Friday
April 18, 2014

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 - Calculate ΔG at 25C for the precipitation of lead(II) chloride...
chem lab (webwork) - What is the pH of the solution created by combining 1.80 mL...
Chemistry - 50.00 mL samples of 0.200 mol/L potassium phosphate with an excess ...
chem lab (webwork) - What is the pH of the solution created by combining 1.80 mL...
Chemistry help!!! - The class will react 50.00 mL samples of .200 mol/L ...
Chemistry - If 32.0 mL lead(II) nitrate solution reacts completely with excess ...
Chemistry Lab - 5.00 mL of .00500 M ferric nitrate is added to 5.00 mL of nitric...
Chemistry - 7 grams of chloride was dissolved in water. 20 ml of lead(II)nitrate...
Chemistry - 7 grams of chloride was dissolved in water. 20 ml of lead(II)nitrate...
Chemistry Lab - You need 123 mL of 0.245 M NaOH solution for a certain ...

Search
Members