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Calculate the equilibrium constant for the reaction
2Fe3++H3AsO3+H2O=2Fe2++H3AsO4+2H+
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- You are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization just like water on Earth. Y2O + Y2O ⇌ Y3O+ + OY– Through a series of experiments, you determine the equilibrium constant (Keq) for this autoionization reaction at various temperatures. The value of Keq at 28.7ºC is 7.6 x 10-14. What is the pY of the pure substance at this temperature? Report your answer to the hundreths placeIf the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility = mol/LExplain why colour of KMnO4 disappears when oxalic acid is added to its solution in acidic medium.
- The dissociation vapor pressure of a salt A2B(s) ⇌ A2(g) + B(g) at 367°C is 208 kPa but at 477°C it has risen to 547 kPa. For the dissociation reaction of A2B(s), calculate (i) the equilibrium constant, (ii) the standard reaction Gibbs energy, (iii) the standard enthalpy, and (iv) the standard entropy of dissociation, all at 422°C. Assume that the vapor behaves as a perfect gas and that ΔrH° and ΔrS° are independent of temperature in the range given.Calculate the pH of: A 0.0850 molar solution of the intermediate (HA) form of threonine. It is a polyprotic question.The chemical formula for the oxalate ion is C2O42-. A liter of a saturated solution of calcium oxalate at 25 oC was evaporated to dryness, giving 0.0061 g of solid CaC2O4 residue. Calculate the solubility product constant for CaC2O4 at 25 oC.
- Calculate the equilibrium constant, Kc, of the reaction: HCO3-(aq) + HCO3-(aq) ↔ H2CO3(aq) + CO32- , Kc = ? Based on your result, do you expect this reaction to occur in the left-to-right direction?What is the difference between alkalinity and buffering capacity?50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?