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A hard water solution contains 4.8 g of calcium chloride.

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 85P Chapter 8

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 85P

PROBLEM 85P

A hard water solution contains 4.8 g of calcium chloride. How much sodium phosphate in grams should be added to the solution to completely precipitate all of the calcium?

Step-by-Step Solution:
Step 1 of 3

Solution 85P

Here, we have to determine the amount of sodium phosphate required to precipitate all of the calcium.

3CaCl2(aq) +2 Na3(PO4)------> 6NaCl(s) + Ca3(PO4)2

Molar mass of CaCl2 =110.98 g/mol

Molar mass of Na3(PO4) =163.94 g/mol

Therefore,

g CaCl2(aq)= mol CaCl2(aq) = g Na3(PO4) = mol Na3(PO4)

Thus the amount of sodium phosphate required

= 4.8 g CaCl2(aq)   x  x x...

Step 2 of 3

Chapter 8, Problem 85P is Solved
Step 3 of 3

Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

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