Buffer Solutions

Step 1: Understand the equilibrium involved.
In the Bowler's solution, we have a base (B $%5E-$ ) and its conjugate acid (HB) in equal concentration. This forms a buffer solution. The pH of a buffer solution formed by a weak base and its conjugate acid is given by: $%5Ctext%7BpOH%7D%20%3D%20%5Ctext%7Bp%7DK_%5Ctext%7Bb%7D%20%2B%20%5Clog%20%5Cleft(%20%5Cfrac%7B%5B%5Ctext%7BHB%7D%5D%7D%7B%5B%5Ctext%7BB%7D%5E-%5D%7D%20%5Cright)$ Step 2: Use given values.
Since the concentrations of B $%5E-$ and HB are equal, $%5Clog%20%5Cleft(%20%5Cfrac%7B%5B%5Ctext%7BHB%7D%5D%7D%7B%5B%5Ctext%7BB%7D%5E-%5D%7D%20%5Cright)%20%3D%20%5Clog(1)%20%3D%200$ So, $%5Ctext%7BpOH%7D%20%3D%20%5Ctext%7Bp%7DK_%5Ctext%7Bb%7D$ We are given: $%5Cfrac%7BK_%5Ctext%7BB%7D%7D%7B%5B%5Ctext%7BB%7D%5E-%5D%7D%20%3D%2010%5E%7B-10%7D%20%5CRightarrow%20K_%5Ctext%7BB%7D%20%3D%2010%5E%7B-10%7D%20%5Ctimes%20%5B%5Ctext%7BB%7D%5E-%5D$ Since $%5BB%5E-%5D$ cancels out in the ratio when $%5BB%5E-%5D%20%3D%20%5BHB%5D$ , we simply interpret: $K_b%20%3D%2010%5E%7B-10%7D%20%5CRightarrow%20%5Ctext%7Bp%7DK_b%20%3D%2010$ $%5Ctext%7BpOH%7D%20%3D%2010%20%5CRightarrow%20%5Ctext%7BpH%7D%20%3D%2014%20-%20%5Ctext%7BpOH%7D%20%3D%2014%20-%2010%20%3D%204$

High-Yield Trend

Chapter Questions
1 MCQs

Official Solution

Buffer Solutions

High-Yield Trend

Chapter Questions 1 MCQs

Official Solution

Chapter Questions
1 MCQs