A solution contains 0.097 M Ce3+, 1.55x10-3 M Ce4+, 1.55x10-3 M Mn2+, 0.097 M MnO4-, and 1.00 M HClO4 (F= 9.649 x 104 C/mol). a) Write a balanced net reaction that can occur between species in this solution. b) Calculate deltaG0 and K for the reaction. c) Calculate E and deltaG for the conditions given. Ce4+ + e- = Ce3+  E0= 1.70 V MnO4- + 8H+ + 5e- = Mn2+ + 4H2O   E0= 1.507 V

It is found that 8.70e-09 g of Ga(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ga(OH)3.The Ksp of Y2(CO3)3 at 25 oC is 1.03e-31. What is the molar solubility of Y2(CO3)3?

2. The popular antacid, Milk of Magnesia, is a suspension of magnesium hydroxide, Mg(OH)2. In water, Mg(OH)2 undergoes the reaction shown in Equation 9. Mg(OH),(s, white) = Mg²+(aq) +20H¯(aq) (Eq. 9) (1) What would you observe if you added an acid to an equilibrium mixture containing MgtOH)2 H water? (2) Write a chemical equation that accounts for the effect of the added acid. (3) Briefly explain how your answer to (1) is consistent with Le Châtelier's principle.

Given that Ksp for AgCl is 1.6E-10 and Kf for Ag(CN)2- is 5.6E8, calculate the concentration of Ag+ when 0.15 M AgNO3 is reacted with 0.25 M KCN.

1. Calculate the concentration of ions in the following saturated solutions: (a) [1'] in Agl solution with [Ag'] = 9.1 x 10° M; Ksp= 8.3 x 107 (b) [A*] in Al(OH); solution with [OH] = 2.9 x 10° M; Ksp = 1.8 x 10 33 2. 2.4414 g sample containing KCI, K;SO4 and inert materials was dissolved in sufficient water to give 250 mL of solution. A Mohr titration of a 50 ml aliquot required 41.36 ml of 0.05818 M AGNO3. A second 50mL aliquot was treated with 40 ml of 0.1083M NaB(CsHs)4. The reaction is NaB(CsHs)a + + KB(CsHs)4s) + Na*. The solid was filtered, redissolved in acetone, and titrated with K* 49.98mL of the AgNO: solution according to the reaction KB(C,H;). + Ag* + AgB(CsHs)46) + K*. Calculate the percentage of KCl and K:SO, in the sample. a. As a food chemist for a major potato chip company, you are responsible for determining the salt content of new potato chip products for the packaging label. The potato chips are seasoned with table salt, NaCl. You weigh out a handful of the chips…

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Given that the Ksp for silver chloride is 1.76 x 10-10, and the Kf of silver(I) diammine cation [Ag(NH3)2 +] is 1.7 x 107, calculate the maximum number of grams of silver chloride that will dissolve in 250.0 mL of a 3.25 M solution of ammonia.

To 200.0 ml of a solution of Al(NO3)3 with concentration (2.000x10^-3) mol L-1, (3.0x10^2) ml of (1.00x10^-1) mol L-1 NaF is added. Determine the concentration of free aluminum ions after equilibrium has been established.(K+(AIF63-) = 7.0 x 1019) Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer units

ΔG = -RT ln Ka, with Ka that represents the association constant for a complex. (a) Write an expression of ΔG as a function of Kd, the dissociation constant for the same process. (b) Calculate the change in ΔG (thus, the value of ΔΔG) if you consider a 10-fold stronger association for the complex (hint: you don’t need to know the actual values of Ka, Kd, or ΔG). Assume the temperature equal to 25°C.

To 200.0 ml of a solution of Al(NO3)3 with concentration (1.000x10^-3) mol L-1, (3.0x10^2) ml of (2.000x10^-1) mol L-1 NaF is added. Determine the concentration of free aluminum ions after equilibrium has been established.(K(AIF63-) = 7.0 x 1019) Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: