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Prepare 1 L of an acetic acid sodium acetate buffer with a pH of 5.00 and...

Prepare 1 L of an acetic acid sodium acetate buffer with a pH of 5.00 and a buffer concentration of 100 mM. Besides water you only have a 500g bottle of sodium acetate trihydrate, 1L of 1.00 hydrochloric acid, and 1L of 1.00 M sodium hydroxide.

A. Identify the reagents needed and calculate all amounts needed.

B. Calculate the change in pH of a 250 mL portion of the buffer that has 1 mL of 1.00 M NaOH added to it.

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Expert Solution

Substitute this in the above equation

Since total volume is 1 L, molar concentration is equal to number of moles.

Number of moles of sodium acetate trihydrate

Number of moles of acetic acid

0.0355 moles of acetic acid are obtained by neutralisation of 0.0355 moles of sodium acetate trihydrate with 0.0355 moles of HCl.

Total number of moles of sodium acetate trihydrate

Molar mass of sodium acetate trihydrate is 136 g/mol

Mass of sodium acetate trihydrate

0.0355 moles of HCl (1 M) are obtained from 0.0355 L (or 35.5 mL) of 1 M HCl solution.

Hence, wee need 0.0355 L (or 35.5 mL) of 1 M HCl solution and 13.6 g of solid sodium acetate trihydrate.

1 mL of 1.00 M NaOH is added

NaOH will combine with acetic acid to form sodium acetate

pH will increase by

queen_honey_blossom answered 1 year ago

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