Wednesday
July 30, 2014

Homework Help: Chemistry

Posted by Joseph on Tuesday, March 29, 2011 at 12:55am.

A student titrates HCl with 0.0125M KOH. Starting with 50.00 ml of the acid it takes 40.0 ml of base to reach equilavence point.

A. What is the concentration of the HCl?

B. What is the initial pH of the acid solution?

C. What is the pH of the reaction mixture after the addition of 20.00 ml of base?

D. What is the pH at equivlance point?

E. What is the pH after the addition of 50.00 ml of the base?

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

Chemistry - A student titrates HCl with 0.0125M KOH. Starting with 50.00 ml of ...
Chemistry - A student titrates HCl with 0.0125M KOH. Starting with 50.00 ml of ...
Chemistry - A student titrates 0.100M KOH into 50.00 ml of weak acid HX. The pH ...
Chemistry - A student titrates 0.025 M KOH into 50.00 ml of a solution of ...
Chemistry - A student titrates 0.025 M KOH into 50.00 ml of a solution of ...
Chemistry - A titration is performed by adding .600 M KOH to 40.0 mL of .800 M ...
Chemistry - A 23.0mL sample of a diprotic acid is titrated with 0.260M KOH. If ...
chemistry - 31.0mL sample of LiOH, concentration unknown, is titrated with .52 M...
Chemistry - If a chemist titrates 300.0 mL of H2SO4 with a 3.0 M solution of ...
Chemistry - If a chemist titrates 300.0 mL of H2SO4 with a 3.0 M solution of ...

Search
Members