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What would be the expected equivalence point volume if you titrate 25.00 mL of 0.0265 M KHP (a weak monoprotic acid) with 0.0368 M NaOH?

A. 18.0 mL
B. 34.7 mL
C. 39.1 mL
D. 58.3 mL
E. 25.2 mL

Answer :

The expected equivalence point volume if you titrate 25.00 mL of 0.0265 M KHP (weak monoprotic acid) with 0.0368 M NaOH is 18.0 mL. So, the correct option is a.

Step 1: Determine the balanced chemical equation. KHP + NaOH → NaKP + H2O

Step 2: Calculate the number of moles of KHP.

Number of moles of KHP = (Concentration × Volume) / 1000

Number of moles of KHP = (0.0265 M × 25.00 mL) / 1000

Number of moles of KHP = 0.0006625 mol

Step 3: Use the balanced chemical equation to determine the number of moles of NaOH that reacted with KHP. 1 mol of KHP reacts with 1 mol of NaOH.

Moles of NaOH = 0.0006625 mol

Step 4: Calculate the volume of NaOH used to react with KHP.

Volume of NaOH = (Moles of NaOH × 1000) / Concentration of NaOH

Volume of NaOH = (0.0006625 mol × 1000) / 0.0368 M

Volume of NaOH = 18.0 mL

Therefore, the expected equivalence point volume if you titrate 25.00 mL of 0.0265 M KHP (weak monoprotic acid) with 0.0368 M NaOH is 18.0 mL.

You can learn more about equivalence points at: brainly.com/question/29999744

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