Consider the dissolution of the metal salt MX2 in water and its subsequent interaction with the ligand L: MX-(s) M2 + (aq) + 2X(aq) M2+(aq) + 2L(aq) = ML:(aq) Given the equilibrium constants: Ksp (MX) = 4.0 x 10-12 Kf (for ML formation) = 1.0 x 106 If the solution is saturated with respect to MX, and 0.1 M L is added, what is the molar solubility of MX, in this solution?

Given that the Gf for Pb2+(aq) and Cl-(aq) is -24.3 kJ/mole and -131.2 kJ/mole respectively, determine the solubility product, Ksp, for PbCl2(s).

The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)

The blue complex Cu(H,O);+ and the yellow complex CuCl- exist in equilibrium. Cu(H, O);+(aq) + 4 CI¯(aq) = CuCl (aq) + 4 H, O(1) Upon addition of LiCl to this equilibrium in solution, which observation would be expected? The solution turns blue. The solution turns yellow. The Cu2+ salts precipitate out of solution. The volume of water decreases. Incorrect O O O

In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoClą2-. Co2+(aq) is pink and CoCl42-(aq) is blue. At Low Temperature the pink color predominates. At High Temperature the blue color is strong. If we represent the equilibrium as: Coclą2 (aq) = Co2*(aq) + 4CI(aq) We can conclude that: 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of Co2+: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.

The fictitious complex M(SCN)2 can be produced from an aqueous equilibrium in which the M2+ ion is mixed with the thiocyanate ion. A solution containing initial concentrations of M2+ and SCN- are 0.000100 M and 0.000300 M  respectively has an equilibrium concentration of M(SCN)2 of 2.00 x 10-5 M. What are the equilibrium concentrations of the two starting ions and what is the value of the equilibrium constant? [M2+] = ___ x 10__ M [SCN-]= ___ x 10__ M Kc = ___ x 10 __

In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl². Co²+ (aq) is pink and CoC14² (aq) is blue. At low temperature the pink color predominates. At high temperature the blue color is strong. If we represent the equilibrium as: Co²+ (aq) + 4C1 (aq) = CoCl₂² (aq) We can conclude that: 1. This reaction O exothermic. O endothermic. Oneutral. O More information is needed to answer this question. 2. When the temperature is increased the equilibrium constant, K: O increases. Odecreases. O remains the same. O More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of Co²+: O increases. Odecreases. O remains the same. OMore information is needed to answer this question. Previc

Consider the following reaction, which is endothermic in the forward direction Fe+3(aq) + NCS-(aq) ↔ FeNCS+2 (aq)               yellow.           colorless      blood red If Fe+3 can make complex ions with chloride ions and hydrogen phosphate ions, can be reduced by Sn2+ ions, and can precipitate with hydroxide ions (becoming colourless in all cases), what would be the colour of the equilibrium under the condition of the following stressors? (ie. Which way would it shift)  The addition of HCl The addition of strong base The addition of Fe(NO3)3 Heating the solution Increasing the pressure surrounding the solution

7. Given the following equilibrium constants, Cd(103)2 Ksp = 2.3 × 10¬8 Cd(NH3)4* Kr = 1.0 × 10' ( Cd²*(aq) + 4NH3 (aq)→ Cd(NH3)a²* (aq)) determine the equilibrium constant K for the dissolution of the sparingly soluble salt Cd(IO3)2 in aqueous ammonia (shown below): Cd(1O3)2(s) + 4NH3(aq) %3D %3D - Cd(NH3)42*(aq) + 2103-(aq) a) 0.23 b) 2.3 x 1015 c) 4.3 x 1014 d) 4.3 e) 1.0 x 107 f) none of the above

Consider the insoluble compound silver chloride, AgCl. The silver ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of AgCl (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. 1.6x107. Be sure to specify states such as (aq) or (s). For Ag(NH3)2+, Kf = K= + Use the References to access important values if needed for this question. Submit Answer + Retry Entire Group 2 more group attempts remaining