8) Hydrofluoric acid Use Ka and Kb values from the equation sheet provided CHEM_III_Eqn_Sheet How many grams of HF must be dissolved in water to create 788 mL of a solution with a pH of 2.47? Mass of HF 7.9e-4 g Incorrect. Hint: find the concentration of the hydrofluoric acid in solution, given the pH. Solving some of the previous problems may help.
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2. What is the percent ionization of hydrofluoric acid in (a) 0.20 M HF and (b) 0.020 M HF? Ka = 6.6 x 10^-4 a) Determine [H3O+] and [F-] in 0.500 M HF. Ka HF = 6.6 x 10^-4 b) Determine these concentrations in a solution that is 0.100 M HCl and 0.500 M HF. Ka HF = 6.6 x 10^-4 2. Calculate [H3O+] and [COOH-] in a solution that is 0.100 M HCOOH, formic acid, and 0.150 M NaCOOH. Ka HCOOH = 1.8 x 10^-4
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Arsenic acid H3AsO4 is a triprotic acid very similar to phosphoric acid. The acid dissociation constants for the three acidic protons are: Ka1 = 6.46 x 10^-3, Ka2 = 1.15 x 10^-7, and Ka3 = 3.16 x 10^-12. a) What ratio of conjugate base to acid is needed to make an arsenate buffer at pH 6.64? b) Which arsenate species serves as the acid and which serves as the base for the buffer at pH 6.64?
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