Which is the molar solubility of BaF_2 in a 0.0750 M LiF solution. K_sp (BaF_2)

Question

Which is the molar solubility of BaF_2 in a 0.0750 M LiF solution. K_sp (BaF_2) = 1.7 ties 10^-6 M^2, 0.0750 M 2.3 times 10^-5 M 1.2 times 10^-2 M 3.0 times 10^-4 M which of the following processes have a delta S > 0? 2 HBr(g) rightarrow H_2(g) rightarrow H_2(g) + Br_2(1) 2 NH_3(g) + CO_2(g) rightarrow NH_2CONH_2(aq) + H_2O(I) lithium fluoride forms from its elements sodium chloride dissolves in pure water All of the above processes have a delta s > 0. Consider a reaction that has a positive delta H and a positive delta S. Which of the following statements is TRUE? This reaction will be nonspontaneous at all temperatures. This reaction will be spontaneous at all temperatures. This reaction will be nonspontaneous only at low temperatures. This reaction will be spontaneous only at low temperatures. It is not possible to determine without more information. Determine delta G degree_rxn for the following reaction at 318 K. CaCO_3 rightarrow CaO(s) + CO_2(g) delta H degree = +179.2 kj;delta s degree = +160.2 J/K +128.3 kJ -230.1kJ +230.1 kJ +179.2 kJ -128.3 kJ

Explanation / Answer

16)

BaF2 ----> Ba2+ + 2 F-

   s 7.5*10^-2 + 2s

LiF here is Strong electrolyte

It will dissociate completely to give [F-] = 0.075 M

At equilibrium:

Ksp = [Ba2+][F-]^2

1.7*10^-6=(s)*(7.5*10^-2+ 2s)^2

Since Ksp is small, s can be ignored as compared to 7.5*10^-2

Above expression thus becomes:

1.7*10^-6=(s)*(7.5*10^-2)^2

1.7*10^-6= 1(s)^1 * 5.625*10^-3

s = 3.0*10^-4 M

Answer: D

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