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4 years ago

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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(Kb)). 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.

1 answer:

dolphi86 [110]4 years ago

8 0

Answer:

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

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