4) Does the pH increase, decrease or remain the same on the addition of the of t

Question

4) Does the pH increase, decrease or remain the same on the addition of the of the following?

LiF to and HF solution

KI to and HI solution

NH4Cl to and NH3 solution

HBr to an CH3COO-/CH3COOH (acetic acid/acetate buffer) solution

Remain the same

Decrease

Increase

5) Which of the following (select all that apply) gives a buffer solution when equal volumes of the two solutions are mixed?

0.10 M HF and 0.10 M NaF

0.10 M HF and 0.10 M NaOH

0.50 M HF and 0.25 M NaOH

0.25 M HCl and 0.50 M NaF

6) Which of the following (select all that apply) gives a buffer solution when equal volumes of the two solutions are mixed?

0.10 M NH3 and 0.10 M NH4Cl

0.10 M NH3 and 0.10 M NaOH

0.10 M NH4Cl and 0.10 M NaOH

0.50 M NH4Cl and 0.25 M NOH

      -       A.       B.       C.   

LiF to and HF solution

      -       A.       B.       C.   

KI to and HI solution

      -       A.       B.       C.   

NH4Cl to and NH3 solution

      -       A.       B.       C.   

HBr to an CH3COO-/CH3COOH (acetic acid/acetate buffer) solution

A.

Remain the same

B.

Decrease

C.

Increase

Explanation / Answer

4) Does the pH increase, decrease or remain the same on the addition of the of the following?

a. LiF to and HF solution

PH will increase        

If we add F-, the conjugate base, shifts the equilibrium toward reactants less acid dissociated, less [H3O+], higher pH.

b. KI to and HI solution

HI is a strong acid and will completely dissociate. Therefore, the reaction equilibrium being dealt with involves the dissociation of water. Addition of KI does nothing to the equilibrium, and the pH does not change.

PH remain constant

c. NH4Cl to and NH3 solution

PH will decreases

NH4Cl will add NH4+ to the reaction mixture. NH3 is a base, NH4+ is a reaction product. The reaction will shift to the reactant side, and the amount of OH- in the reaction mixture decreases, as will the pH.

d. HBr to an CH3COO-/CH3COOH (acetic acid/acetate buffer) solution.

PH will increase

Which of the following (select all that apply) gives a buffer solution when equal volumes of the two solutions are mixed?

a)

Buffer.

Both are remain at equilibrium

b) Not Buffer

The OH- reacts will all of the HF. This solution will be the equivalent of a solution of NaF

C) Buffer.

The OH- reacts will some but not all of the HF.

d) Buffer

As the HCl reacts with some but not all of the F

6) Which of the following (select all that apply) gives a buffer solution when equal volumes of the two solutions are mixed?

A buffer is a mixture of a weak acid and its conjugate base.

A) buffer

NH4+ is the acid, and NH3 is the conjugate base

B) Not Buffer

NaOH is strong base after dissociation from H3O+ ions

C) Buffer

The OH- will neutralize some of the NH4+ making NH3, while some NH4+ remains.

D] Not buffer

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