The molal solubility m, of the sparingly soluble salt BaF2 in water at 25°C, following from the dissolution equilibrium BaF2(s) = Ba?+(aq) + 2 F¯(aq) , is ms = 1.830 x 10-2 mol kg¬1. What is the value of the solubility product equilibrium constant Ksp(BaF2) in water at 25 °C? Assume that the Debye-Hückel limiting law for the activity coefficients applies in this situation.

The molal solubility m, of the sparingly soluble salt BaF2 in water at 25°C, following from the dissolution equilibrium BaF2(s) = Ba?+(aq) + 2 F¯(aq) , is ms = 1.830 x 10-2 mol kg¬1. What is the value of the solubility product equilibrium constant Ksp(BaF2) in water at 25 °C? Assume that the Debye-Hückel limiting law for the activity coefficients applies in this situation.

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

At 25 °C, the equilibrium partial pressures for the reaction 2 A(g) + 4B(g) = 2C(g) + D(g) were found to be P = 4.62 bar, P = 4.70 bar, Pe=5.81 bar, and Pp = 5.90 bar. What is the standard change in Gibbs free energy of this reaction at 25 C? AG kJ/mol
What is the A,G for the following reaction (in kJ mol ¹) at 298 K? 2 Si (s) + 3 H2(g) Si₂H6 (g) 1 The conditions for this reaction are: PH2 = 1.21 bar PsizH6 = 0.5 bar. You will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation). A copy of Appendix II has also been posted on eClass. Please use the method of Gibbs energy of formation to calculate ArG" if needed. For partial credit, enter the value of "Q" for this reaction. Answer:
Calculate the equilibrium constant at 37 degree Celsius for the reaction glucose +6O2 +36ADP +36Phosphate => 6CO2 +42H2O +36ATP Where change in G=-423kcal/mole of Glucose
Consider the dissolution of calcium fluoride: CaF2(s) → Ca?*(aq) + 2 F(aq) Part B which has the following standard enthalpy and entropy of reaction: At 368.3 K, the solubility of calcium fluoride is 3.32×10¬4 mol L-1. Compute the Gibbs energy change (A,G) for the reaction if this saturated solution is suddenly cooled to 275.0 K. 1 A:H° = 14.4 kJ mol- A,S° = -149.2 J K-1 mol-1 17.6 kJ mol-1 -10.7 kJ mol-1 0.0 kJ mol-1 25.2 kJ mol-1 3.6 kJ mol-1
Calculate the standard Gibbs energy change for the following reaction at 298 K H2(g) + Cl2(g) ® 2HCl(g) [DfHo = –92.3 kJ mol–1 for HCl; S in J K–1 mol–1 is 131, 223, and 187 for H2, Cl2 and HCl, respectively].
If 2.00 mL of 0.500 M NaOH are added to1.000 Lof0.400 M CaCl2,what is the value of the reaction quotient and will precipitation occur?
Physical Chem #4
ST5G.2 - Estimate the solubility of CaF2(aq) [in units of MICROmolar] in the presence of 0.716 molar CaCl2(aq). Type your answer...