13. The molar conductivity of 0.0300 M HF (aq) is 4.10 mS m² mol¹. Determine the acidity constant, Ka, of the acid. a) 8.87×10- b) 3.40x10+ c) 1.05x10+ d) 1.10×105
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- If the cell constants of 0.2 cm^-1 and the molar conductivity of H+ and Cl- are known, 350 S.cm^2.mol^-1 and 76 S.cm^2.mol^-1, respectively, calculate the electrical conductivity of a 0.01 M HCl solution !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 ?The table below provides data for the enthalpy and entropy of formation of compounds A and B at standard conditions (298 K) Compound DHfo (kJ mol-1) Sfo(J K-1mol-1) A –135.2 189.2 B –157.6 192.1 i) Calculate the standard Gibbs energy of formation for A and B. ii) Calculate the Gibbs energy change for the reaction A - B at standard conditions. iii) Calculate the enthalpy change for the reaction A - B at 350 K if the average heat capacity C0p = 42 J.K-1.mol-1.
- The molar conductivity of a 0.05 M solution of a weak base (B) is 4.9 x 10-1 mSm2/mol and the sum of the limiting ionic conductivities for BH+ and OH‑ is 23.7 mSm2/mol. What is the value of the base constant Kb?If the specific conductance of a 0.02N acetic acid is 105.3 at 25oC, what is the ionization constant if the molar conductivity is 325.0?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 .
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