An aqueous solution 0-10M H2S ans 0-20M HCl- If the equilibrium constants for the formation of HS- from H2S is 1-0- 10-7 and that of S2- from HS- ions is 1-2- 10-13 then the concentration of S2-ions in aqueous solution is-

The correct option is C 3× 10^ 20 0.1 αH_2S⇋0.2+2 α2H^+ + αS^2 Keq = K_1 × K_2 = 1.2 × 10^ 20 ∴ 1.2× 10^ 20 =(0.2+2α)^2(α)0.1 α As Ke ...

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Byju's Answer

Standard XII

Chemistry

Order of Reaction

An aqueous so...

Question

An aqueous solution $0.10 M H_{2} S$ ans $0.20 M H C l$ . If the equilibrium constants for the formation of $H S^{-}$ from $H_{2} S$ is $1.0 \times 10^{- 7}$ and that of $S^{2 -}$ from $H S^{-}$ ions is $1.2 \times 10^{- 13}$ then the concentration of $S^{2 -}$ ions in aqueous solution is:

6 \times 10^{- 21}

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5 \times 10^{- 19}

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5 \times 10^{- 8}

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3 \times 10^{- 20}

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Solution

The correct option is C $3 \times 10^{- 20}$
$H_{2} S 0.1 - α ⇋ 2 H^{+} 0.2 + 2 α + S^{2 -} α$

$K e q = K_{1} \times K_{2} = 1.2 \times 10^{- 20}$

$∴ 1.2 \times 10^{- 20} = \frac{(0.2 + 2 α)^{2} (α)}{0.1 - α}$

As $K e q$ is too small, $α <<< 0.1$
$∴ 0.2 + 2 α = 0.2$
$∴ {0.2}^{2} \times α = 1.2 \times 10^{- 21}$
$∴ α = 3 \times 10^{- 20}$

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An aqueous solution 0.10MH2S ans 0.20MHCl. If the equilibrium constants for the formation of HS− from H2S is 1.0×10−7 and that of S2− from HS− ions is 1.2×10−13 then the concentration of S2−ions in aqueous solution is:

The correct option is C 3×10−20H2S0.1−α⇋2H+0.2+2α+S2−αKeq=K1×K2=1.2×10−20∴1.2×10−20=(0.2+2α)2(α)0.1−αAs Keq is too small, α<<<0.1∴0.2+2α=0.2 ∴0.22×α=1.2×10−21∴α=3×10−20

An aqueous solution $0.10 M H_{2} S$ ans $0.20 M H C l$ . If the equilibrium constants for the formation of $H S^{-}$ from $H_{2} S$ is $1.0 \times 10^{- 7}$ and that of $S^{2 -}$ from $H S^{-}$ ions is $1.2 \times 10^{- 13}$ then the concentration of $S^{2 -}$ ions in aqueous solution is: