If given the following solubilities, how do you calculate the $K_{s p}$ $K_(sp)$ for each compound?

Question

If given the following solubilities, how do you calculate the $K_{s p}$ $K_(sp)$ for each compound?

(a) $C u S C N$ $CuSCN$ , 5.0 mg/L
(b) $S n S$ $SnS$ , 2.0 x $10^{- 5}$ $10^-5$ g/L
(c) $C o {(O H)}_{2}$ $Co(OH)_2$ , 3,2 x $10^{3}$ $10^3$ g/L
(d) $A g_{2} C r O_{4}$ $Ag_2CrO_4$ , 3.4 x $10^{- 2}$ $10^-2$ g/L?

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Answer 1 · 2018-06-02T20:40:19

I will do you ONE example..... $d .$ $d.$

Explanation:

We examine the solubility equilibrium...

$A g_{2} C r O_{4} (s) H_{2} O ⇌ 2 A g^{+} + C r O_{4}^{2 -}$ $Ag_2CrO_4(s) stackrel(H_2O)rightleftharpoons2Ag^+ + CrO_4^(2-)$

For which we write the solubility expression....

$K_{sp} = {[A g^{+}]}^{2} [C r O_{4}^{2 -}]$ $K_"sp"=[Ag^+]^2[CrO_4^(2-)]$

But if $S = solubility of silver chromate...$ $S="solubility of silver chromate..."$ , then $[A g^{+}] = 2 S$ $[Ag^+]=2S$ , and $[C r O_{4}^{2 -}] = S$ $[CrO_4^(2-)]=S$ ...thus $K_{sp} = {(2 S)}^{2} S = 4 S^{3}$ $K_"sp"=(2S)^2S=4S^3$ ...

Now $S = \frac{\frac{3.4 \times 10^{- 2} \cdot g}{331.73 \cdot g \cdot m o l^{- 1}}}{1 \cdot L} = 1.0025 \times 10^{- 4} \cdot m o l \cdot L^{- 1}$ $S=((3.4xx10^-2*g)/(331.73 *g*mol^-1))/(1*L)=1.0025xx10^-4*mol*L^-1$ ...

$K_{sp} = 4 \times {(1.0025 \times 10^{- 4})}^{3} = 4.03 \times 10^{- 12}$ $K_"sp"=4xx(1.0025xx10^-4)^3=4.03xx10^-12$ .

When you do the others perhaps you might post the solutions in this thread?

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If given the following solubilities, how do you calculate the $K_{s p}$ $K_(sp)$ for each compound?

(a) $C u S C N$ $CuSCN$ , 5.0 mg/L
(b) $S n S$ $SnS$ , 2.0 x $10^{- 5}$ $10^-5$ g/L
(c) $C o {(O H)}_{2}$ $Co(OH)_2$ , 3,2 x $10^{3}$ $10^3$ g/L
(d) $A g_{2} C r O_{4}$ $Ag_2CrO_4$ , 3.4 x $10^{- 2}$ $10^-2$ g/L?

1 Answer

Explanation:

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If given the following solubilities, how do you calculate the KspK_(sp) for each compound?

(a) CuSCNCuSCN, 5.0 mg/L (b) SnSSnS, 2.0 x 10−510^-5 g/L (c) Co(OH)2Co(OH)_2, 3,2 x 10310^3 g/L (d) Ag2CrO4Ag_2CrO_4, 3.4 x 10−210^-2 g/L?

1 Answer

Explanation:

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Impact of this question

If given the following solubilities, how do you calculate the $K_{s p}$ $K_(sp)$ for each compound?

(a) $C u S C N$ $CuSCN$ , 5.0 mg/L
(b) $S n S$ $SnS$ , 2.0 x $10^{- 5}$ $10^-5$ g/L
(c) $C o {(O H)}_{2}$ $Co(OH)_2$ , 3,2 x $10^{3}$ $10^3$ g/L
(d) $A g_{2} C r O_{4}$ $Ag_2CrO_4$ , 3.4 x $10^{- 2}$ $10^-2$ g/L?