Question

How many milliliters of a 0.15--M solution of KOH will be reuired to titrate 40.00mL of a 0.656-M solution of H3PO4?

H3PO4 + 2KOH ? K2HPO4 + 2H2O

Answer 1

To titrate 40.00 mL of a 0.0656-M solution of H3PO4 with a 0.1500-M solution of KOH, you would need 80.00 mL of the KOH solution.

Step-by-step explanation:

To solve this question, we need to use the balanced chemical equation:

H3PO4 + 2KOH --> K2HPO4 + 2H2O

From the equation, we can see that the ratio of KOH to H3PO4 is 2:1.

Therefore, to titrate 40.00 mL of a 0.0656-M solution of H3PO4, we need twice the volume of a 0.1500-M solution of KOH.

This means we would need 2 x 40.00 mL = 80.00 mL of the KOH solution.