Question

1.A 1.00 liter solution contains 0.28 M acetic acid and 0.36 M sodium acetate.

If 0.180 moles of potassium hydroxide are added to this system, indicate whether the following statements are true or false.

(Assume that the volume does not change upon the addition of potassium hydroxide.)

A. The number of moles of CH₃COOH will remain the same.

B. The number of moles of CH₃COO^- will decrease.

C. The equilibrium concentration of H₃O⁺ will increase.

D. The pH will increase.

E. The ratio of [CH₃COOH] / [CH₃COO^-] will remain the same.

2.

A buffer solution is made that is 0.347 M in and 0.347 M in.

If  for is, what is the pH of the buffer solution?

pH =

Write the net ionic equation for the reaction that occurs when 0.085 mol KOH is added to 1.00 L of the buffer solution.

(Use the lowest possible coefficients. Omit states of matter.)

3.

A buffer solution is made that is 0.396 M in and 0.396 M in.

If  for is, what is the pH of the buffer solution?

pH =

Write the net ionic equation for the reaction that occurs when 0.085 mol KOH is added to 1.00 L of the buffer solution.

(Use the lowest possible coefficients. Omit states of matter.)

Answer 1

Given: 1 lit solution of 0.28 M acetic acid and 0.36 M Sodium acetate.

Now, 0.18 moles of KOH are added to this system so,

A) False, because added base(KOH) will react with the already present acetic acid and hence moles of acetic acid will reduce.

B) False, because CH3COO- will form by the reaction of acetic acid and KOH and therefore moles of CH3COO- will also increase.

C) False, because added KOH will neutralize the already present H3O+ ions in the solution, so the equilibrium concentration of H3O+ will decrease.

D) True, On adding base concentration of H+ ions will decrease so pH will increase.

E) False, Since [CH3COOH] will decrease and [CH3COO-] will increase so the ratio [CH3COOH]/[CH3COO-] will definitely decrease.