14. The Kp for the dissociation of solid GaPO, in water is given by [Ga* ][PO,3-] [GAPO4] A) [GAPO4] (Ga³* ][PO,¯] Ksp B) g Ksp =[Ga³* ][PO,³- Kp =[Ga³*]°[PO,³¬ D) Ksp ds, a =[Ga³* ][p$* ]o²-r*
Q: Using the data in the table, calculate Kp and AG for this reaction at 25°C. PCl;(g) = PCl;(g) +…
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Q: The Kp for the reaction A (g) ⇌ 2 B (g) is 0.0650. What is Kp for the reaction 2 A (g) ⇌ 4 B (g)?
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- The following question is taken from a Chemistry Advanced Placement Examination and is used with the permission of the Educational Testing Service. Solve the following problem: MgF2(s)Mg2+(aq)+2F(aq) In a saturated solution of MgF2 at 18 C, the concentration of Mg2+ is 1.21103M . The equilibrium is represented by the preceding equation. (a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 C. (b) Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 18 C to which 0.100 mol of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible. (c) Predict whether a precipitate of MgF2 will form when 100.0 mL of a 3.00103 -M solution of Mg(NO3)2 is mixed with 200.0 mL of a .2.00103 -M solution of NaF at 18 C. Show the calculations to support your prediction.. (d) At 27 C the concentration of Mg2+ in a saturated solution of MgF2 is 1.17103M . Is the dissolving of MgF2 in water all endothermic or an exothermic process? Give an explanation to support your conclusion.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).Hydrogen sulfide is bubbled into a solution that is 0.10 M in both Pb2+ and Fe2+ and 0.30 M in HCl. After the solution has come to equilibrium it is saturated with H2S ( H2S[H2S]=0.10M). What concentrations of Pb2+ and Fe2+ remain in the solution? For a saturated solution of H2S we can use the equilibrium: H2S(aq)+2H2O(l)2H3O+(aq)+S2(aq)K=1.01026 (Hint: The [H3O+] changes as metal sulfides precipitate.)
- . The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.The formation constant* of [M(CN) 2 ]^ - is 5.30 * 10 ^ 18 , where M is a generic metal. A 0.140 mole quantity of M(NO 3 ) is added to a liter of 0.750 M solution. What is the concentration of mathcal W ^ + at equilibrium?[M^+2]=A certain reaction has an equilibrium constant of 10.1 at 25oC. A ⇄ B Determine its ΔG, in kJ/mol, if [A]=0.05 M and [B]=1x10-4 M?
- What are the main equilibria involved in the CO2–Carbonate system and what kind of equilibrium constant is associated with each (K?)? What is the overall reaction for carbonate species in water that is exposed to the atmosphere and carbonate minerals?The solubility product constant for Al(OH)3 is 1.90x10-33, and the formation constant for Al(OH)4– is 7.70x1033 at 25°C. Calculate the value of the equilibrium constant*, K, under standard conditions for: Al(OH)3 (s) + OH- (aq) ------> Al (OH)4 - (aq)Another way to write the equation for the equilibrium includes the waters of hydration: Al(H2O)3(OH)3 (s) + OH- (aq) ------> Al(H2O)2(OH)4- (aq)In nature, silver iodide (AgI) is obtained in the form of the mineral iodargyrite. This compound has a bright yellow color and has a melting point of 552 oC. However, in the laboratory this compound can be prepared by heating a solution of silver nitrate (AgNO3) and an alkaline iodide such as potassium iodide (KI).a. What are the effects of the salts KI and AgNO3 on the solubility of AgI in water? Please describe your answer. b. Describe the effect of the salt KNO3 on the solubility of AgI in water. Explain why it’s different from the effects noted in question 9a?
- Some sulfuric acid is spilled on a lab bench. You can neutralizethe acid by sprinkling sodium bicarbonate on it and thenmopping up the resulting solution. The sodium bicarbonatereacts with sulfuric acid according to:2 NaHCO3(s) + H2SO4(aq)----->Na2SO4(aq) + 2 H2O(l)+ 2 CO2(g)Sodium bicarbonate is added until the fizzing due to the formationof CO2(g) stops. If 27 mL of 6.0 M H2SO4 was spilled,what is the minimum mass of NaHCO3 that must be addedto the spill to neutralize the acid?A solution is prepared such that the initial concentration of Cd2+ is 3.80×10-2 M and the initial concentration of Br- is 7.50×10-2 M. Cd2+and Br- are allowed to react as shown below to establish equilibrium with the complex CdBr42-.The equilibrium concentration of the complex CdBr42- is determined to be 2.9×10-3 M. Cd2+ (aq) + 4 Br- (aq) CdBr42- (aq) What is the formation constant, Kf, for this complex?The solubility of lead(II) chloride, PbCl2 (MM: 278.1 g/mol), in water at 60 °C is 1.94 g/L. a) Calculate the Ksp for lead(II) chloride.