What is the pH of a solution consisting of 0.584M HF acid and 0.425NaF. The K a of HF is K a =6.6x10 −4 .

Write the reaction and the corresponding Kb equilibrium expression for each of the following substances acting as bases in water. a. NH3 b. C5H5N

Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?

Consider 0.10 M solutions of the following compound: AlCl3, NaCN, KOH, CsClO4, and NaF. Place these solutions in order of increasing pH.

Ethanol (ethyl alcohol), CH3CH2OH, can act as a BrnstedLowry acid. Write the chemical equation for the reaction of ethanol as an acid with hydroxide ion, OH. Ethanol can also react as a BrnstedLowry base. Write the chemical equation for the reaction of ethanol as a base with hydronium ion, H3O+. Explain how you arrived at these chemical equations. Both of these reactions can also be considered Lewis acid base reactions. Explain this.

Lactic acid, C3H6O3, occurs in sour milk as a result of the metabolism of certain bacteria. Calculate the pH of a solution of 56. mg lactic acid in 250. mL water. Ka for D-lactic acid is 1.5 × 10−4.

Write the chemical equation for the ionization of caffeine, a weak base. The chemical formula of caffeine is C8H10N4O2.

Write the acid ionization constant expression for the ionization of each of the following monoprotic acids. a. HF (hydrofluoric acid) b. HC2H3O2 (acetic acid)

Arrange the following 0.10 M aqueous solutions in order of increasing pH: HF, NaF, HNO3, and NaNO3.

What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.