Question 1

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

Accepted Answer

Henderson-

Question 2

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 3

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 
A) 5.15 
B) 8.71 
C) 5.85 
D) 9.91 
E) 13.0

Question 4

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 base 
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 base

Question 5

What is the Henderson-Hasselbach equation?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 6

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

Question 7

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 8

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

Question 9

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 M 
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 M

Question 10

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 adduct 
A) Shift ion 
B) Shift reagent 
C) Equilibrium ion 
D) Common ion effect 
E) Ion adduct

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

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

Question 13

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 14

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 15

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 M 
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 M

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

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

Question 18

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 M 
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 M

Question 19

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

Question 20

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) 8.21 
A) 10.26 
B) 9.30 
C) 9.21 
D) 8.30 
E) 8.21

Exam 17: Acid-Base Equilibria and Solubility Equilibria

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

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

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 results in a buffered solution?

What is the Henderson-Hasselbach equation?

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?

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?

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

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

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?

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

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)

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?

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]

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.

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-

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

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

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]

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

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

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.

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?

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

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

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)

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?

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]

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-

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

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

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]