Calculate the pH of each of the solutions and the change in pH to 0.01 pH...

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Chemistry

Calculate the pH of each of the solutions and the change in pHto 0.01 pH units caused by adding 10.0 mL of 3.63-M HCl to 440. mLof each of the following solutions.
a.) .181 M C2H3O2 1-
ph before mixing: 9.00 (correct)
pH after mixing: ??
b.) a buffer solution that is 0.181 M in each C2H3O2 1- andHC2H3O2
pH before mixing: ??
pH after mixing: ??
Thank you!! Sincerely, a confused college student

Answer & Explanation Solved by verified expert

4.2 Ratings (585 Votes)

10.0 mL 3.22 M HCl + 420 mL water

pH before mixing= -0.51 for HCl and 7 for water
pH after mixing= 1.13
pH change= 1.64

b) 10.0 mL 3.22 M HCl + 420 mL 0.160 M CH3COO-
reaction: HCl + CH3COO- --> CH3COOH + Cl-

we have 32.22 mmoles of HCl and 67.20 mmoles of CH3COO-, so we will obtain 67.20-32.22=34.98 mmoles of CH3COO and 32.22 mmoles of CH3COOH in a total of 430 mL. This is a buffer solution.

pH before mixing=-0.51 for HCl and x2/0.160=1.8E-5 and pOH=2.77 and pH=11.23 for CH3COO-
pH after mixing= pH=pKa-log[Cb/Ca]=4.74-log

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