Question 1

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed

Accepted Answer

A)   0.10 M NH3 and 0.10 M HCl
B)   0.10 M NH4+ and 0.10 M KOH
C)   0.20 M NH3 0.10 M KOH
D)   0.20 M NH3 and 0.10 M HCl
E)   0.20 M NH4+ and 0.10M HCl

Question 2

The pH at the equivalence point of a titration may differ from 7.0 due to

Accepted Answer

A)   the initial concentration of the standard solution.
B)   the indicator used.
C)   the self-ionization of H2O.
D)   the initial pH of the unknown.
E)   hydrolysis of the salt formed.

Question 3

Methyl red is a common acid-base indicator. It has a Ka equal to 6.3 * 10-6. Its un-ionized form is red and its anionic form is yellow. What color would a methyl red solution have at pH = 7.8

Accepted Answer

A)   green
B)   red
C)   blue
D)   yellow
E)   violet

Question 4

The solubility of a salt increases as its Ksp increases.

Accepted Answer

A) True 
 B)False

Question 5

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

Question 6

Which of the following is the most acidic solution

Accepted Answer

A)   0.10 M CH3COOH and 0.10 M CH3COONa
B)   0.10 M CH3COOH
C)   0.10 M HNO2
D)   0.10 M HNO2 and 0.10 M NaNO2
E)   0.10 M CH3COONa

Question 7

Calculate the molar solubility of silver carbonate. (Ksp (Ag2CO3 = 8.1 x 10-12) )

Accepted Answer

A)   1.1 x 10-4 M
B)   1.3 x 10-4 M
C)   1.5 x 10-4 M
D)   1.7 x 10-4 M
E)   None of the above

Question 8

500. mL of a solution containing 1.5 M NH3(aq)  is mixed with 500. mL of a solution containing 0.50M of HCl(aq) . What is the pH of the final solution
(Kb(NH3)  = 1.8 x 10-5)

Accepted Answer

A)   9.16
B)   9.36
C)   9.56
D)   9.76
E)   None of the Above

Question 9

A sample of rainwater collected near a lead smelter is analyzed for acid content. Experiments show that a 100. mL sample of the rainwater is neutralized by 22.4 milliters of 0.0122 M NaOH. Assuming that the acid present is sulfurous acid, which resulted from the reaction of SO2 with water, what is the molarity of acid in the rainwater

Accepted Answer

A)   1.17 * 10-3 M
B)   1.27 * 10-3 M
C)   1.37 * 10-3 M
D)   1.47 * 10-3 M
E)   None of the above

Question 10

The percent ionization of a weak acid HA is greater in a solution containing the salt NaA than it is in a solution of the weak acid only.

Accepted Answer

A) True 
 B)False

Question 11

Calculate the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl. [Ka(HOCl)  = 3.2 * 10-8]

Accepted Answer

A)   0.39
B)   3.94
C)   6.58
D)   7.49
E)   8.40

Question 12

Will a precipitate (ppt)  form when 300. mL of 5.0 * 10-5 M AgNO3 are added to 200. mL of 2.5 * 10-7 M NaBr? Answer yes or no, and identify the precipitate if there is one.

Accepted Answer

A)   Yes, the ppt is AgNO3(s) 
B)   Yes, the ppt is AgBr(s) 
C)   Yes, the ppt is NaBr(s) 
D)   Yes, the ppt is NaNO3(s) 
E)   No, a precipitate will not form

Question 13

A 50.0 mL sample of 2.0 * 10-4 M CuNO3 is added to 50.0 mL of 4.0 M NaCN. The formation constant of the complex ion Cu(CN) 32- is 1.0 * 109. What is the copper(I)  ion concentration in this system at equilibrium

Accepted Answer

A)   2.3 * 10-14 M
B)   1.3 * 10-14 M
C)   1.3 * 10-13 M
D)   2.3 * 10-13 M
E)   None of the above

Question 14

For PbCl2 (Ksp = 2.4 * 10-4) , will a precipitate of PbCl2 form when 0.10 L of 3.0 * 10-2 M Pb(NO3) 2 is added to 400 mL of 9.0 * 10-2 M NaCl

Accepted Answer

A)  Yes, because Q > Ksp.
B)   No, because Q sp.
C)   No, because Q = Ksp
D)   Yes, because Q sp.

Question 15

Calculate the molar solubility of AgBr in a 0.25M solution of NH3(aq)  (Ksp (AgBr)  = 7.7 x 10-13 ; Kf (Ag(NH3) 2+)  = 1.5 x 107.

Accepted Answer

A)   8.8 x 10-7 M
B)   3.4 x 10-3 M
C)   8.4 x 10-4 M
D)   2.5 x 10-1 M
E)   9.7 x 102 M

Question 16

What mass of ammonium nitrate must be added to 350. mL of a 0.150 M solution of ammonia to give a buffer having a pH of 9.00 
(Kb(NH3)  = 1.8 * 10-5)

Accepted Answer

A)   7.6 g
B)   2.4 g
C)   5.4 g
D)   11 g
E)   3.3 g

Question 17

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 18

Which of the following compounds is more soluble in a 0.10 M NaCN solution than in pure neutral water

Accepted Answer

A)   Mg(OH) 2
B)   Ca3(PO4) 2
C)   CaCO3
D)   AgBr
E)   NH4ClO4

Question 19

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH

Accepted Answer

A)   1.0
B)   6.0
C)   7.0
D)   8.0
E)   13.0

Question 20

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

Exam 16: Acid-Base Equilibria and Solubility Equilibria

500. mL of a solution containing 1.5 M NH₃(aq) is mixed with 500. mL of a solution containing 0.50M of HCl(aq) . What is the pH of the final solution (K_b(NH₃) = 1.8 x 10^-5)

Correct Answer
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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
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The solubility of a salt increases as its K_sp increases.

Correct Answer
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Calculate the molar solubility of AgBr in a 0.25M solution of NH₃(aq) (K_sp (AgBr) = 7.7 x 10^-13 ; K_f (Ag(NH₃) ₂⁺) = 1.5 x 10⁷.

Correct Answer
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Which of the following yields a buffer solution when equal volumes of the two solutions are mixed

Correct Answer
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What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH

Correct Answer
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Calculate the molar solubility of silver carbonate. (K_sp (Ag₂CO₃ = 8.1 x 10^-12) )

Correct Answer
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Will a precipitate (ppt) form when 300. mL of 5.0 * 10^-5 M AgNO₃ are added to 200. mL of 2.5 * 10^-7 M NaBr? Answer yes or no, and identify the precipitate if there is one.

Correct Answer
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Which of the following compounds is more soluble in a 0.10 M NaCN solution than in pure neutral water

Correct Answer
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Correct Answer
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The percent ionization of a weak acid HA is greater in a solution containing the salt NaA than it is in a solution of the weak acid only.

Correct Answer
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A 50.0 mL sample of 2.0 * 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. The formation constant of the complex ion Cu(CN) ₃^2- is 1.0 * 10⁹. What is the copper(I) ion concentration in this system at equilibrium

Correct Answer
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Calculate the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl. [K_a(HOCl) = 3.2 * 10^-8]

Correct Answer
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Which of the following is the most acidic solution

Correct Answer
verified

What mass of ammonium nitrate must be added to 350. mL of a 0.150 M solution of ammonia to give a buffer having a pH of 9.00 (K_b(NH₃) = 1.8 * 10^-5)

Correct Answer
verified

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

The pH at the equivalence point of a titration may differ from 7.0 due to

Correct Answer
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For PbCl₂ (K_sp = 2.4 * 10^-4) , will a precipitate of PbCl₂ form when 0.10 L of 3.0 * 10^-2 M Pb(NO₃) ₂ is added to 400 mL of 9.0 * 10^-2 M NaCl

Correct Answer
verified

Methyl red is a common acid-base indicator. It has a K_a equal to 6.3 * 10^-6. Its un-ionized form is red and its anionic form is yellow. What color would a methyl red solution have at pH = 7.8

Correct Answer
verified

Exam 16: Acid-Base Equilibria and Solubility Equilibria

500. mL of a solution containing 1.5 M NH3(aq) is mixed with 500. mL of a solution containing 0.50M of HCl(aq) . What is the pH of the final solution (Kb(NH3) = 1.8 x 10-5)

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

The solubility of a salt increases as its Ksp increases.

Correct AnswerverifiedShow Answer

Calculate the molar solubility of AgBr in a 0.25M solution of NH3(aq) (Ksp (AgBr) = 7.7 x 10-13 ; Kf (Ag(NH3) 2+) = 1.5 x 107.

Correct AnswerverifiedShow Answer

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed

Correct AnswerverifiedShow Answer

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH

Correct AnswerverifiedShow Answer

Calculate the molar solubility of silver carbonate. (Ksp (Ag2CO3 = 8.1 x 10-12) )

Correct AnswerverifiedShow Answer

Will a precipitate (ppt) form when 300. mL of 5.0 * 10-5 M AgNO3 are added to 200. mL of 2.5 * 10-7 M NaBr? Answer yes or no, and identify the precipitate if there is one.

Correct AnswerverifiedShow Answer

Which of the following compounds is more soluble in a 0.10 M NaCN solution than in pure neutral water

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The percent ionization of a weak acid HA is greater in a solution containing the salt NaA than it is in a solution of the weak acid only.

Correct AnswerverifiedShow Answer

A 50.0 mL sample of 2.0 * 10-4 M CuNO3 is added to 50.0 mL of 4.0 M NaCN. The formation constant of the complex ion Cu(CN) 32- is 1.0 * 109. What is the copper(I) ion concentration in this system at equilibrium

Correct AnswerverifiedShow Answer

Calculate the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl. [Ka(HOCl) = 3.2 * 10-8]

Correct AnswerverifiedShow Answer

Which of the following is the most acidic solution

Correct AnswerverifiedShow Answer

What mass of ammonium nitrate must be added to 350. mL of a 0.150 M solution of ammonia to give a buffer having a pH of 9.00 (Kb(NH3) = 1.8 * 10-5)

Correct AnswerverifiedShow 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 AnswerverifiedShow Answer

The pH at the equivalence point of a titration may differ from 7.0 due to

Correct AnswerverifiedShow Answer

For PbCl2 (Ksp = 2.4 * 10-4) , will a precipitate of PbCl2 form when 0.10 L of 3.0 * 10-2 M Pb(NO3) 2 is added to 400 mL of 9.0 * 10-2 M NaCl

Correct AnswerverifiedShow Answer

Methyl red is a common acid-base indicator. It has a Ka equal to 6.3 * 10-6. Its un-ionized form is red and its anionic form is yellow. What color would a methyl red solution have at pH = 7.8

Correct AnswerverifiedShow Answer

500. mL of a solution containing 1.5 M NH₃(aq) is mixed with 500. mL of a solution containing 0.50M of HCl(aq) . What is the pH of the final solution (K_b(NH₃) = 1.8 x 10^-5)

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

The solubility of a salt increases as its K_sp increases.

Correct Answer
verified

Calculate the molar solubility of AgBr in a 0.25M solution of NH₃(aq) (K_sp (AgBr) = 7.7 x 10^-13 ; K_f (Ag(NH₃) ₂⁺) = 1.5 x 10⁷.

Correct Answer
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Correct Answer
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Correct Answer
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Calculate the molar solubility of silver carbonate. (K_sp (Ag₂CO₃ = 8.1 x 10^-12) )

Correct Answer
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Will a precipitate (ppt) form when 300. mL of 5.0 * 10^-5 M AgNO₃ are added to 200. mL of 2.5 * 10^-7 M NaBr? Answer yes or no, and identify the precipitate if there is one.

Correct Answer
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Correct Answer
verified

Correct Answer
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Correct Answer
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A 50.0 mL sample of 2.0 * 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. The formation constant of the complex ion Cu(CN) ₃^2- is 1.0 * 10⁹. What is the copper(I) ion concentration in this system at equilibrium

Correct Answer
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Calculate the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl. [K_a(HOCl) = 3.2 * 10^-8]

Correct Answer
verified

Correct Answer
verified

What mass of ammonium nitrate must be added to 350. mL of a 0.150 M solution of ammonia to give a buffer having a pH of 9.00 (K_b(NH₃) = 1.8 * 10^-5)

Correct Answer
verified

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

Correct Answer
verified

For PbCl₂ (K_sp = 2.4 * 10^-4) , will a precipitate of PbCl₂ form when 0.10 L of 3.0 * 10^-2 M Pb(NO₃) ₂ is added to 400 mL of 9.0 * 10^-2 M NaCl

Correct Answer
verified

Methyl red is a common acid-base indicator. It has a K_a equal to 6.3 * 10^-6. Its un-ionized form is red and its anionic form is yellow. What color would a methyl red solution have at pH = 7.8

Correct Answer
verified