Question 1

Will a precipitate (ppt)  form when 20.0 mL of 1.1 × 10-3 M Ba(NO3) 2 are added to 80.0 mL of 8.4 × 10-4M Na2CO3?

Accepted Answer

A)   Yes, the ppt is Ba(NO3) 2.
B)   Yes, the ppt is NaNO3.
C)   Yes, the ppt is BaCO3.
D)   Yes, the ppt is Na2CO3.
E)   No, a precipitate will not form.F) C) and E)
G) C) and D)

Question 2

Describe how to make a sodium formate (HCOONa)/formic acid (HCOOH) buffer that has a pH of 4.77. Ka = 1.7 × 10-4

Accepted Answer

Prepare a solution h...

Question 3

Below is a titration curve for the titration of 50.0 mL of a 0.100 M solution of the weak acid HA with a 0.100 M solution of NaOH. a of HA? A)  4 B)  6 C)  8 D)  9 E)  12" class="answers-bank-image d-inline" rel="preload" > What is the approximate pKa of HA?

Accepted Answer

A)   4
B)   6
C)   8
D)   9
E)   12F) B) and C)
G) B) and D)

Question 4

The endpoint is used to estimate the equivalence point.

Accepted Answer

A) True 
 B)False

Question 5

A 20.00-mL sample of 0.3000 M HBr is titrated with 0.15 M NaOH. What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?

Accepted Answer

A)   1.00
B)   3.13
C)   10.87
D)   11.05
E)   13.14F) A) and E)
G) A) and C)

Question 6

The "p" of the pH equation and pKa equation represents ________.

Accepted Answer

Question 7

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

Accepted Answer

Henderson-...

Question 8

The amount of strong acid added to a buffer solution cannot exceed the original amount of conjugate base present in order for the buffer to still work.

Accepted Answer

A) True 
 B)False

Question 9

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH)  and 0.20 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(CH3COOH)  = 1.8 × 10-5]

Accepted Answer

A)   4.65
B)   4.71
C)   4.56
D)   4.84
E)   5.07F) B) and E)
G) A) and E)

Question 10

When the concentration of the conjugate base of a weak acid is less than the concentration of the weak acid in a buffer solution, the pH of the solution is

Accepted Answer

A)   lower than the pKa.
B)   higher than the pKa.
C)   always acidic.
D)   always basic.
E)   equal to the pKa.F) A) and B)
G) B) and C)

Question 11

What name is given to a solution that contains a weak acid and its conjugate base?

Accepted Answer

The answer of What name is given to a solution...

Question 12

After 50.0 mL of a 0.100 M solution of NaOH is added to 50.0 mL of a 0.100 M solution of an unknown acid, the equilibrium pH is basic. What may be concluded about the identity of the acid?

Accepted Answer

A)   The acid can only be a strong monoprotic acid.
B)   The acid can only be a weak monoprotic acid.
C)   The acid must be a strong acid, but could be either monoprotic, diprotic, or polyprotic.
D)   The acid must be a weak acid, but could be either monoprotic, diprotic, or polyprotic.
E)   The acid could be either a strong or weak acid, and could be either a monoprotic, diprotic, orpolyprotic acid.F) B) and C)
G) D) and E)

Question 13

A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH3COOH. What is the pH of this buffer? [Ka(CH3COOH)  = 1.8 × 10-5]

Accepted Answer

A)   4.57
B)   4.52
C)   4.87
D)   4.92
E)   4.97F) B) and E)
G) A) and E)

Question 14

When an acid, HA, is titrated with 0.1 M NaOH, the pH at the half equivalence point of the titration is 4.5. What is the Ka of the acid?

Accepted Answer

A)   3.2 x 10-5
B)   3.2 x 10-10
C)   1.8 x 10-3
D)   7.0 x 10-7
E)   HA is a strong acidF) A) and E)
G) B) and C)

Question 15

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

Accepted Answer

A)   AgF
B)   AgCN
C)   CO2
D)   NaCl
E)   CH3COOKF) A) and B)
G) A) and E)

Question 16

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 17

Write the ion product expression for calcium phosphate, Ca3(PO4) 2.

Accepted Answer

A)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)   (3 × [Ca2+]) (2 × [PO43- ]" class="answers-bank-image d-inline" rel="preload" >
B)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)   (3 × [Ca2+]) (2 × [PO43- ]" class="answers-bank-image d-inline" rel="preload" >
C)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)   (3 × [Ca2+]) (2 × [PO43- ]" class="answers-bank-image d-inline" rel="preload" >
D)   3(PO4) 2. 
A)     
B)     
C)     
D)     
E)   (3 × [Ca2+]) (2 × [PO43- ]" class="answers-bank-image d-inline" rel="preload" >
E)   (3 × [Ca2+]) (2 × [PO43- ]F) B) and C)
G) B) and E)

Question 18

What is the name 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 E)
G) A) and B)

Question 19

Calculate the pH at the equivalence point for the titration of 50.0 mL of 0.20 M NH3 with 0.20 M HCl. [Kb(NH3)  = 1.8 × 10-5]

Accepted Answer

A)   2.87
B)   4.98
C)   5.13
D)   7.00
E)   11.13F) A) and C)
G) A) and E)

Question 20

Suppose 50.0 mL of a 0.100 M solution of the weak acid HA is titrated with a 0.100 M solution of NaOH. Which diagram best represents the equilibrium composition of the solution at point X on the titration curve below? (Solvent water molecules are omitted for clarity.)

Accepted Answer

A)   
B)   
C)   
D)   
E)   F) None of the above
G) All of the above

Exam 17: Acid-Base Equilibria and Solubility Equilibria

Suppose 50.0 mL of a 0.100 M solution of the weak acid HA is titrated with a 0.100 M solution of NaOH. Which diagram best represents the equilibrium composition of the solution at point X on the titration curve below? (Solvent water molecules are omitted for clarity.)

Correct AnswerverifiedShow Answer

Write the ion product expression for calcium phosphate, Ca3(PO4) 2.

Correct AnswerverifiedShow Answer

Calculate the pH at the equivalence point for the titration of 50.0 mL of 0.20 M NH3 with 0.20 M HCl. [Kb(NH3) = 1.8 × 10-5]

Correct AnswerverifiedShow Answer

Describe how to make a sodium formate (HCOONa)/formic acid (HCOOH) buffer that has a pH of 4.77. Ka = 1.7 × 10-4

Correct AnswerverifiedPrepare a solution h...View AnswerShow Answer

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH) and 0.20 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(CH3COOH) = 1.8 × 10-5]

Correct AnswerverifiedShow Answer

What is the name 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

A 20.00-mL sample of 0.3000 M HBr is titrated with 0.15 M NaOH. What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?

Correct AnswerverifiedShow Answer

Will a precipitate (ppt) form when 20.0 mL of 1.1 × 10-3 M Ba(NO3) 2 are added to 80.0 mL of 8.4 × 10-4M Na2CO3?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

The amount of strong acid added to a buffer solution cannot exceed the original amount of conjugate base present in order for the buffer to still work.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedHenderson-...View AnswerShow Answer

Below is a titration curve for the titration of 50.0 mL of a 0.100 M solution of the weak acid HA with a 0.100 M solution of NaOH. What is the approximate pKa of HA?

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

A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH3COOH. What is the pH of this buffer? [Ka(CH3COOH) = 1.8 × 10-5]

Correct AnswerverifiedShow Answer

The "p" of the pH equation and pKa equation represents ________.

Correct AnswerverifiedShow Answer

When the concentration of the conjugate base of a weak acid is less than the concentration of the weak acid in a buffer solution, the pH of the solution is

Correct AnswerverifiedShow Answer

After 50.0 mL of a 0.100 M solution of NaOH is added to 50.0 mL of a 0.100 M solution of an unknown acid, the equilibrium pH is basic. What may be concluded about the identity of the acid?

Correct AnswerverifiedShow Answer

When an acid, HA, is titrated with 0.1 M NaOH, the pH at the half equivalence point of the titration is 4.5. What is the Ka of the acid?

Correct AnswerverifiedShow Answer

The endpoint is used to estimate the equivalence point.

Correct AnswerverifiedShow Answer

What name is given to a solution that contains a weak acid and its conjugate base?

Correct AnswerverifiedShow Answer

Correct Answer
verified

Write the ion product expression for calcium phosphate, Ca₃(PO₄) ₂.

Correct Answer
verified

Calculate the pH at the equivalence point for the titration of 50.0 mL of 0.20 M NH₃ with 0.20 M HCl. [K_b(NH₃) = 1.8 × 10^-5]

Correct Answer
verified

Describe how to make a sodium formate (HCOONa)/formic acid (HCOOH) buffer that has a pH of 4.77. K_a = 1.7 × 10^-4

Correct Answer
verified
Prepare a solution h...
View Answer

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH₃COOH) and 0.20 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(CH₃COOH) = 1.8 × 10^-5]

Correct Answer
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Correct Answer
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Correct Answer
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Will a precipitate (ppt) form when 20.0 mL of 1.1 × 10^-3^MBa(NO₃) ₂ are added to 80.0 mL of 8.4 × 10^-4^M Na₂CO₃?

Correct Answer
verified

Correct Answer
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Correct Answer
verified

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

Correct Answer
verified
Henderson-...
View Answer

Below is a titration curve for the titration of 50.0 mL of a 0.100 M solution of the weak acid HA with a 0.100 M solution of NaOH. What is the approximate pK_a of HA?

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

A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH₃COOH. What is the pH of this buffer? [K_a(CH₃COOH) = 1.8 × 10^-5]

Correct Answer
verified

The "p" of the pH equation and pK_a equation represents ________.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

When an acid, HA, is titrated with 0.1 M NaOH, the pH at the half equivalence point of the titration is 4.5. What is the K_a of the acid?

Correct Answer
verified

Correct Answer
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Correct Answer
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