The solubility of Mg_3(PO_4)_2 in pure water is 8.6 times 10^-6 M in pure water

Question

The solubility of Mg_3(PO_4)_2 in pure water is 8.6 times 10^-6 M in pure water at 25 degree C. What is the value of K_sp for this compound at 25 degree C? (a) 2.9 times 10^-3 (b) 2.5 times 10^-15 (c) 1.3 times 10^-30 (d) 5.1 times 10^-24 (e) 4.7 times 10^-26 What will happen if HCl is added to a saturated aqueous solution of Mg_3(PO_4)_2 in water? ("Saturated solution" means that there is solid Mg_3(PO_4)_2 present and the system is at equilibrium.) (a) Nothing happens (b) The Mg_3(PO_4)_2 solubility equilibrium shifts to the RIGHT and more solid Mg_3(PO_4)_2 dissolves. (c) The Mg_3(PO_4)_2 solubility equilibrium shifts to the LEFT and more Mg_3(PO_4)_2 precipitates out of solution. (d) The Mg_3(PO_4)_2 solubility equilibrium shifts to the RIGHT and more Mg_3(PO_4)_2 precipitates out of solution. (e) The Mg_3(PO_4)_2 solubility equilibrium shifts to the LEFT and more solid Mg_3(PO_4)_2 dissolves. Ru^3+ ion forms a complex ion with 6 ammonia molecules. What is the K_f expression for the formation this complex ion? (a) [Ru^3+] [NH_3]^6/[Ru(NH_3)^3+_4] (b) [Ru^3+] [NH^+_4]^6 (c) [Ru^3+][NH_3]_6 (d) [Ru(NH^+_4)^3+_4]/[Ru^3+] [NH^+_4]^6 (e) [Ru(NH)^3+_4/[Ru^3+] [NH_3]^6 What is the maximum amount of potassium fluoride (M_w = 58.1g/mol) that can be added to 100. mL of a 1.0 times 10^-4 M solution of lead(II) nitrate without precipitating out lead(II) fluoride? K_sp of lead(II) fluoride = 3.6 times 10^-8 (a) 0.080 g (b) 1.5 times 10^-3 g (c) 0.11 g (d) 2.1 times 10^-3 g (e) 7.2 times 10^-5 g Degree of dissociation a for a weak acid HA is defined as, alpha = [H_3O^+]/C_HA where C_HA is the total concentration of HA. How alpha will depend on acid dissociation equilibrium constant K_a if C_NA >> K_a (a) alpha = 1/C_HA (b) alpha = -K_a - Squareroot K^2_a - 4K_a C_NA (c) alpha = Squareroot K_a/C_NA (d) alpha = Squareroot K_a C_HA (e) alpha = K_a C_NA Consider the dissolution of MnS in water (K_sp = 3.0 times 10^-14). MnS(s) + H_2O(l) Mn^2+ (aq) + HS^-(aq) + OH^-(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system? (a) The solubility will be unchanged. (b) The solubility will decrease (c) The solubility will increase. (d) The amount of KOH added must be known before its effect can be predicted. (e) The pK_a of H_2S is needed before a reliable prediction can be made.

Explanation / Answer

Ksp = [Mg2+]3 [PO43-] 2

Therefore

Ksp = (8.6*10-6)3 * (8.6*10-6)2

= (8.6*10-6)5

= 4.7042702*10-26

Thank you and good luck.

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