(a) Papaverine hydrochloride is an alkaloid drug used as a muscle relaxant, particularly for acute myocardial infarctions and angina It is a weak acid. If a 0.205 M solution of papaverine hydrochloride has a pH of 3.31, what is its Ka?

The compound methylamine is a weak base like ammonia. A solution contains 5.89x10-2 M CH3NH3+ and 0.330 M methylamine, CH3NH2. The pH of this solution is

(A) Consider a solution of 1.34×10-3 M hydrochloric acid. What would be the hydrogen ion concentration of this solution? And the pH?

(a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH, 0.10MHF(aq) or 0.10MHC2H3O2(aq). Do not perform any numerical calculations. (b) Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2(aq) or a 0.010M solution of HC2H3O2(aq) ? Justify your answer including the calculation of percent ionization for each solution.

calculate the pH of a dilute solution that contains the molar ratio of sodium acetate to acetic acid ( pka 4.76) of 1:3

(a)  Calculate the pH of a 0.20 M solution of benzoic acid at 25°C.(b)  How many moles of acetic acid must be dissolved per liter of water to            obtain the same pH as that from part (a)?

Predict ionization of the following drug as a function of pH. See attached figures. Answers A - C A I BII C II

What is the pH of a 0.639 M solution of lactic acid? The pKa of lactic acid is 3.854.

The pH of an aqueous solution of 0.400 M hydrocyanic acid, (Ka (HCN) = 4.00 × 10-10) is

Find the pH of the following solutions:   0.03M trichloroacetic acid, Cl3CCO2H, pKa = 0.638