February 19, 2017

Homework Help: Chemistry

Posted by Anonymous on Sunday, October 16, 2011 at 10:06pm.

A 0.4584 g sample of impure zinc chloride, ZnCl2, FW = 136.3 g/mole, was dissolved in water and excess silver nitrate was added to the solution. The mass of the dry silver chloride, AgCl, FW = 143.3 g/mole, produced was 0.8564 g. The balanced precipitation is: ZnCl2 (aq) + 2 AgNO3 (aq) --> 2 Agcl (s) + Zn(NO3)2 (aq).

1. Calculate the moles of zinc chloride present in the sample.

2. Calculate the mass of zinc chloride in the sample.

3. Calculate the percent purity of the zinc cholride in the sample.

Answer This Question

First Name:
School Subject:

Related Questions

More Related Questions