mL NaOH x M NaOH = mL acid x M acid.
mL NaOH x 0.125M = 25.0 x 0.175
Solve for mL NaOH. The 20% ionization is extraneous information.
Determine the volume of 0.125 M NaOH required to titrate to the equivalence point 25.0 mL of a 0.175 M solution of a monoprotic weak acid that is 20% ionized.
Answer is 35.0 mL. How do you find it?!
It's been a really long time since we talked about titrations. Please help (:
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