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Bingel [31]
3 years ago
14

A 110.0 ml sample of 0.20 mhf is titrated with 0.10 mcsoh. determine the ph of the solution after the addition of 440.0 ml of cs

oh. the ka of hf is 3.5×10−4.
Chemistry
1 answer:
Margarita [4]3 years ago
6 0
Given:

Concentration of HF = 0.20 m
Volume of HF = 110 ml
Concentration of CsOH = 0.10 m
Volume of CsOH = 440 ml
Ka (HF) = 3.5 x 10^-4

Balanced Chemical Equation:

HF + CsOH ===> CsF + H2O 

pH of the solution = log ([acid]/[base]) + pKa
pH = log ([0.20*(110/1000)]/[0.10*(440/1000)]) - log(3.5x10^-4)
pH = 3.15<span />
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