At 25 degree C, the value for K_sp(Pnl_2) = 1.4 10^-8. Calculate the molar solub

Question

At 25 degree C, the value for K_sp(Pnl_2) = 1.4 10^-8. Calculate the molar solubility of Pbl_2 in pure water. Pnl(s) doubleheadarrow Pn^2+_(aq) + 2l^-_(aq) Calculate the molar solubility of Pbl_2, in o.200M Pb(NO_3)_2 solution. The solubility of Pbl_2 in pure water is: a) less than b) almost the same c) impossible to predict d) greater than the solubility of Pbl_2 in Kl solution. Predict the sign of the entropy change of the system (Delta S) ("0", > 0, or 0 Delta S? A B C D 2. 2 Fe_(s) + 3/2 O_2(g) rightarrow Fe_2O_3(s) Delta H 0 Delta S? A B C D 4. 2C_4H_10 (e)+ l3O_2(g) rightarrow 8CO_2(g) + 10H_2O(g) Delta H

Explanation / Answer

Diassociation of PbI2 is

PbI2 (aq) <----> Pb2+ (aq) + 2 I- (aq)

1 mole 1 mole 2 mole

Let x moles be diassociated so x moles of Pb2+ will be present and 2x moles of I- will be present

Ksp = [Pb2+] [I-] = x * (2x)2 = 1.4 * 10-8

3 x3 =  1.4 * 10-8

x =  1.67 * 10-3

Molar solubility is 1.67 * 10-3

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