   # A 500.0-mL sample of 0.200 M sodium phosphate is mixed with 400.0 mL of 0.289 M barium chloride. What is the mass of the solid produced? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 6, Problem 116CWP
Textbook Problem
75 views

## A 500.0-mL sample of 0.200 M sodium phosphate is mixed with 400.0 mL of 0.289 M barium chloride. What is the mass of the solid produced?

Interpretation Introduction

Interpretation:

Calculate the mass of solid when given barium chloride and sodium phosphate is mixed.

Concept Introduction:

The precipitate will be formed when two soluble salt solutions combined together is called as a precipitation reaction.

The balanced equation is

3BaCl2(aq)+2Na3PO4(aq)Ba3(PO4)2(s)+6NaCl(aq)

Formula

Mole=volumeofsolution (L)×molarity (M)litre (L) (1)

### Explanation of Solution

Explanation

Record the data from the question

Volume of barium chloride is 0.4L , molarity of barium chloride is 0.289M

Molecular weight of Ba3(PO4)2 is 601.8g , volume of Na3PO4 is 0.5L

Molarity of Na3PO4 is 0.2M

0.4000LBaCl2×0.289moleBaCl2Litre×1moleBa3(PO4)23moleBaCl2×601.8gBa3(PO4)2mloeBa3(PO4)2

=23

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