Saturday
November 29, 2014

Homework Help: Chemistry

Posted by Anonymous on Saturday, February 8, 2014 at 2:03pm.

A titration involves titrating 0.4 M NaOH into a solution of 0.2 M H3PO4.
a.) Calculate the volume of NaOH that will be required to reach the first equivalence point.
b.) Calculate the volume of NaOH required to reach the second equivalence point.
Other information: 10 ml H3PO4 was added to 250 ml of deionized water, and solution was then titrated with NaOH.

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

Chemistry - A solution contains 25 mmol of H3PO4 and 10. mmol of NaH2PO4. What ...
please help analytical chemistry - 50 ml of a .1103M solution of formic acid is ...
chemistry - 50 ml of a .1103M solution of formic acid is titrated with a .2511M ...
chemistry - 11.During an acid-base titration, 25 mL of NaOH 0.2 M were required ...
chemistry 2 - Titration of 50.0 mL of acetic acid reaches equivalence after ...
Chemistry - During an acid-base titration, 25 mL of NaOH 0.2 M were required to...
Chemistry - calculate the molar concentration of H3PO4 in the cola sample. ...
college chemistry - In class, we discussed the titration of a 50.0 mL sample of ...
chemistry - I am confused on how to do the last question. Calculate molarity of ...
Chemistry - In this case, the inflection point, and equivalence, occurs after 23...

Search
Members