What is the pH of a solution that results from diluting 0.700 mol acetic acid (CH3CO2H)...
What is the pH of a solution that results from diluting 0.700 mol acetic acid (CH3CO2H) and 0.129 mol sodium acetate (NaCH3CO2) with water to a volume of 1.41 L? (Ka of CH3CO2H = 1.8E-5)
Homework Answers
Ka = 1.8*10^-5
pKa = - log (Ka)
= - log(1.8*10^-5)
= 4.745
use:
pH = pKa + log {[conjugate base]/[acid]}
Since volume is same for numerator and denominator, above expression can also be written as:
pH = pKa + log {mol(conjugate base)/mol(acid)}
= 4.745+ log {0.129/0.7}
= 4.01
Answer: 4.01
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