You need to produce a buffer solution that has a ph of 5.39. you already have a solution that contains 10. mmol (millimoles) of acetic acid. how many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution?

Milli moles of acetate = 43.65 mmol

Explanation:

The pH of a buffer solution is calculated using Henderson Hassalbalch's equation, which is:

Where

[Salt] = concentration of salt (sodium acetate, the conjugate base)

[acid] = concentration of acid (acetic acid) = 10 mmol

pH = 5.39

For acetic acid

pKa =4.75

Putting values

Taking antilog

moles of acetate = 43.65 mmol

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

nacl is added to the aqueous of what? ? in order to get a proper answer you have to specify the exact composition of the aqueous solution.