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- Show the calculations to demonstrate that 2% AgNO3 is approximately 0.1M in Ag+ ions.The percent ionization of niacin 1Ka = 1.5 x 10-52 in a 0.020M solution is 2.7%. Calculate the percentage of niacin moleculesionized in a solution that is (a) 0.010 M, (b) 1.0 x 10-3 M.Calculate the value of Kc for a solution of 0.05 M HN3, if the equilibrium concentration of N3-= 5.0*10^-6
- Determine the pH of a 0.92 mol L–1 NaF solution at 25 °C. The Ka of HF is 3.5 × 10–5. 11.44 9.54 4.45 9.21 4.46Which salt below will produce the lowest [H 3O +] in an aqueous solution? 0.1170 M N2H5Br, Kb(N2H4) = 8.900e-7 0.1170 M CH3NH3Br, Kb(CH3NH2) = 0.0003700 0.1170 M CH3CH2CH2NH3Cl, Kb(CH3CH2CH2NH2) = 0.0005100 0.1170 M C6H5NH3Br, Kb(C6H5NH2) = 4.300e-10The pKa of Cl3CCO2H is 0.64. What is the pH of a 0.580 M solution? What percentage of the Cl3CCO2H is dissociated?
- Write both the charge balance equation (CBE) and mass balance equation (MBE) for the following solutions at equilibrium: 1. 0.12 M H2A 2. 0.40 M NH4ClCalculate the pH of a solution that contains 3.9 x 10-4 M H3O⁺ at 25°C. A) 4.59 B) 3.41 C) 10.59 D) 9.41 E) 0.59Determine the pH for a 0.267 M NaC3H5O3 solution at 25 C, the Ka for HC3H5O3 is 1.3 x 10^-5