Abuffer solution with a volume of 0.0255 l consists of 0.61 m hypochlorous acid (hclo), a weak acid, plus 0.61 m potassium hypochlorite (kclo). the acid dissociation constant of hypochlorous acid, ka, is 4.0 x 10^−8.
1. determine the ph of the buffer solution after the addition of 0.0039 mol rubidium hydroxide (rboh), a strong base. (assume no change in solution volume.)

7.62

Explanation:

According to the Henderson-Hasselbach equation, the pH value o a buffer can be calculated by the following equation:

Let's identify the variables:

Identify the moles of each component:

The strong base reacts with acid to produce more of the basic component:

Hydroxide is the limiting reactant. The new amounts of the weak acid and base are:

Let's use the molar amounts in the equation, as we have exactly same volume for each component in the buffer:

the answer for sodium is 0.186

the answer for rubidium is 0.251

i wish i could but this one is weird give me abc and i can solve it.