Which of the following happens when NH4OH is added gradually to the solution containing 1M A2+ and 1MB3+ ions ?Given : KspA(OH)2=9×10−10 and KspB(OH)3=27×10−18 at 298 K.

A(OH) 2 and B(OH) 3 will precipitate together

Which of the following happens when NH4OH is added gradually to the solution containing 1M A2+ and 1MB3+ ions ?Given : KspA(OH)2=9×10−10 and KspB(OH)3=27×10−18 at 298 K.

A(OH) 2 and B(OH) 3 will precipitate together

B(OH) 3 will precipitate before A(OH) 2

Both A(OH) 2 and B(OH) 3 do not show precipitation with NH 4 OH

A(OH) 2 will precipitate before B(OH) 3

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Which of the following happens when NH₄OH is added gradually to the solution containing 1M A²⁺ and 1MB³⁺ ions ?
Given : $K_{sp} [A (OH)_{2}] = 9 \times 10^{- 10}$ and $K_{sp} [B (OH)_{3}] = 27 \times 10^{- 18}$ at 298 K.

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A(OH)₂ and B(OH)₃ will precipitate together

B(OH)₃ will precipitate before A(OH)₂

Both A(OH)₂ and B(OH)₃ do not show precipitation with NH₄OH

A(OH)₂ will precipitate before B(OH)₃

answer is A.

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Detailed Solution

Condition for precipitation $Q_{ip} > K_{sp}$

$\begin{array}{l} \begin{aligned} For [A (OH)_{2}] \\ [A^{2 +}] {[{OH}^{-}]}^{2} > 9 \times 10^{- 10} \\ [A^{+ 2}] = 1 M \\ \Rightarrow [{OH}^{-}] > 3 \times 10^{- 5} M \end{aligned} \\ For [B (OH)_{3}] \\ \begin{aligned} [B^{3 +}] {[{OH}^{-}]}^{3} > 27 \times 10^{- 18} \\ [B^{3 +}] = 1 M \\ \Rightarrow [{OH}^{-}] > 3 \times 10^{- 6} M \end{aligned} \end{array}$

So, B(OH)₃ will precipitate before A(OH)₂

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