For nos. 4 - 7: Consider a saturated solution of barium iodate in 0.025 M BaCl2. Ba(IO3)2(s) = Ba2* + 2103 Ksp = 1.57 x 10-9 at 25°C For the salt: %3D 4. What is the ionic strength of the solution?
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- For nos. 4 - 7: Consider a saturated solution of barium iodate in 0.025 M BaCl2. For the salt: Ba(lO3)2(s) Ba2+ + 21O3 Ksp = 1.57 x 10-9 at 25°CThe equilibrium constant of the reaction 2 C3H6 (g) ⇌ C2H4(g) + C4H8(g) is found to fit the expression InK= -1.04-(1088 K)/T +(1.51 x 10-2 K2)/T2between 300 K and 600 K. (a) Calculate the standard reaction Gibbs energy at each temperature at 390 K and 410 K. (b) Use the van 't Hoff equation to determine the standard reaction enthalpy at 400 K. (c) Hence also calculate the standard reaction entropy at 400 K.The Ksp of Fe3(PO4)2 is 5.51⋅10-21 M. Calculate the solubility of Fe2+ and PO43- in a saturated solution.
- ST5G.2 - Estimate the solubility of CaF2(aq) [in units of PICOmolar] in the presence of 0.701 molar AIF3(aq). [This is a bit fictitious - I don't think aluminum fluoride is soluble, but I want you to think carefully about the fluoride concentration.] Type your answer..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?The concentration of calcium carbonate in a sample of water saturated with the solid was found to be 7.00 x 10-5 moldm-3 at 200C. What is the solubility product of calcium carbonate at this temperature?
- 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].Please explain how the relationship S = 0.330(Ksp)^(1/5) was derivedto calculate the solubility (S) of cerium(IV) ions in a saturated solution of cerium(IV) fluoride, CeF4.The solubility product constant of Hg2Cl2 is 2 × 10-18 at 25°C. Estimate the concentration of Hg22+ and Cl2 in equilibrium with solid Hg2Cl2 at 25°C.
- The bisulfate (or hydrogen sulfate) anion, HSO4 , is a weak acid. The equilibrium constant for the aqueous acid reaction HSO4 (ag) = H* (ag) + SO,2- (ag) is 1.2 x 10-2 (a) Calculate AG° for this equilibrium. Assume a tempera- ture of 25.0°C. (b) At low concentrations, activity coefficients are approxi- mately 1 and the activity of a dissolved solute equals its molality. Determine the equilibrium molalities of a 0.010-molal solution of sodium hydrogen sulfate.ST5G.2 - Estimate the solubility of CaF2(aq) [in units of MICROmolar] in the presence of 0.716 molar CaCl2(aq). Type your answer...19" 0.00014 m Na2 Coz are combined? Determine the solubility of Cul (s) (Ksp.= 1.1x1013 In 0.15m Cu₂ (03 (aq) Solution,