Question 1

Calculate the minimum concentration of Mg2+ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride.[Ksp(MgF2) = 6.9 × 10-9] rev: 08_14_2014_QC_52437

Accepted Answer

A)  1.4 × 107 M
B)  6.9 × 10-9 M
C)  6.9 × 10-8 M
D)  1.7 × 10-7 M
E)  6.9 × 10-7 MF) A) and B)
G) A) and D)

Question 2

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 D)
G) B) and E)

Question 3

A wildlife biologist is interested in testing the pH of the water in a lake.He obtains a 200.0-mL
sample of the 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.Is the lake acidic,basic,or neutral?

Accepted Answer

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

Question 4

mL of 0.150 M KI? [Ksp(PbI2) =1.4 × 10-8]

Accepted Answer

A)  2.2 × 10-2 M
B)  1.5 × 10-7 M
C)  6.2 × 10-7 M
D)  9.3 × 10-8 M
E)  1.4 × 10-8 MF) B) and E)
G) C) and E)

Question 5

What is the name is used to describe the situation when a compound containing an ion in common with a dissolved substance is added to a solution at equilibrium which shifts the equilibrium?

Accepted Answer

A)  Shift ion
B)  Shift reagent
C)  Equilibrium ion
D)  Common ion effect
E)  Ion adductF) C) and D)
G) A) and B)

Question 6

The solubility of lead(II) iodide is 0.064 g/100 mL at 20°C.What is the solubility product for lead(II) iodide?

Accepted Answer

A)  1.1 × 10-8
B)  2.7 × 10-9
C)  1.1 × 10-11
D)  2.7 × 10-12
E)  1.1 × 10-3F) A) and E)
G) A) and D)

Question 7

The indicator propyl red has Ka = 3.3 × 10-6.What would be the approximate pH range over which it would change color?

Accepted Answer

A)  3.5 - 5.5
B)  4.5 - 6.5
C)  5.5 - 7.5
D)  6.5 - 8.5
E)  7.5 - 9.5F) D) and E)
G) B) and C)

Question 8

40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH.After 20.0 mL of the base solution has been added,the pH in the titration flask is 5.10.What was the concentration of the original acetic acid solution? (Ka(CH3COOH) = 1.8 × 10-5)

Accepted Answer

A)  0.11 M
B)  0.022 M
C)  0.072 M
D)  0.050 M
E)  0.015 MF) B) and C)
G) A) and E)

Question 9

Propanoic acid (CH3CH2COOH)has a Ka of 1.34 × 10-5.A 25.00-mL sample of 0.1000 mol • L-1
propanoic acid (in flask)is titrated with 0.1000 mol • L-1 NaOH solution,added from a buret.Carry out the calculations of the quantities indicated below.
a.The pH after 0.00 mL of NaOH is added.
b.The pH after 15.00 mL of NaOH is added.

Accepted Answer

Question 10

NaCl is added slowly to a solution that is 0.010 M each in Cu+,Ag+,and Au+.The Ksp for CuCl,
AgCl,and AuCl are 1.9 × 10-7,1.8 × 10-10,and 2.0 × 10-13,respectively.Which compound will precipitate first?

Accepted Answer

Question 11

A CH3COOH/CH3COO- buffer can be produced by adding a strong acid to a solution of CH3COO- ions.

Accepted Answer

A) True 
 B)False

Question 12

Which 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 HP O42-

Accepted Answer

A)  NaH2PO4 only
B)  NaH2PO4 and Na2HPO4
C)  Na3PO4 and Na2HPO4
D)  NaHPO4 and H3PO4
E)  H3PO4 and Na3PO4F) None of the above
G) B) and C)

Question 13

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 B)
F) None of the above

Question 14

pH = pKa + log [conjugate base]/[weak acid] is the ______-______ equation.

Accepted Answer

Henderson-...

Question 15

After the equivalence point,the titration curve of a weak acid is identical to that of a ______ ______.

Accepted Answer

The answer of After the equivalence point,the titration curve of...

Question 16

A(n)___________________ occurs when a compound containing an ion in common with a dissolved substance is added to a solution at equilibrium resulting in a shift of the equilibrium to the left.

Accepted Answer

The answer of A(n)___________________ occurs when a compound containing an...

Question 17

What is the Henderson-Hasselbach equation?

Accepted Answer

A)   
B)   
C)   
D)   
E)   F) A) and D)
G) B) and D)

Question 18

A 25.0-mL sample of 1.00 M NH3 is titrated with 0.15 M HCl.What is the pH of the solution after 15.00 mL of acid have been added to the ammonia solution? [Kb(NH3) = 1.8 × 10-5]

Accepted Answer

A)  10.26
B)  9.30
C)  9.21
D)  8.30
E)  8.21F) A) and B)
G) A) and C)

Question 19

Which results in a buffered solution?

Accepted Answer

A)  A solution containing a strong acid and its conjugate base
B)  A solution containing a strong base and its conjugate acid
C)  A solution containing a catalyst
D)  A solution containing two organic liquids
E)  A solution containing a weak acid and its conjugate baseF) C) and E)
G) A) and B)

Question 20

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? [Ka(HCOOH) = 1.7 × 10-4]

Accepted Answer

A)  1.1 × 10-4 M
B)  2.6 × 10-4 M
C)  4.3 × 10-4 M
D)  6.7 × 10-5 M
E)  1.7 × 10-4 MF) None of the above
G) C) and E)

Exam 17: Acid-Base Equilibria and Solubility Equilibria

A wildlife biologist is interested in testing the pH of the water in a lake.He obtains a 200.0-mL sample of the 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.Is the lake acidic,basic,or neutral?

Correct Answer
verified

A 25.0-mL sample of 1.00 M NH₃ is titrated with 0.15 M HCl.What is the pH of the solution after 15.00 mL of acid have been added to the ammonia solution? [K_b(NH₃) = 1.8 × 10^-5]

Correct Answer
verified

NaCl is added slowly to a solution that is 0.010 M each in Cu⁺,Ag⁺,and Au⁺.The K_sp for CuCl, AgCl,and AuCl are 1.9 × 10^-7,1.8 × 10^-10,and 2.0 × 10^-13,respectively.Which compound will precipitate first?

Correct Answer
verified

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

A(n)___________________ occurs when a compound containing an ion in common with a dissolved substance is added to a solution at equilibrium resulting in a shift of the equilibrium to the left.

Correct Answer
verified

What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? [K_a(HCOOH) = 1.7 × 10^-4]

Correct Answer
verified

The solubility of lead(II) iodide is 0.064 g/100 mL at 20°C.What is the solubility product for lead(II) iodide?

Correct Answer
verified

Which 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 HP O₄^2-

Correct Answer
verified

40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH.After 20.0 mL of the base solution has been added,the pH in the titration flask is 5.10.What was the concentration of the original acetic acid solution? (K_a(CH₃COOH) = 1.8 × 10^-5)

Correct Answer
verified

The indicator propyl red has K_a = 3.3 × 10^-6.What would be the approximate pH range over which it would change color?

Correct Answer
verified

After the equivalence point,the titration curve of a weak acid is identical to that of a .

Correct Answer
verified

Correct Answer
verified

What is the name is used to describe the situation when a compound containing an ion in common with a dissolved substance is added to a solution at equilibrium which shifts the equilibrium?

Correct Answer
verified

What is the Henderson-Hasselbach equation?

Correct Answer
verified

Calculate the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride.[K_sp(MgF₂) = 6.9 × 10^-9] rev: 08_14_2014_QC_52437

Correct Answer
verified

mL of 0.150 M KI? [K_sp(PbI₂) =1.4 × 10^-8]

Correct Answer
verified

pH = pK_a + log [conjugate base]/[weak acid] is the - equation.

Correct Answer
verified
Henderson-...
View Answer

For PbCl₂ (K_sp = 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 Answer
verified

A CH₃COOH/CH₃COO^- buffer can be produced by adding a strong acid to a solution of CH₃COO^-ions.

Correct Answer
verified

Which results in a buffered solution?

Correct Answer
verified

Exam 17: Acid-Base Equilibria and Solubility Equilibria

A wildlife biologist is interested in testing the pH of the water in a lake.He obtains a 200.0-mL sample of the 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.Is the lake acidic,basic,or neutral?

Correct AnswerverifiedShow Answer

A 25.0-mL sample of 1.00 M NH3 is titrated with 0.15 M HCl.What is the pH of the solution after 15.00 mL of acid have been added to the ammonia solution? [Kb(NH3) = 1.8 × 10-5]

Correct AnswerverifiedShow Answer

NaCl is added slowly to a solution that is 0.010 M each in Cu+,Ag+,and Au+.The Ksp for CuCl, AgCl,and AuCl are 1.9 × 10-7,1.8 × 10-10,and 2.0 × 10-13,respectively.Which compound will precipitate first?

Correct AnswerverifiedShow Answer

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

A(n)___________________ occurs when a compound containing an ion in common with a dissolved substance is added to a solution at equilibrium resulting in a shift of the equilibrium to the left.

Correct AnswerverifiedShow Answer

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? [Ka(HCOOH) = 1.7 × 10-4]

Correct AnswerverifiedShow Answer

The solubility of lead(II) iodide is 0.064 g/100 mL at 20°C.What is the solubility product for lead(II) iodide?

Correct AnswerverifiedShow Answer

Which 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 HP O42-

Correct AnswerverifiedShow Answer

40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH.After 20.0 mL of the base solution has been added,the pH in the titration flask is 5.10.What was the concentration of the original acetic acid solution? (Ka(CH3COOH) = 1.8 × 10-5)

Correct AnswerverifiedShow Answer

The indicator propyl red has Ka = 3.3 × 10-6.What would be the approximate pH range over which it would change color?

Correct AnswerverifiedShow Answer

After the equivalence point,the titration curve of a weak acid is identical to that of a ______ ______.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

What is the name is used to describe the situation when a compound containing an ion in common with a dissolved substance is added to a solution at equilibrium which shifts the equilibrium?

Correct AnswerverifiedShow Answer

What is the Henderson-Hasselbach equation?

Correct AnswerverifiedShow Answer

Calculate the minimum concentration of Mg2+ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride.[Ksp(MgF2) = 6.9 × 10-9] rev: 08_14_2014_QC_52437

Correct AnswerverifiedShow Answer

mL of 0.150 M KI? [Ksp(PbI2) =1.4 × 10-8]

Correct AnswerverifiedShow Answer

pH = pKa + log [conjugate base]/[weak acid] is the ______-______ equation.

Correct AnswerverifiedHenderson-...View AnswerShow Answer

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 AnswerverifiedShow Answer

A CH3COOH/CH3COO- buffer can be produced by adding a strong acid to a solution of CH3COO- ions.

Correct AnswerverifiedShow Answer

Which results in a buffered solution?

Correct AnswerverifiedShow Answer

Correct Answer
verified

A 25.0-mL sample of 1.00 M NH₃ is titrated with 0.15 M HCl.What is the pH of the solution after 15.00 mL of acid have been added to the ammonia solution? [K_b(NH₃) = 1.8 × 10^-5]

Correct Answer
verified

NaCl is added slowly to a solution that is 0.010 M each in Cu⁺,Ag⁺,and Au⁺.The K_sp for CuCl, AgCl,and AuCl are 1.9 × 10^-7,1.8 × 10^-10,and 2.0 × 10^-13,respectively.Which compound will precipitate first?

Correct Answer
verified

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

Correct Answer
verified

What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? [K_a(HCOOH) = 1.7 × 10^-4]

Correct Answer
verified

Correct Answer
verified

Which 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 HP O₄^2-

Correct Answer
verified

40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH.After 20.0 mL of the base solution has been added,the pH in the titration flask is 5.10.What was the concentration of the original acetic acid solution? (K_a(CH₃COOH) = 1.8 × 10^-5)

Correct Answer
verified

The indicator propyl red has K_a = 3.3 × 10^-6.What would be the approximate pH range over which it would change color?

Correct Answer
verified

After the equivalence point,the titration curve of a weak acid is identical to that of a .

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Calculate the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride.[K_sp(MgF₂) = 6.9 × 10^-9] rev: 08_14_2014_QC_52437

Correct Answer
verified

mL of 0.150 M KI? [K_sp(PbI₂) =1.4 × 10^-8]

Correct Answer
verified

pH = pK_a + log [conjugate base]/[weak acid] is the - equation.

Correct Answer
verified
Henderson-...
View Answer

For PbCl₂ (K_sp = 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 Answer
verified

A CH₃COOH/CH₃COO^- buffer can be produced by adding a strong acid to a solution of CH₃COO^-ions.

Correct Answer
verified

Correct Answer
verified