Question 1

Which pair of substances could form a buffered aqueous solution?

Accepted Answer

A)   HCl, NaCl
B)   HNO3, NaNO3
C)   H3PO4, NaH2PO4
D)   H2SO4, CH3COOH
E)   NH3, NaOHF) None of the above
G) A) and E)

Question 2

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. Determine to Ka for HClO. a for HClO.   A)  1.1 × 10-7 B)  3.5 × 10-8 C)  1.2 × 10-8 D)  4.9 × 10-11 E)  None of the answers is correct." class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   1.1 × 10-7
B)   3.5 × 10-8
C)   1.2 × 10-8
D)   4.9 × 10-11
E)   None of the answers is correct.F) C) and D)
G) None of the above

Question 3

Which indicator would be the best to use if 0.050 M benzoic acid (Ka = 6.6 × 10-5)  is titrated with 0.050 M NaOH?

Accepted Answer

A)   bromphenol blue, pH range: 3.0 - 4.5
B)   bromcresol green, pH range: 3.8 - 5.4
C)   alizarin, pH range: 5.7 - 7.2
D)   phenol red, pH range: 6.9 - 8.5E) A) and C)
F) A) and D)

Question 4

A(n) ________ is an ion containing a central metal cation bonded to one or more molecules or ions.

Accepted Answer

The answer of A(n) ________ is an ion containing a...

Question 5

Which of the following is correct?

Accepted Answer

A)   Solubility is the concentration of unsaturated ions in solution.
B)   Ksp is the same as the solubility.
C)   Ksp is an equilibrium constant and solubility is the concentration of a saturated solution.
D)   Ksp is the solubility product constant for a precipitate.
E)   Solubility = Kw × Ksp.F) All of the above
G) A) and B)

Question 6

What is the pH of a buffer that consists of 0.45 M CH3COOH and 0.35 M CH3COONa? [Ka(CH3COOH)  = 1.8 × 10-5]

Accepted Answer

A)   3.43
B)   4.64
C)   4.85
D)   4.74
E)   6.06F) C) and E)
G) A) and B)

Question 7

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

Accepted Answer

A)   is greater than 7.0.
B)   is equal to 7.0.
C)   is between 3.5 and 7.0.
D)   is equal to the pKa of the acid.
E)   is equal to 3.5.F) A) and D)
G) All of the above

Question 8

An indicator is a weak acid that is one color in its protonated form and another color in its deprotonated form.

Accepted Answer

A) True 
 B)False

Question 9

Which combination may be used to prepare a buffer having a pH of 8.8? Ka= 7 × 10-3 for H3PO4; 8 × 10-8 for H2PO4-; 5 × 10-13 for HPO42-

Accepted Answer

A)   NaH2PO4 only
B)   NaH2PO4 and Na2HPO4
C)   Na3PO4 and Na2HPO4
D)   NaHPO4 and H3PO4
E)   H3PO4 and Na3PO4F) B) and D)
G) A) and E)

Question 10

A wildlife biologist is interested in testing the pH of the water in a lake. He obtains a 200.0-mL sample of the lake water and titrates this sample with a 0.050 M NaOH solution. Neutralization of the lake water requires 40.0 mL of the NaOH solution. Assuming that lake water sample only contains a strong acid, estimate the pH of the lake.

Accepted Answer

The answer of A wildlife biologist is interested in testing...

Question 11

Which is more soluble in a basic solution than in pure water?

Accepted Answer

A)   Mg(OH) 2
B)   CaHPO4
C)   NaCl
D)   CaCO3
E)   AgIF) B) and C)
G) B) and D) B

Question 12

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

Accepted Answer

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

Question 13

The molar solubility of tin(II)  iodide is 1.28 × 10-2 mol/L. What is Ksp for this compound?

Accepted Answer

A)   8.39 × 10-6
B)   1.28 × 10-2
C)   4.20 × 10-6
D)   1.64 × 10-4
E)   2.10 × 10-6F) B) and D)
G) B) and C)

Question 14

Which of the following compounds is appreciably more soluble in 1 M HNO3 than in pure water?

Accepted Answer

A)   FeCO3
B)   AgBr
C)   BaSO4
D)   NaNO3
E)   NaClF) A) and B)
G) A) and E)

Question 15

What is the effect on the equilibrium when sodium formate is added to a solution of formic acid? HCOOH(aq)  +(aq)  + HCOO-(aq)  A)  There is no change in the equilibrium. B)  The equilibrium shifts to the right. C)  More information is needed to answer the question. D)  The equilibrium shifts to the left. E)  The pH decreases." class="answers-bank-image d-inline" rel="preload" > H+(aq)  + HCOO-(aq)

Accepted Answer

A)   There is no change in the equilibrium.
B)   The equilibrium shifts to the right.
C)   More information is needed to answer the question.
D)   The equilibrium shifts to the left.
E)   The pH decreases.F) A) and C)
G) None of the above

Question 16

Bromothymol blue is a common acid-base indicator. It has a Ka equal to 1.6 × 10-7. Its un-ionized form is yellow and its conjugate base is blue. What color would a solution have at pH = 5.8?

Accepted Answer

Question 17

The endpoint in a titration is defined as the point when the appropriate indicator changes color.

Accepted Answer

A) True 
 B)False

Question 18

An acetic acid buffer containing 0.50 M CH3COOH and 0.50 M CH3COONa has a pH of 4.74. What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

Accepted Answer

A)   4.77
B)   4.71
C)   4.68
D)   4.62
E)   1.70.F) None of the above
G) A) and B)

Question 19

A 10.0-mL sample of 0.75 M CH3CH2COOH is titrated with 0.30 M NaOH. What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? [Ka(CH3CH2COOH)  = 1.3 × 10-5]

Accepted Answer

A)   5.75
B)   4.94
C)   4.83
D)   4.02
E)   3.95F) C) and D)
G) D) and E) A

Question 20

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)   violetF) A) and E)
G) A) and B)

Exam 17: Acid-Base Equilibria and Solubility Equilibria

Which pair of substances could form a buffered aqueous solution?

Correct Answer
verified

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. Determine to K_a for HClO.

Correct Answer
verified

Which indicator would be the best to use if 0.050 M benzoic acid (K_a = 6.6 × 10^-5) is titrated with 0.050 M NaOH?

Correct Answer
verified

A(n) ________ is an ion containing a central metal cation bonded to one or more molecules or ions.

Correct Answer
verified

Which of the following is correct?

Correct Answer
verified

What is the pH of a buffer that consists of 0.45 M CH₃COOH and 0.35 M CH₃COONa? [K_a(CH₃COOH) = 1.8 × 10^-5]

Correct Answer
verified

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

Correct Answer
verified

An indicator is a weak acid that is one color in its protonated form and another color in its deprotonated form.

Correct Answer
verified

Which combination may be used to prepare a buffer having a pH of 8.8? K_a= 7 × 10^-3 for H₃PO₄; 8 × 10^-8 for H₂PO₄^-; 5 × 10^-13 for HPO₄^2-

Correct Answer
verified

Correct Answer
verified

Which is more soluble in a basic solution than in pure water?

Correct Answer
verified
B

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

Correct Answer
verified
B

The molar solubility of tin(II) iodide is 1.28 × 10^-2 mol/L. What is K_sp for this compound?

Correct Answer
verified

Which of the following compounds is appreciably more soluble in 1 M HNO₃ than in pure water?

Correct Answer
verified

What is the effect on the equilibrium when sodium formate is added to a solution of formic acid? HCOOH(aq) H⁺(aq) + HCOO^-(aq)

Correct Answer
verified

Bromothymol blue is a common acid-base indicator. It has a K_a equal to 1.6 × 10^-7. Its un-ionized form is yellow and its conjugate base is blue. What color would a solution have at pH = 5.8?

Correct Answer
verified

The endpoint in a titration is defined as the point when the appropriate indicator changes color.

Correct Answer
verified

An acetic acid buffer containing 0.50 M CH₃COOH and 0.50 M CH₃COONa has a pH of 4.74. What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

Correct Answer
verified

A 10.0-mL sample of 0.75 M CH₃CH₂COOH is titrated with 0.30 M NaOH. What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? [K_a(CH₃CH₂COOH) = 1.3 × 10^-5]

Correct Answer
verified
A

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 17: Acid-Base Equilibria and Solubility Equilibria

Which pair of substances could form a buffered aqueous solution?

Correct AnswerverifiedShow Answer

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. Determine to Ka for HClO.

Correct AnswerverifiedShow Answer

Which indicator would be the best to use if 0.050 M benzoic acid (Ka = 6.6 × 10-5) is titrated with 0.050 M NaOH?

Correct AnswerverifiedShow Answer

A(n) ________ is an ion containing a central metal cation bonded to one or more molecules or ions.

Correct AnswerverifiedShow Answer

Which of the following is correct?

Correct AnswerverifiedShow Answer

What is the pH of a buffer that consists of 0.45 M CH3COOH and 0.35 M CH3COONa? [Ka(CH3COOH) = 1.8 × 10-5]

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

An indicator is a weak acid that is one color in its protonated form and another color in its deprotonated form.

Correct AnswerverifiedShow Answer

Which combination may be used to prepare a buffer having a pH of 8.8? Ka= 7 × 10-3 for H3PO4; 8 × 10-8 for H2PO4-; 5 × 10-13 for HPO42-

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Which is more soluble in a basic solution than in pure water?

Correct AnswerverifiedB

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

Correct AnswerverifiedB

The molar solubility of tin(II) iodide is 1.28 × 10-2 mol/L. What is Ksp for this compound?

Correct AnswerverifiedShow Answer

Which of the following compounds is appreciably more soluble in 1 M HNO3 than in pure water?

Correct AnswerverifiedShow Answer

What is the effect on the equilibrium when sodium formate is added to a solution of formic acid? HCOOH(aq) H+(aq) + HCOO-(aq)

Correct AnswerverifiedShow Answer

Bromothymol blue is a common acid-base indicator. It has a Ka equal to 1.6 × 10-7. Its un-ionized form is yellow and its conjugate base is blue. What color would a solution have at pH = 5.8?

Correct AnswerverifiedShow Answer

The endpoint in a titration is defined as the point when the appropriate indicator changes color.

Correct AnswerverifiedShow Answer

An acetic acid buffer containing 0.50 M CH3COOH and 0.50 M CH3COONa has a pH of 4.74. What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

Correct AnswerverifiedShow Answer

A 10.0-mL sample of 0.75 M CH3CH2COOH is titrated with 0.30 M NaOH. What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? [Ka(CH3CH2COOH) = 1.3 × 10-5]

Correct AnswerverifiedA

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

Correct Answer
verified

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. Determine to K_a for HClO.

Correct Answer
verified

Which indicator would be the best to use if 0.050 M benzoic acid (K_a = 6.6 × 10^-5) is titrated with 0.050 M NaOH?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

What is the pH of a buffer that consists of 0.45 M CH₃COOH and 0.35 M CH₃COONa? [K_a(CH₃COOH) = 1.8 × 10^-5]

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Which combination may be used to prepare a buffer having a pH of 8.8? K_a= 7 × 10^-3 for H₃PO₄; 8 × 10^-8 for H₂PO₄^-; 5 × 10^-13 for HPO₄^2-

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
B

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

Correct Answer
verified
B

The molar solubility of tin(II) iodide is 1.28 × 10^-2 mol/L. What is K_sp for this compound?

Correct Answer
verified

Which of the following compounds is appreciably more soluble in 1 M HNO₃ than in pure water?

Correct Answer
verified

What is the effect on the equilibrium when sodium formate is added to a solution of formic acid? HCOOH(aq) H⁺(aq) + HCOO^-(aq)

Correct Answer
verified

Bromothymol blue is a common acid-base indicator. It has a K_a equal to 1.6 × 10^-7. Its un-ionized form is yellow and its conjugate base is blue. What color would a solution have at pH = 5.8?

Correct Answer
verified

Correct Answer
verified

An acetic acid buffer containing 0.50 M CH₃COOH and 0.50 M CH₃COONa has a pH of 4.74. What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

Correct Answer
verified

A 10.0-mL sample of 0.75 M CH₃CH₂COOH is titrated with 0.30 M NaOH. What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? [K_a(CH₃CH₂COOH) = 1.3 × 10^-5]

Correct Answer
verified
A

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