A sparingly soluble salt silver phosphate, Ag3PO4, is in equilibrium with its ions in solution according to the following equation A93PO4(s) = 3 Ag*(aq) + PO-(aq) Write an expression for Ksp of Ag3PO4 The solubility of silver phosphate, Ag3PO4, at 25°C is 1.59 x 10 mol/L. What is the Kgp for the silver phosphate at 25°C?

A sparingly soluble salt silver phosphate, Ag3PO4, is in equilibrium with its ions in solution according to the following equation A93PO4(s) = 3 Ag*(aq) + PO-(aq) Write an expression for Ksp of Ag3PO4 The solubility of silver phosphate, Ag3PO4, at 25°C is 1.59 x 10 mol/L. What is the Kgp for the silver phosphate at 25°C?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 80AP

See similar textbooks

Similar questions

The solubility product constant, Ksp, at 25°C for AgI(s) in water has the value 8.3 × 10–17. Calculate ΔG at 25°C for the process AgI(s) ⟷⟷ Ag+(aq) + I–(aq) where [Ag+] = 9.1 × 10–9 M and [I–] = 9.1 × 10–9 M. (R = 8.314 J/K • mol)
Certain bacteria in the soil obtain the necessary energy for growth by oxidizing nitrite to r nitrate: 2NO2- (aq) + O2(g) —> 2NO3-(aq) Given that the standard Gibbs energies of formation of NO2- and NO3- are -34.6 kJ mol-1 and -110.5 kJ mol-1, respectively, calculate the amount of Gibbs energy released when 1 mole of No2- is oxidized to 1 mole of NO3-.
The hardness of water (hardness count) is usually expressed in parts per million (by mass) of CaCO3. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 175mg CaCO3il? How many milliliters of concentrated sulfuric acid, 94.0% (w/w), specific gravity of 1.831 are required to prepare 1 liter of a 0.100 M solution? The solubility-product constant for Ce(IO3)3 is 3.2x1010. What is the Ce3+ concentration in a solution prepared by mixing 50.0 ml of 0.0250 M Ce3.. with 50.00 ml of water?
4.32) Certain bacteria in soil obtain the necessary energy for growth by oxidizing nitrite to nitrate: 2NO2- (aq) + O2 (g) —-> 2NO3- Given that the standard Gibbs energies of formation of NO2- and NO3- are -34.6 kJ mol-1 and -110.5 kJ mol-1, respectively, Calculate the amount of Gibbs energy released when 1 mole of NO2- is oxidized to 1 mole of NO3-.
Determine the solubility product constant (Ksp) of borax, a slightly soluble sodium salt, in water at two different temperatures and evaluate the enthalpy, entropy and Gibbs free energy change for dissolving borax in water. The equilibrium expression for the process is: Na2B4O5(OH)4 10H2O (s) ⇌ 2 Na+ (aq) + B4O5(OH)4 2- (aq) + 10H2O(l) Since liquid water and solid borax are not included in the Ksp expression, the solubility product expression associated with this reaction is: Ksp = [Na+]2[borate] The concentration of the borate ion in equilibrium with solid borax can be determined by titration with HCl based on the following equation: B4O5(OH)42- + 2HCl(aq) + 3H2O (l) → 4 H3BO3(aq)+2Cl-(aq) The Ksp for borax will be evaluated at room temperature at 5oC. Knowing the Ksp values at two temperatures allows the use of the following equations to calculate the change in enthalpy and Gibbs free energy: In(Ksp1/Ksp2)=ΔH/R((1/T2)-(1/T1)) ΔGo= - RT InKsp Once ΔHo and ΔGo are known, you can find…
Another metal phosphate is cobalt(III) phosphate. It will behave similar to calcium phosphate in an acid solution, and will form an equilibrium between reactants and products. What is the net ionic equation including phases for CoPO4(s) dissolving in H3O+(aq) ?
Estimate the temperature at which the equilibrium constant for the decomposition of CaCO3(s, calcite) to CO2(g) and CaO(s) becomes 1; assume pCO2 = 1 bar .
Calculate the percentage change in Kx for the reaction H2CO(g) ⇋ CO(g) + H2(g) when the total pressure is increased from 1.0 bar to 2.0 bar at constant temperature.
The solubility of Sb2S3 in water is 1.0×10−5 mol / litre at 298 K. What will be its solubility product
Assume that the solubility of carbon dioxide gas in pop at 5oC is 0.586 g/100 mL and at 20oC its solubility is 0.169 g/100 mL. What mass of carbon dioxide gas will escape from a 355-mL can of Coke that has been taken out of the fridge and has been sitting open at 20oC?
For the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium in J/mol? The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 81 oC is Keq = 478,789. (b) What is the standard reaction Gibbs energy of this reaction in J/mol?
1. Write and balance the chemical equation where KOH and HCL reacts. 2. calculate ΔHb for the reaction involving K with HCl. Report your value in units of kJ/mole. 3. Calculate ΔH for the reaction involving MgO and HC1. KOH (s) + HCl (aq) → KCl (aq) + H2O (I) ΔH=