Calculate the pH of 6-66 - 10-3 M solution AlOH3 its first dissociation is 100

Al(OH)_3⇌ Al(OH)_2^+ + OH^ [OH^ ]=6.66 × 10^ 3 (α = 100%) Al(OH)_2^+ ⇌ Al(OH)^+2 + OH^ [OH^ ]= 3.33 × 10^ 3 (α = 50%) Total [OH]^ = 6.66 × 10^ 3+3.33 × 10 ...

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Standard XI

Chemistry

pH the Power of H

Calculate the...

Question

Calculate the pH of $6.66 \times 10^{- 3} M$ solution $A l (O H)_{3}$ its first dissociation is 100% whereas second dissociation is 50% and third dissociation is negligible.

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Solution

The correct option is B 12
$A l (O H)_{3} ⇌ A l (O H)_{2}^{+} + O H^{-} [O H^{-}] = 6.66 \times 10^{- 3} (α = 100 %) A l (O H)_{2}^{+} ⇌ A l (O H)^{+ 2} + O H^{-} [O H^{-}] = 3.33 \times 10^{- 3} (α = 50 %)$
Total $[O H]^{-} = 6.66 \times 10^{- 3} + 3.33 \times 10^{- 3} = 10 \times 10^{- 3}$
Total $[O H]^{-} = 10^{- 2}$
$p O H = - l o g [O H^{-}]$
$p O H = - l o g 10^{- 2}$
$p O H = 2$
also, $p H + p O H = 14$
$p H + 2 = 14$
$p H = 12$
$∴ p H = 12$

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pH the Power of H

Standard XI Chemistry

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Calculate the pH of 6.66×10−3 M solution Al(OH)3 its first dissociation is 100% whereas second dissociation is 50% and third dissociation is negligible.

The correct option is B 12Al(OH)3⇌Al(OH)+2+OH−[OH−]=6.66×10−3(α=100%)Al(OH)+2⇌Al(OH)+2+OH−[OH−]=3.33×10−3(α=50%) Total [OH]−=6.66×10−3+3.33×10−3=10×10−3 Total [OH]−=10−2 pOH=−log [OH−] pOH=−log 10−2 pOH=2 also, pH+pOH=14 pH+2=14 pH=12 ∴ pH=12

Calculate the pH of $6.66 \times 10^{- 3} M$ solution $A l (O H)_{3}$ its first dissociation is 100% whereas second dissociation is 50% and third dissociation is negligible.