A litre of buffer solution contains 0 . 1 mole of each of NH 3 and NH 4 Cl . On the addition of 0 . 02 mole of HCl by dissolving gaseous HCl , the pH of the solution is found to be _ _ _ _ _ × 10 - 3 (Nearest integer) Given: pK b NH 3

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A litre of buffer solution contains 0 . 1 mole of each of NH 3 and NH 4 Cl . On the addition of 0 . 02 mole of HCl by dissolving gaseous HCl , the pH of the solution is found to be _ _ _ _ _ &#215; 10 - 3 (Nearest integer) Given: pK b NH 3 = 4 . 745 log 2 = 0 . 301 log 3 = 0 . 477 T = 298 K ]

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In resultant solution after addition of HCl to the basic buffer: n NH 3 = 0 . 1 - 0 . 02 = 0 . 08 n NH 4 Cl = n NH 4 + = 0 . 1 + 0 . 02 = 0 . 12 Using Henderson-Hasselbach equation: pOH = pK b + log NH 4 + NH 3 = 4 . 745 + log 0 . 12 0 . 08 = 4 . 745 + log 3 2 = 4 . 745 + 0 . 477 - 0 . 301 pOH = 4 . 921 We know, pH = 14 - pH = 9 . 079

A litre of buffer solution contains 0 . 1 mole of each of NH 3 and NH 4 Cl . On the addition of 0 . 02 mole of HCl by dissolving gaseous HCl , the pH of the solution is found to be _ _ _ _ _ × 10 - 3 (Nearest integer) Given: pK b NH 3 = 4 . 745 log 2 = 0 . 301 log 3 = 0 . 477 T = 298 K ]

Correct answer

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More from Ionic Equilibrium

A litre of buffer solution contains 0 . 1 mole of each of NH 3 and NH 4 Cl . On the addition of 0 . 02 mole of HCl by dissolving gaseous HCl , the pH of the solution is found to be _ _ _ _ _ &#215; 10 - 3 (Nearest integer) Given: pK b NH 3 = 4 . 745 log 2 = 0 . 301 log 3 = 0 . 477 T = 298 K ]

Correct answer

Step-by-step solution

More from Ionic Equilibrium

A litre of buffer solution contains 0 . 1 mole of each of NH 3 and NH 4 Cl . On the addition of 0 . 02 mole of HCl by dissolving gaseous HCl , the pH of the solution is found to be _ _ _ _ _ × 10 - 3 (Nearest integer) Given: pK b NH 3 = 4 . 745 log 2 = 0 . 301 log 3 = 0 . 477 T = 298 K ]