   # If you mix 48 mL of 0.0012 M BaCl 2 with 24 mL of 1.0 × 10 −6 M Na 2 SO 4 , will a precipitate of BaSO 4 form? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 17, Problem 79GQ
Textbook Problem
3 views

## If you mix 48 mL of 0.0012 M BaCl2 with 24 mL of 1.0 × 10−6 M Na2SO4, will a precipitate of BaSO4 form?

Interpretation Introduction

Interpretation:

Whether the precipitation of BaSO4 occurs or not on addition of 48 ml 0.0012 MBaCl2 to 24ml 1.0×106 M Na2SO solution has to be predicted.

Concept introduction:

Solubility product constant,Ksp is equilibrium constant and is defined as the product of the equilibrium concentration of the ions of the salt raised to the power of their coefficients in the balanced chemical equation.

The expression for Ksp of a salt is given as,

AxBy(s)xAy+(aq)+yBx(aq)Ksp=[Ay+]x[Bx]y

Here,

• [Ay+] and [Bx] are equilibrium concentration.

Reaction quotient, Q, for a reaction is defined as the product of the concentration of the ions at any time of the reaction (other than equilibrium time ) of the salt raised to the power of their coefficients in the balanced chemical equation.

The expression for Q of a salt is given as,

AxBy(s)xAy+(aq)+yBx(aq)Ksp=[Ay+]x[Bx]y

Here,

• [Ay+] and [Bx] are the concentration at any time except equilibrium.
1. 1. If Q=Ksp, this implies that the solution is saturated solution and the concentration of the ions have reached their maximum limit.
2. 2. If Q<Ksp, this implies that the solution is not saturated and more salt can be added to the solution or the salt present in the solution already will dissolve more until the precipitation starts.
3. 3. If Q>Ksp, this implies that the solution is oversaturated and precipitation of salt will occur.

### Explanation of Solution

Value of reaction quotient,Q, is calculated and compared with the value of Ksp for BaSO4.

Given:

Refer to the Appendix J in the textbook for the value of Ksp

The value of solubility product constant,Ksp, for BaSO4 is 1.1×1010.

BaSO4 is dissociated as follows in water,

BaSO4(s)Ba2+(aq)+SO42(aq)

The expression of Q for BaSO4 is,

Q=[Ba2+][SO42] (1)

millimoles of Ba2+=48×0.0012=0.0576millimoles of SO42=24×(1.0×106)=2.4×105

Total volume of the solution is 72 ml.

Concentration of Barium ions in the solution is,

[Ba2+]=0.057672=8.0×104 M

Concentration of sulphate ions in the solution is,

[SO42]=(2

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