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What is the pH at which Mg(OH)(2) begins...

What is the pH at which `Mg(OH)_(2)` begins to precipitate from a solution containing 0.1 M `Mg^(2+)` ions ? `[K_(sp)" for "Mg(OH)_(2)=1.0xx10^(-11)]`

Text Solution

Verified by Experts

`K_("sp") Mg(OH)_(2) = 1.0 xx 10^(-11) = [Mg^(2+)][OH^(-)]^(2)`
`1.0 xx 10^(-11) = (0.10) [OH^(-)]^(2)`
` [OH^(-)] = 1 xx 10^(-5) " " [H^(+)] = (1xx10^(-14))/(1 xx 10^(-5)) = 1 xx 10^(-9)`
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Which of the following concentration of NH_(4)^(+) will be sufficient to present the precipitation of Mg(OH)_(2) form a solution which is 0.01 M MgCl_(2) and 0.1 M NH_(3)(aq) . Given that K_(sp)Mg(OH)_(2)=2.5xx10^(-11) and K_(b) for NH_(3) = 2xx10^(-5) .

Knowledge Check

  • Calculate pH at which Mg(OH)_(2) begins to precipitate from a solution containing 0.10M Mg^(2+) ions. (K_(SP)of Mg(OH)_(2)=1xx10^(-11))

    A
    4
    B
    6
    C
    9
    D
    7

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