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:

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:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 52E: The concentration of Mg2+ in seawater is 0.052 M. At what pH will 99% of the Mg2+ be precipitated as...

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Calculate K for the reactions in Question 2.
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
A 25.0 mL aqueous solution of 0.150 mol L-1 Co3+(aq) was prepared. To this solution, 0.0500 mol of NH3 is added. What is the concentration of Co3+ once equilibrium is reached at 25⁰C? (Kf([CO(NH3)6]3+) = 2.3 × 1033) a. 3.7 × 10-35 mol L-1 b. 8.9 × 10-33 mol L-1 c. 4.6 × 10-32 mol L-1 d. 1.1 × 10-38 mol L-1 e. 4.9× 10-34 mol L-1
What must be the correct equilibrium expression for the reaction; CO2(g) <−> CO(g) + O2(g) Ke = ? When Ke = [C] [D] [A] [B]
What is the equilibrium molar concentration of Cu+ in a solution prepared by adding 0.1558 mol of CuNO3 to a solution of CN-? The final volume of the solution was 1.00 L and the concentration of CN- was 2.7046 M before equilibrium was established.Cu+(aq) + 2CN-(aq)↔[Cu(CN)2]-(aq) Kf = 1.00e16 a) 2.79E-18 b) 9.05E-17 c) 2.09E-18 d) 3.71E-18
What is the equilibrium molar concentration of Cu+ in a solution prepared by adding 0.1558 mol of CuNO3 to a solution of CN-? The final volume of the solution was 1.00 L and the concentration of CN- was 2.7046 M before equilibrium was established.Cu+(aq) + 2CN-(aq)↔[Cu(CN)2]-(aq) Kf = 1.00e16
4. If 283.0 mg of AgBr is completely dissolved in 143.0 mL of 0.2 M NH3, what is the equilibrium concentration of Ag* (aq) in the final solution? K[Ag(NH3)2] = 1.7E7 Include at least 3 significant figures in your answer. M Grade This Exercise 5. The acid ionization constant of Fe(H₂O)2+ (aq) is 3E-6. Compute the pH of a 0.11 M aqueous solution of Fe(NO3)2- Include at least 3 significant figures in your answer. D Grade This Exercise 6. Compute the solubility of Mg(OH)2 in a buffer solution at pH=10.71. The solubility product of magnesium hydroxide is 1.2E-11 Include at least 3 significant figures in your answer. D M
What is the solubility product expression for Al(OH)3? Ksp = [A1³+][3OH-] Ksp = [A1³+][OH-]³ O Ksp = [A1³+][3OH-]³ O Ksp = [A1³+][OH-] O Ksp = 3[A1³+][OH-]³
Write K expression for the following reaction: 2H2O2(aq) ↔ 2H2O(l) + O2(g)
Predict the products of each reaction, and whether the solution at equilibrium will be acidic, basic, or neutral. At equilibrium the solution is...? reaction acidic N,0,(s) + 3H,0(1) → 0 basic neutral O acidic co, (g) + H,0(1) basic neutral acidic Na, 0 (s) + H,0(1) - 0 basic neutral
(ii) Calculate the pH of a 0.250 M solution of a weak acid with Ka = 2.5 x 107 [HA] [H'] (A'] initial change equilibrium
1.Calculate the normality of the solutions containing 5.267g/L K2Cr2O7 (the Cr is reduced to Cr3+).(FW=294.19 g/mol) 2.A and B react as follows: A + B 2C. The equilibrium constant is 5.0 x 106. If 0.40 mol of Aand 0.70 mol of B are mixed in 1L, what are the concentrations of A, B and C after reaction? 3. The following data is given at a certain temperature:(1) 2N2 (g) + O2 (g) 2N2O (g) K1 = 1.2 x 10-35(2) N2O4 (g) 2NO2 (g) K2 = 4.6 x 10-3(3) ½N2 (g) + O2 (g) NO2 (g) K3 = 4.1 x 10-9Calculate the molar equilibrium constant, K for the reaction:2N2O (g) + 3O2 (g) 2N2O4 (g)