O ACIDS AND BASES Calculating the pH of a weak acid titrated with a strong Ansle
ID: 706552 • Letter: O
Question
O ACIDS AND BASES Calculating the pH of a weak acid titrated with a strong Ansley An analytical chemist is titrating 217.3 mL of a 0.3400 M solution of acetic acid (HCH,CO2) with a 1.200 M solution of NaOH. The p K of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 47.76 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. alo Ar PH Explanation CheckExplanation / Answer
no of moles of CH3COOH = molarity* volume in L
= 0.34*0.2173
= 0.073882 moles
no of moles of NaOH = molarity* volume in L
= 1.2*0.04776 = 0.057312moles
CH3COOH(aq) + NaOH(aq) ---------> CH3COONa(aq) + H2O(l)
I 0.073882 0.057312 0
C -0.057312 -0.057312 0.057312
E 0.01657 0 0.057312
PH = Pka + log[CH3COONa]/[CH3COOH]
= 4.70 + log0.057312/0.01657
= 4.70 + 0.54 = 5.24 >>>>answer
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