10 mL of 0.0100 M HCl are added to 25.0 mL of a buffer solution that is 0.010 M HC2H3O2 and 0.1 M C2H3O2-. What is the pH of the resulting solution?
mol of HCl added = 0.01M *10.0 mL = 0.1 mmol
CH3COONa will react with H+ to form CH3COOH
Before Reaction:
mol of CH3COONa = 0.1 M *25.0 mL
mol of CH3COONa = 2.5 mmol
mol of CH3COOH = 0.01 M *25.0 mL
mol of CH3COOH = 0.25 mmol
after reaction,
mol of CH3COONa = mol present initially - mol added
mmol of CH3COONa = (2.5 - 0.1) mmol
mol of CH3COONa = 2.4 mmol
mol of CH3COOH = mol present initially + mol added
mol of CH3COOH = (0.25 + 0.1) mmol
mol of CH3COOH = 0.35 mmol
Ka = 1.8*10^-5
pKa = - log (Ka)
= - log(1.8*10^-5)
= 4.7447
since volume is both in numerator and denominator, we can use mol instead of concentration
use:
pH = pKa + log {[conjugate base]/[acid]}
= 4.7447+ log {2.4/0.35}
= 5.58
Answer: 5.58
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