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Calculate the change in pH that occurs when 0.00100 mol of gaseous HCl is added to...

Calculate the change in pH that occurs when 0.00100 mol of gaseous HCl is added to a buffer solution that is prepared by dissolving 4.92 g of sodium acetate ( molar mass= 82.03 g/mol) in 250 mL of 0.150 mol/L of acetic acid solution? Assume no change in volume upon addition of either the sodium acetate or HCl. (Ka for acetic acid = 1.8x10^-5) *please explain!*

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Answer #1

The solution is250mL of 0.150M acetic acid solution.

Now 4.92 g of sodium acetate is dissolved in it.

Molarity of sodium acetate = (4.92/82.03g/mol) (1000/250)

= 0.2399 M

The solution now forms a buffer consisting of a weak acid (acetic acid) and its conjugate base(sodium acetate).

Its pH is calculated using Hendersen equation

pH = pka + log [conjugate base]/[acid]

= (5 - log 1.8) + log (0.2399/0.150)

= 4.9439

When 0.0010 moles of Hcl is added, the reaction that takes place is

CH3COONa + HCl -------> CH3COOH + NaCl

0.2399 - 0.150 - initial concentrations

0.001 change

0.2389 0 0.151 - after reaction

New pH of the solution = 4.74 + log (0.2389/0.151)

= 4.9392

Thus the chang e in pH = 4.9439 -4.9392

=0.0046 6

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