A mixture of weak acid is $$0.1$$ M in HCOOH (Ka$$ $$=$$ $$1.8$$ × $$10-4) and $$0.1$$ M in HOCN (Ka$$ $$=$$ $$3.1$$ ×$$10-4). [$$H3O+$$] of mixture is x × $$10-3$$ . Value of x is . . . . .

H⊕$$mix=$$Σ$$KaiCi=1.8$$×$$10$$−$$4$$×$$0.1+3.1$$×$$10$$−$$4$$×$$0.1=4.9$$×$$10$$−$$5M=7$$×$$10$$−$$3MThus$$ x is $$7$$.

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Ionic equilibrium

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Question

A mixture of weak acid is 0.1 M in HCOOH (K_a = 1.8 × 10^-4) and 0.1 M in HOCN
(K_a = 3.1 ×10^-4). [H₃O⁺] of mixture is x × 10^-3 . Value of x is . . . . .

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Solution

$\begin{array}{l} {[H^{\oplus}]}_{mix} = \sqrt{Σ K_{a i} C_{i}} \\ = \sqrt{1.8 \times 10^{- 4} \times 0.1 + 3.1 \times 10^{- 4} \times 0.1} \\ = \sqrt{4.9 \times 10^{- 5}} M = 7 \times 10^{- 3} M \end{array}$
Thus x is 7.

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