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# Consider the reaction:2 K3PO4(aq) + 3 NiCl2(aq) ?

## Problem 91P Chapter 13

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition

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Problem 91P

Consider the reaction:

2 K3PO4(aq) + 3 NiCl2(aq) → Ni3(PO4)2(s) + 6 KCl(aq)

What volume of 0.225 M K3PO4 solution is necessary to completely react with 134 mL of 0.0112 M NiCl2?

Step-by-Step Solution:
Step 1 of 3

Solution: Here, we are going to calculate the volume of K3PO4 solution.

Step1:

Molarity(M) is defined as number of moles of solute dissolved in one litre (or one cubic decimetre) of solution.

Moles of solute

Molarity = -------------------------------        ------(1)

Volume of solution in litre

Step2:

Given, Volume of NiCl2 solution = 134 mL = 134 / 1000 L = 0.134 L        [1000 mL = 1 L]

Molarity of NiCl2 solution = 0.0112 M

Therefore, number of moles of NiCl2 solution = molarity x volume of solution in litres

= 0.0112 M x 0.134 L

= 0.0015008 mol

Step3:

The given reaction...

Step 2 of 3

Step 3 of 3

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Consider the reaction:2 K3PO4(aq) + 3 NiCl2(aq) ?

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Get Full Access to Introductory Chemistry - 5 Edition - Chapter 13 - Problem 91p