Answered

Discover answers to your questions with Westonci.ca, the leading Q&A platform that connects you with knowledgeable experts. Discover in-depth answers to your questions from a wide network of experts on our user-friendly Q&A platform. Our platform provides a seamless experience for finding reliable answers from a network of experienced professionals.

A 3.458 g sample of KHP, a monoprotic acid, requires 45.71 mL of a KOH solution to reach the endpoint. What is the concentration of the KOH solution? The molar mass of KHP is 204.22 g/mol.

Sagot :

sebassandin

Answer:

[tex]M_{KOH}=0.3704M[/tex]

Explanation:

Hello there!

In this case, since the titration of bases when using monoprotic acids like KHP, occurs in a 1:1 mole ratio, it is possible to use the following equation, because at the endpoint the moles of the KHP and KOH get equal:

[tex]n_{KHP}=n_{KOH}[/tex]

In such a way, we first calculate the moles of KOH given the mass and molar mass of KHP:

[tex]n_{KHP}=n_{KOH}=3.458g*\frac{1mol}{204.22g}=0.0169mol[/tex]

Next, since we have the volume of KOH, we first take it to liters (0.04571 L) to that we obtain the following concentration:

[tex]M_{KOH}=\frac{0.0169mol}{0.04571L}\\\\M_{KOH}=0.3704M[/tex]

Regards!

We appreciate your time. Please revisit us for more reliable answers to any questions you may have. We hope this was helpful. Please come back whenever you need more information or answers to your queries. Discover more at Westonci.ca. Return for the latest expert answers and updates on various topics.