The solubility product constant, Ksp, of the aluminum hydroxide, Al(OH)₃ at the temperature is 1.91×10¯³⁹
<h3>What is solubility of product? </h3>
The solubility of product (Ksp) is defined as the concentration of products raised to their coefficient coefficients. This is illustrated below:
mA <=> nC + eD
Ksp = [C]^n × [D]^e
With the above information in mind, we can obtain the solubility of the product. This is illustrated below:
<h3>Dissociation equation </h3>
Al(OH)₃(aq) → Al³⁺(aq) + 3OH¯(aq)
From the balanced equation above,
1 mole of Al(OH)₃ contains 1 mole of Al³⁺ and 3 moles of OH¯
<h3>How to determine the concentration of Al³⁺ and OH¯</h3>
From the balanced equation above,
1 mole of Al(OH)₃ contains 1 mole of Al³⁺ and 3 moles of OH¯
Therefore,
2.9×10¯⁹ M Al(OH)₃ will also contain
- 1 × 2.9×10¯⁹ = 2.9×10¯⁹ M Al³⁺
- 3 × 2.9×10¯⁹ = 8.7×10¯⁹ M OH¯
<h3>How to determine the solubility of product </h3>
Concentration of Al³⁺ = 2.9×10¯⁹ M
Concentration of OH¯ = 8.7×10¯⁹ M
Solubility product (Ksp) =?
Al(OH)₃(aq) → Al³⁺(aq) + 3OH¯(aq)
Ksp = [Al³⁺] × [OH¯]³
Ksp = 2.9×10¯⁹ × (8.7×10¯⁹)³
Ksp = 1.91×10¯³⁹
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