A solution was prepared from 80mL 0.1 M acetic acid and 20mL of 0.1 M sodium ace

Question

A solution was prepared from 80mL 0.1 M acetic acid and 20mL of 0.1 M sodium acetate. What is the expected pH of the solution?

-> I believe the equation to find pH is: pH=pKa + log([A-]/[HA]), but I unfortunately don't know how to apply this to the information I'm given.

-> How do you find pKa? (and if possible please use numbers from question being asked)

-> What do you use for [A-] and [HA]?

A step by step explanation for finding each part would be greatly appreciated. 5 stars guarranteed for a good step by step explanation and correct answer! Thank you!

Explanation / Answer

Since both the solutions are having same concentration i.e. 0.1 M, the volume ratio used in preparing the buffer is exactly the same as the mole ratio

CH?COOH + H?O ? CH?COO? + H?O?

Ka = [CH?COO?][H?O?]/[CH?COOH]

pKa = 4.75 =

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