a buffer is made by mixing 0.1 moles of acetic acd a sodium acetate in 500 ml of solution. determine the pH of the buffer. (Ka for acetic acid - 1.8E-5)

Substitute into the Henderson-Hasselbalch equation and solve for pH. I think the answer ( I just did it in my head so be sure to confirm this) is 4.74.

To determine the pH of the buffer, we need to calculate the concentration of the acid (acetic acid) and its conjugate base (sodium acetate) in the buffer solution.

The number of moles of acetic acid (CH3COOH) present in the solution is given as 0.1 moles. The volume of the solution is 500 ml, which is equivalent to 0.5 liters.

First, we need to calculate the concentrations of acetic acid and sodium acetate in the buffer solution.

Concentration (C) is calculated using the formula:

C = moles / volume

The concentration of acetic acid (CH3COOH) is:

C(CH3COOH) = 0.1 moles / 0.5 L = 0.2 M

The concentration of sodium acetate (CH3COONa) will depend on the volume and concentration of the sodium acetate solution used to make the buffer. Please provide the concentration and volume of the sodium acetate solution to calculate its concentration in the buffer accurately.