Explain how a solution containing 0.75 M acetic acid (HC_2H_3O_2) and 0.75 M sod

Question

Explain how a solution containing 0.75 M acetic acid (HC_2H_3O_2) and 0.75 M sodium acetate (NaC_2H_3O_2) can resist changes in pH when small amounts of either HCI or NaOH are added. Write the balanced chemical equation for the chemical reaction that occurs when HCI is added to the given buffer system. The buffer solution contains both sodium acetate and acetic acid in equimolar concentrations. The sodium acetate dissociates into sodium ions and acetate ions (C_2H_3O_2) while the HCI completely dissociates into H_3O^+ and CI^- ions in the aqueous solution. The CI^- ions are spectator ions and do not participate m the reaction while the acetate ions react with the H_3O^+ to form acetic acid (HC_2H_3O_2) and water. This prevents the H_3O^+ ion concentration from increasing and lowing the pH of the solution. Write the balanced chemical equation for this reaction. (Include states-of-matter under the given conditions in your answer.) Write the balanced chemical equation for the

Explanation / Answer

The buffer is mixture of acetic acid and sodium acetate.

CH3COOH -----------> CH3COO-

when HCl is added

CH3COO- + HCl ---------------> CH3COOH + Cl-

When NaOH is aded

CH3COOH + NaOH ---------> CH3COONa + H2O

Part 1.

CH3COO-(aq) + H3O+(aq) ----------> CH3COOH(aq) + H2O (l)

Part 2

CH3COOH(aq) + OH- (aq) -------------> CH3COO- (aq) + H2O(l)

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