The solubility of Mg ( OH )2 in a particular buffer solution is found to be 0.65 g L -1. Thus, pH of the buffer solution is [Ks p. of .Mg ( OH )2=1.8 × 10-11]

Question

The solubility of Mg ( OH )2 in a particular buffer solution is found to be 0.65 g L -1. Thus, pH of the buffer solution is [Ks p. of .Mg ( OH )2=1.8 × 10-11] (A) 9.6 (B) 5.3 (C) 4.4 (D) 8.7

Tardigrade Admin · Accepted Answer

[ Mg ( OH )2]=0.65 gL -1=(0.65/58) mol L -1 ∴ [ Mg 2+]=(0.65/58) M [ Mg 2+][ OH ]2=Ks p=1.8 × 10-11 ∴ [ OH -]2=1.8 × 10-11 × (58/0.65) =1.606 × 10-9 [ OH- ]=4.0 × 10-5 pOH =4.4 pH =14-4.4=9.6

Q. The solubility of Mg(OH)2​ in a particular buffer solution is found to be 0.65gL−1. Thus, pH of the buffer solution is [Ksp​ of Mg(OH)2​=1.8×10−11]

9.6

5.3

4.4

8.7

[Mg(OH)2​]=0.65gL−1=580.65​molL−1 ∴[Mg2+]=580.65​M [Mg2+][OH]2=Ksp​=1.8×10−11 ∴[OH−]2=1.8×10−11×0.6558​ =1.606×10−9 [OH−]=4.0×10−5 pOH=4.4 pH=14−4.4=9.6

Q. The solubility of $M g (O H)_{2}$ in a particular buffer solution is found to be $0.65 g L^{- 1}$ . Thus, $p H$ of the buffer solution is $[K_{s p}$ of $M g (O H)_{2} = 1.8 \times 1 0^{- 11}]$