1.0 mL of .50 M Acetic Acid (CH3COOH) is mixed with 3.0 mL of .50 M Acetate Ion (NaC2H3O2) to create a buffer. Drops of 1.0 M HCl solution are added until the buffer is "consumed.'

Write the acid-base reaction that consumed the buffer. Calculate the equilibrium constant for this reaction.

(30 drops were needed to consume it).

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Write reaction equations to explain how acetic acid-acetate buffer reacts with an acid and reacts with a base.

Say, for example, that you had prepared a Buffer C, in which you mixed 1.35 g of sodium acetate, NaC2H3O2, with 100.0 mL of 1.0 M acetic acid.

a. What would be the initial pH of Buffer C?

b. If you add 5.0 mL of 0.5 M NaOH solution to 20.0 mL each of Buffer B and Buffer C, which bufferâs pH would change less? Explain.

A buffer is prepared by adding 20.0 g of sodium acetate (CH₃COONa) to 500 mL of a 0.150 M acetic acid (CH₃COOH) solution. (a) Determine the pH of the buffer. (b) Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer. (c) Write the complete ionic equation for the reaction that occurs when a few drops of sodium hydroxide solution are added to the buffer.

greenbear617

You are given 60 ml of 0.50 M acetic acid/acetate buffer to test. The starting composition of the two major species are:

Concentration of CH3COOH is 0.300 M, Concentration of CH3COO- is 0.200 M

a) Use the Handerson-Hasselbach equation to estimate the initial pH of the buffer.

b) You add 1.0 ml of 1.00 M HCl to the buffer. Calculate the molarity of H3O+ added as HCl, and the final molarities of acetic acid and acetate ion at equilibrium. What is the new value of pH?

c)Now take a fresh 60 ml of the buffer and add 1.0 ml of 1.00 M NaOH. Using steps similar to those above, calculate the new pH of the solution.

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