Sunday
March 29, 2015

Homework Help: Chemistry

Posted by Anonymous on Monday, October 30, 2006 at 8:04pm.

You made 100.0 ml of a lead (II) nitrate solution for lab but forgot to cap it. The next lab session you noticed that there was only 80.0 ml left. In addition, you forgot the initial concentration of the solution. You decide to take 2.00 ml of the solution and add an excess of a concentrated sodium chloride solution. You obtain a solid with a mass of 3.407g. What was the concentration ofthe original lead (II) nitrate solution?

Convert 3.407g PbCl2 to mols. That will be mols Pb(NO3)2 in 2.00 mL solution. That times 80/2 will be the mols in 80 mL and mols in the original 100 mL. Calculate molarity from there.Post your work if you get stuck. We will need that to know where you are having a problem.

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

chemistry - You made 100.0 mL of a lead(II) nitrate solution for lab but forgot ...
Chemistry - 1. Imagine that you work at a company that prepares chemical ...
Organic Chemistry - In lab, we purified acetanilide through recrystallization. ...
Forgot my book, need science help!! - Please help me I have a whole section to ...
Biology I - Hi! Hoping someone knows this/has some on hand. Without being ...
chemistry - a lab experiment calls for 10% acetic acid solution. The lab has ...
chem - A chemistry lab experiment requires 33.3 g of silver nitrate. How many ...
chemistry - 20.0 mL of a 2.2 M lead (II) nitrate solution is mixed with 100.0 ...
Chemistry - 50.00 mL samples of 0.200 mol/L potassium phosphate with an excess ...
chemistry - describe how to prepare a .50 m solution of lead nitrate using only ...

Members