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Question Description

I’m stuck on a Chemistry question and need an explanation.

Acrylic acid is a weak monoprotic acid with Ka = 5.5×10-5 M. NaOH(s) was gradually added to 1.00 L of 8.58×10-2 M acrylic acid.

1)Calculate the pH of the solution after the addition of 8.58×10-2 mol of NaOH(s). 

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Final Answer

[H+] = (8580-8.58v)/(1000+v) * 10^(-2), where v is the volume of NaOH added

v = 149 mL

and:

[H+] = 0.06354

so:

pH = 1.197


Rabianaaz N (570)
UC Berkeley

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