Question
Suppose 50.0 mL of an aqueous solution containing an unknown monoprotic weak
acid is titrated with 0.250 M KOH. The titration requires 31.52 mL of the potassium hydroxide
solution to reach the equivalence point. What is the concentration (in molarity) of the unknown
acid solution?
acid is titrated with 0.250 M KOH. The titration requires 31.52 mL of the potassium hydroxide
solution to reach the equivalence point. What is the concentration (in molarity) of the unknown
acid solution?
Answers
HA + KOH --> H2O + KA
mols KOH = M x L = ?
mols HA = moles KOH (from the coefficients in the balanced equation.
M HA = moles HA/L HA
mols KOH = M x L = ?
mols HA = moles KOH (from the coefficients in the balanced equation.
M HA = moles HA/L HA
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