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A buffer is prepared by adding 23.0 g of sodium acetate (CH3COONa) to 510 mL of...

A buffer is prepared by adding 23.0 g of sodium acetate (CH3COONa) to 510 mL of a 0.145 Macetic acid (CH3COOH) solution.

Determine the pH of the buffer.

Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer.

Write the complete ionic equation for the reaction that occurs when a few drops of sodium hydroxide solution are added to the buffer.

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Answer #1

pH of buffer may be obtained with:

pH = pKa + log(A-/HA)

pH = 4.756

mol A- = mass/MW = 23/82.0338 = 0.28037

[A-] = mol A- /V = 0.28037/.510 = 0.549745

Then:

pH = pKa + log(A-/HA) = 4.756 + log(0.549745/0.145) = 5.334

Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer.

HCl --> H+ and Cl-

in equilibrium, A- is present thereofre

A- + H+ <--> HA net ionic equaiton

Write the complete ionic equation for the reaction that occurs when a few drops of sodium hydroxide solution are added to the buffer.

NAOH --> Na+ and OH-

HA is present in equilibrium thereofre:

HA --> H+ and A- + OH-

H2O is produced and A- increases

OH- + H+ --> H2O net ionic equation

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