Question 1

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The Ka of lactic acid is 1.37 × 10- 4.

Accepted Answer

A)   4.13
B)   3.57
C)   5.48
D)   14.28
E)   10.43F) A) and E)
G) A) and D)

Question 2

Consider the following table of Ksp values. sp values.   -Which compound listed below has the smallest molar solubility in water? A)  CdCO3 B)  CaF2  C)  Cd(OH) 2  D)  ZnCO3  E)  AgI" class="answers-bank-image d-inline" rel="preload" >
-Which compound listed below has the smallest molar solubility in water?

Accepted Answer

A)   CdCO3
B)   CaF2 
C)   Cd(OH) 2 
D)   ZnCO3 
E)   AgIF) C) and D)
G) All of the above

Question 3

In which of the following aqueous solutions would you expect AgCl to have the lowest solubility?

Accepted Answer

A)   0.020 M BaCl2
B)   0.020 KCl
C)   pure water
D)   0.020 AgNO3
E)   0.015 NaClF) C) and E)
G) All of the above

Question 4

A solution is prepared by dissolving 0.23 mol of hydrazoic acid and 0.27 mol of sodium azide in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts with the present in the buffer solution. The Ka of hydrazoic acid is 1.9 × 10- 5.

Accepted Answer

A)   azide
B)   This is a buffer solution:The pH does not change upon addition of acid or base.
C)   H3O+
D)   H2O
E)   hydrazoic acidF) All of the above
G) B) and E)

Question 5

How many milliliters of 0.0850 M NaOH are required to titrate 25.0 mL of 0.0720 M HBr to the equivalence point?

Accepted Answer

A)   3.92
B)   21.2
C)   0.245
D)   0.153
E)   29.5F) A) and C)
G) B) and C)

Question 6

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770 × 10- 5.

Accepted Answer

Question 7

What is the molar solubility of magnesium carbonate ( MgCO3 )  in water? The solubility- product constant for MgCO3 is 3.5 × 10- 8 at 25°C.

Accepted Answer

A)   7.0 × 10- 8 
B)   1.8 × 10- 8 
C)   1.9 × 10- 4 
D)   7.46
E)   2.6 × 10- 4F) All of the above
G) B) and E)

Question 8

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770× 10- 5.

Accepted Answer

Exam 17: Additional Aspects of Equilibria

In which of the following aqueous solutions would you expect AgCl to have the lowest solubility?

Correct Answer
verified

Consider the following table of K_spvalues. -Which compound listed below has the smallest molar solubility in water?

Correct Answer
verified

How many milliliters of 0.0850 M NaOH are required to titrate 25.0 mL of 0.0720 M HBr to the equivalence point?

Correct Answer
verified

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770 × 10^-⁵.

Correct Answer
verified

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The K_aof lactic acid is 1.37 × 10^-⁴.

Correct Answer
verified

What is the molar solubility of magnesium carbonate ( MgCO₃) in water? The solubility- product constant for MgCO₃is 3.5 × 10^-⁸at 25°C.

Correct Answer
verified

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770× 10^-⁵.

Correct Answer
verified

Correct Answer
verified

Exam 17: Additional Aspects of Equilibria

In which of the following aqueous solutions would you expect AgCl to have the lowest solubility?

Correct AnswerverifiedShow Answer

Consider the following table of Ksp values. -Which compound listed below has the smallest molar solubility in water?

Correct AnswerverifiedShow Answer

How many milliliters of 0.0850 M NaOH are required to titrate 25.0 mL of 0.0720 M HBr to the equivalence point?

Correct AnswerverifiedShow Answer

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770 × 10- 5.

Correct AnswerverifiedShow Answer

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The Ka of lactic acid is 1.37 × 10- 4.

Correct AnswerverifiedShow Answer

What is the molar solubility of magnesium carbonate ( MgCO3 ) in water? The solubility- product constant for MgCO3 is 3.5 × 10- 8 at 25°C.

Correct AnswerverifiedShow Answer

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770× 10- 5.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Correct Answer
verified

Consider the following table of K_spvalues. -Which compound listed below has the smallest molar solubility in water?

Correct Answer
verified

Correct Answer
verified

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770 × 10^-⁵.

Correct Answer
verified

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The K_aof lactic acid is 1.37 × 10^-⁴.

Correct Answer
verified

What is the molar solubility of magnesium carbonate ( MgCO₃) in water? The solubility- product constant for MgCO₃is 3.5 × 10^-⁸at 25°C.

Correct Answer
verified

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770× 10^-⁵.

Correct Answer
verified

Correct Answer
verified