Quinine (c20h24n2o2) is the most important alkaloid derived from cinchona bark. it is used as an antimalarial drug. for quinine pkb1 = 5.1 and pkb2 = 9.7 (pkb = −log( only 1.0 g of quinine will dissolve in 1900.0 ml of water. calculate the ph of saturated aqueous solution of quinine. consider only the reaction q + h2o equilibrium reaction arrow qh + + oh? described by pkb1, where q = quinine.

The pH of saturated solution of the quinine is 10.05

Explanation:

Quinine (Q) is C20H24N2O2 has a molar mass of 324.4 g/mol

Q can behave as a weak base. Kb and pKb can be calculated for weak bases

pKb1 is to be considered when solving the question.

pKb1 = 5.1

Step 1 : Calculate the Kb of Quinine

            pKb1 = - log [kb]

                5.1  = - log [kb]

                take Antilog of both side

             [kb] = 7.94 x 10∧-6

Step 2: Calculate the concentration of saturated solution of Q in mol/dm3

           From the question, 1900 ml of solution contains 1 g of Q

           Therefore,  1000 ml of solution will contain........... x g of Q

           x = 1000 /1900

           x = 0.526 g in 1 dm3

In calculating concentration in mol/dm3,

Concentration in mol/dm3 = concentration in g /dm3 divided by molar mass

Molar mass of Q = 324.4

Concentration in mol/dm = 0.526 /324.4

                                         = 0.0016 mol/dm3

Step 3: Calculating the Concentration of OH-

            At Equilibrium, Kb = x² / 0.0016

            7.94 x 10∧-6 = x² / 0.0016

            x = √ 0.0016 × 7.94 x 10∧-6

            x = 1. 127 × 10∧-4 mol/dm3

The concentration of OH- = 1. 127 × 10∧-4 mol/dm

Step 4:  Calculating the pH of Quinine

           Recall, pOH = - log [OH-]

           pOH = - log [1. 127 × 10∧-4]

           pOH = 3.948

           Also recall that pH + pOH = 14

           pH = 14 - 3.948

           pH = 10.05

the ratio of the conjugate base to the acid required to attain the desired ph.