   Chapter 16, Problem 82AE

Chapter
Section
Textbook Problem

# Calculate the mass of manganese hydroxide present in 1300 mL of a saturated manganese hydroxide solution. For Mn(OH)2, Ksp = 2.0 × 10−13.

Interpretation Introduction

Interpretation: The mass of manganese hydroxide that will be present in 130mL of a saturated manganese hydroxide solution is to be calculated.

Concept introduction: Solubility is defined as the maximum amount of solute that can dissolve at a certain amount of solvent at certain temperature. The solubility product, Ksp is the equilibrium constant that is applied when salt partially dissolve in a solvent. The solubility product of dissociation of AxBy is calculated by the formula,

Ksp=[A]x[B]y

Explanation

Explanation

To determine: The mass of manganese hydroxide that will be present in 130mL of a saturated manganese hydroxide solution.

The equation to calculate the Ksp for Mn(OH)2 is, Ksp=[Mn2+][OH]2

The reaction at equilibrium is,

Mn(OH)2(s)Mn2+(aq)+2OH(aq)

Formula

The solubility product of CaF2 is calculated as,

Ksp=[Mn2+][OH]2

Where,

• Ksp is solubility product.
• [Mn2+] is equilibrium concentration of Mn2+ .
• [OH] is equilibrium concentration of OH .

The [Mn2+] is 3.7×10-5M_ .

The dissociation reaction of HF is,

Mn(OH)2(s)Mn2+(aq)+2OH(aq)

This reaction takes place in water that already contains 107M OH ions, formed by the self-ionization of water.

The ICE table is formed for the stated reaction.

Mn(OH)2(s)Mn2+(aq)+2OH(aq)Initialconcentration01.0×107Change+x(1.0×107)+2xEquilibriumconcentrationx(1.0×107)+2x

The equilibrium concentration of [Mn2+] is xM .

The equilibrium concentration of [OH] is ((1.0×107)+2x)M .

The given value of Ksp of Mn(OH)2 is 2.0×1013 .

The calculated value of [Mn2+] is xM .

The calculated value of [OH] is ((1

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