State the limits to the generality of the expression for estimating the pH of an amphiprotic salt solution. Suggest reasons for why these limitations exist.
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State the limits to the generality of the expression for estimating the pH of an amphiprotic salt solution. Suggest reasons for why these limitations exist.
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- Sodium acetate, NaCH3CO2, of mass 7.4 g is used to prepare 250 cm3 of aqueous solution. What is the pH of the solution?Outline the change in composition of a solution of the salt of a triprotic acid as the pH is changed from 1 to 14.The solution of total volume 0.50 L was prepared by the addition of 0.10 moles of KF to sifficient water. What are the major species of the solution and pH ?
- Estimate the pH of a solution of 0.50 M HCI(aq), assuming ideal behaviour. The mean activity coefficient at this concentration is 0.769. Calculate a more reliable value of the pH .Describe the general features of the Debye-Huckel theory of electrolyte solutions. Which approximations limit its reliability to very low concentrations?Identify and justify the approximations made in the derivation of the van 't Hoff equation.
- The dissociation vapour pressure (the pressure of gaseous products in equilibrium with the solid reactant) of NH4CI at 427 °C is 608 kPa but at 459 °C it has risen to 1115 kPa. Calculate (a) the equilibrium constant. (b) the standard reaction Gibbs energy, (c) the standard enthalpy, (d) the standardentropy of dissociation, all at 427 °C. Assume that the vapour behaves as a perfect gas and that ΔHΘ and ΔSΘ are independent of temperature in the range given.Derive an effective Henry’s constant formula for ammonia (NH3) dissolved in waterOne of the most extensively studied reactions of industrial chemistry is the synthesis of ammonia, for its successful operation helps to govern the efficiency of the entire economy. The standard Gibbs energy of formation of NH3(g) is -16.5 kJ mol-1, at 298 K. What is the reaction Gibbs energywhen the partial pressure of the N2, H2, and NH3 (treated as perfect gases) are 3.0 bar, 1.0 bar, and 4.0 bar, respectively?What is the spontaneous direction of the reaction in this case?
- Calculate the solubility of calcite in water in contact with a soil atmosphere containing CO2 at the partial pressure of 0.1 bar, and find the pH of the saturated solutionDetermine the molar solubility of CaF2 in a 0.10 M CaCl2(aq) solution. Clearly identify any assumptions/approximations that you make.The standard reaction Gibbs energy for the reactionH2(g) + (1)/(2)O2(g) → H2O(I) is -237.13 kJ mol-1 at 25 °c. Determine the equilibrium constant in terms of concentration, Kc, at this temperature.