Question

Question deleted.

Answer 1

They're telling you that there are 6 grams of acetic acid in every liter. So find the molarity of the solution, then use the Ka of the acid (you have to look this up) to find \([H^+]\), and consequently the pH.

Answer 2

oh okay. thank you very much!

Answer 3

no problem

Answer 4

@aaronq would you know what how to calculate the expected range of 0.1M sodium hydroxide needed to neutralize the vinegar (from above)?

Answer 5

expected range of volume***

Answer 6

Dont know how you can get a range, but you can find the pH value that corresponds to the molarity using the Ka.

Answer 7

yup, i did that and I got pH of 2.38.
but now i have to find the expected volume of 0.1M sodium hydroxide needed to neutralize vinegar and i am confused..

Answer 8

you would need an equivalent number of moles of base. If it's the same concentration, 0.1 M, just add a liter. If not use:

\(M_1V_1=M_2V_2\)

Answer 9

oh, i think i understand now! thank you again :)