value for this compound.

Correct Answer
verified

The solubility product for chromium(III) fluoride is K_sp = 6.6 * 10^-11. What is the molar solubility of chromium(III) fluoride?

Correct Answer
verified

The solubility of Ba(NO₃)₂ is 130.5 g/L at 0^oC. How many moles of dissolved salt are present in 4.0 L of a saturated solution of Ba(NO₃)₂ at 0^oC?

Correct Answer
verified

You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH₃COOH) and 0.30 M sodium acetate (CH₃COONa) . What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [K_a = 1.8 * 10^-5]

Correct Answer
verified