Tuesday
October 21, 2014

Homework Help: Chemistry

Posted by Melia on Monday, November 19, 2012 at 2:18am.

A 100.0mL solution containing aqueous HCl and HBr was titrated with 0.1290M NaOH. The volume of base required to neutralize the acid was 47.56mL. Aqueous AgNO3 was then added to precipitate the Cl- and Br- ions as AgCl and AgBr. The mass of the silver halides obtained was 0.9849 g.

a.)What is the molarity of HBr in the original solution?

b.)What is the molarity of HCl in the original solution?

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

chemistry - 1. if 15.0mL of 4.5 M NaOH are diluted with water to a volume of ...
Chemistry - Which one of the following pairs of 0.100 mol L-1 solutions, when ...
Honors Chemistry - If 20 mL of 0.01 M aqueous HCl is required to neutralize 30 ...
Chemistry - 1.What mass of NaOH(s) must be added to 300 mL of HCl 0.25 M in ...
chemistry - You have 20.00 mL of a 0.1M aqueous solution of the weak base (CH3)...
science - 25 ml sample of 0.150 m solution of aqueous trimethylamine is titrated...
Chemistry - Calculate the volume of 2.503 N HNO3 added to 100 mL of HCl in order...
Chemistry - a 25.0mL sample of a 0.100M solution of aqueous trimethylamine is ...
CHEMISTRY - 1) An NaOH solution of unknown concentration is titrated with HCl. ...
Chemistry.. help plz - 3. How much 0.10 M Base (in mL) is required to ...

Search
Members