An acetic acid buffer containing 0.50 M HC2H3O2 and 0.50 M NaC2H3O2 has a pH of...

An acetic acid buffer containing 0.50 M HC₂H₃O₂ and 0.50 M NaC₂H₃O₂ has a pH of 4.74. What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

A	4.77
B	4.71
C	4.68
D	4.62
E	none of these choices is correct

Solutions

Expert Solution

The answer is A) 4.71

Henderson equation is

pH = pKa + log([A-]/[HA])

pKa of acetic acid is 4.75

[ A- ] = [ HC2H3O2]= 0.5M

[ HA] = [ C2H3O2-] = 0.5M

No of mole of HC2H3O2 = (0.5mol/1000ml)×100ml = 0.05

No of mole of C2H3O2- = 0.05

HCl react with conjugate base C2H3O2-

H+ + C2H3O2- -------> HC2H3O2

1mole of HCl react with 1mole of C2H3O2- to give one mole of HC2H3O2

0.0020mol of HCl react with 0.0020mole of C2H3O2- to give 0.0020 mol of HC2H3O2

No of mole of C2H3O2- = 0.05 - 0.0020 = 0.048mol

No of mole of HC2H3O2 = 0.05 + 0.0020 = 0.052mol

[ C2H3O2- ] = 0.48M

[ HC2H3O2 ] = 0.52M

Therefore,

pH = 4.75 + log( 0.48/0.50)

=4.75 - 0.034

= 4.71

queen_honey_blossom answered 1 year ago

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