Why are these solved differently? i need an explanation not just a quick answer. The Ksp...

Why are these solved differently? i need an explanation not just a quick answer.

The K_sp of Al(OH)₃ is 1.0 x 10^-33. What is the solubility of Al(OH)₃ in 0.00010 M Al(NO₃)_{3? answer is
(7.2x10^-11)}

The K_sp of Al(OH)₃ is 1.0 x 10^-33. What is the solubility of Al(OH)₃ in 0.000010 M NaOH? answer is (1.0x10^-18)

Expert Solution

In the first case we have a aluminium nitrate Al(NO3)3 with aluminium hydroxide Al(OH)3 hence aluminium nitrate is highly soluble and dissociates completely in its ions. Finally we have a additional moles of Al3+ due to aluminium nitrate dissociation it means that in the Ksp equation we have to take total concentration of Al3+ and OH- .We also assume that 's' is the solubility of the ions and its is very small as compared to 0.00010M. After that equating all these values we have a solubility data.

In second part instead of nitrate we have strong base NaOH which dissociates into its ions i.e Na+ and OH- completely.Therefore overall we have additional hydroxide concentration along with hydroxide that are coming from aluminium hydroxide.Therefore in Ksp equation we have to take total concentration of OH- and Al3+ and solve the equation..we get solubility.

queen_honey_blossom answered 10 months ago

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Why are these solved differently? i need an explanation not just a quick answer. The Ksp...

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