×

# A solution contains 0.133 g of dissolved lead. How many ISBN: 9780321910295 34

## Solution for problem 111P Chapter 7

Introductory Chemistry | 5th Edition

• Textbook Solutions
• 2901 Step-by-step solutions solved by professors and subject experts
• Get 24/7 help from StudySoup virtual teaching assistants Introductory Chemistry | 5th Edition

4 5 0 324 Reviews
15
5
Problem 111P

PROBLEM 111P

A solution contains 0.133 g of dissolved lead. How many moles of sodium chloride must be added to the solution to completely precipitate all of the dissolved lead? What mass of sodium chloride must be added?

Step-by-Step Solution:

Solution 111P

Here, we have to determine the moles of NaCl and mass of NaCl.

Step 1:

Calculation of the mass of lead which is dissolved into the solution.

Molar mass of Lead =207.2 g/mol

Mass of lead dissolved in the solution = 0.133 g

Therefore, mole required for Lead is = = 0.000642 mol

Step 2:

Calculation for the mole of NaCl required to dissolve the precipitation.

Pb (s) + 2 NaCl(aq)-------> PbCl2(aq)

Therefore, 2 mole of NaCl required to dissolve the ppt = 2x 0.000642 mol =0.00128 mol

Thus, NaCl required to dissolve the lead precipitation = 0.00128 mol =1.28 x 10-3 mol

Step 3 of 3

##### ISBN: 9780321910295

Unlock Textbook Solution

A solution contains 0.133 g of dissolved lead. How many

×