Question 1

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. A

Question 2

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)  11.12 C

Question 3

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 4

Acid dissociation constants for phosphoric acid are given below.  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.

Question 5

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]

Accepted Answer

The answer of Describe how to prepare 500. mL of...

Question 6

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 sp

Question 7

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 M

Question 8

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):

Accepted Answer

The answer of Write an equation showing the net reaction...

Question 9

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)  5.07

Question 10

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)  4.30

Question 11

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 M

Question 12

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 M

Question 13

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 * 10-3

Question 14

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)  12.0

Question 15

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

Accepted Answer

The answer of Describe how to make a sodium formate...

Question 16

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?

Accepted Answer

The answer of The solubility of Ba(NO₃)₂ is 130.5 g/L...

Question 17

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 18

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]

Accepted Answer

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

Question 19

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%

Question 20

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)  13.0

Exam 17: Acid-Base Equilibria and Solubility Equilibria

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?

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) .

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

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

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]

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]

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

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):

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]

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]

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

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.)

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

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?

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

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?

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

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]

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]

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.

Exam 17: Acid-Base Equilibria and Solubility Equilibria

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?

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) .

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

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

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]

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]

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

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):

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]

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]

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

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.)

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

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?

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

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?

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

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]

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]

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.

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?

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) .

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]

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]

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

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):

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]

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]

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

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.)

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

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?

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?

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

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]

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]

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.