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- Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionThe pH of a 0.10-M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at equilibrium and found to be 2.93 at 25 °C. Calculate the Ka of propanoic acid.Calculate the pH and pOH of the following substances: 1. 0.3 M sulfuric acid (H2SO4) solution 2. 0.125 M potassium hydroxide (KOH) solution 3. 0.8 M hypochlorous acid (HCIO) solution (Ka = 2.9 x 10-8) 4. 0.5 M aniline (C6H5NH2) solution (Kb = 3.8 x 10-10)
- Hydrazoic acid, HN3, has an acid dissociation constant of 2.5 x 10-5. Calculate the equilibrium concentrations of all substances if the initial concentration of HN3 is 0.0750 M. Determine the pH of the solution. Would a 0.0750 M solution of HBr have a higher or lower pH than the 0.0750 M HN3 solution? Explain why.Perform the following to determine the pH of a lactic acid solution. Write the acid/base reaction between lactic acid, HC3H5O3 and water. Write an equilibrium expression for the reaction between lactic acid and water. If the Ka of lactic acid is 3.18 x 10-4, what is the pH of a 0.500 M solution of lactic acid?A solution containing 0.0138 M maleic acid and 0.0188 M disodium maleate. The K₁ values for maleic acid are 1.20 x 10-2 (Kal) and 5.37 x 10-7 (Ka2). pH = A solution containing 0.0384 M succinic acid and 0.022 M potassium hydrogen succinate. The Ka values for succinic acid are 6.21 x 10-5 (Kal) and 2.31 x 10-6 (Ka2). pH =
- Determine the hydroxide ion concentration and pH of 0.0942 M hypochlorous acid solution. Ka = 2.85 x 10-8The equilibrium constant for an acid is called the acid ionization constant (Ka). If acetic acid (weak acid, HC2H3O2) is placed into water, it ionizes to H+ and C2H3O2- with a Ka of 1.82 x 10-5. Determine the pH of the solution when 20.0 g HC2H3O2 (s) is added to water, with a final volume of 1000. mL?A solution contains 0.321 M potassium fluoride and 0.165 M hydrofluoric acid (K₁ = 7.20 × 10-¹). The pH of this solution is A solution contains 0.157 M potassium acetate and 0.167 M acetic acid (Ka = 1.80 × 10-5). The pH of this solution is A solution contains 0.485 M sodium acetate and 0.0779 M acetic acid (Ka = 1.80 × 10-5). The pH of this solution is
- Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80. 5.4 x 10-2 4.9 x 10-7 8.6 x 10-6 4.3 x 10-4Find the pH of a 0.337 M aqueous solution of hydrofluoric acid (HF), for which Ka = 6.8 × 10–4.Determine the pH of a solution of a weak acid (HA) that is 0.17 M. The Ka of the weak acid is 7.5 x 10-5
