of a titration reaction of a

In the laboratory, a general chemistry student measured the pH of a 0.506 M aqueous solution of acetic acid to be 2.506. Use the information she obtained to determine the Ka for this acid. Ka(experiment)

In the laboratory, a general chemistry student measured the pH of a 0.558 M aqueous solution of formic acid, HCOOH to be 1.984. Use the information she obtained to determine the K, for this acid. K(experiment) =

Weak Acid + Strong Acid Base Titration - Example Problem: Consider Titration of 25 mL of .1 M CH3CO2H With .1 M NaOH. Calculate The pH After Adding The Following Volumes of NaOH: a. 0 mL b. 12.5 mL c. 25 mL d. 37.5 mL - I know that the correct the answer for letter d. is 12.28. I just don't know how to get to this answer.

Based on that experimental titration curve of the IU unknown sample, can you sketch out the titration curve if both the starting weak acid solution and the NaOH solution are diluted 10 times? What about diluting another 10 times on top of that? Particularly, you should pay attention to the size of the pH jumps around each equivalence point, as well as the relative positions of the flat regions before or after the pH jumps. For the sake of simplicity, no need to consider activity in this exercise.

A 28.1mL sample of 0.108 M HCI is titrated with 0.175 M NAOH. Calculate the pH after the addition of 36.8 mL of NaOH. Hint: Determine the equivalence point so you know where you are in the titration. Report your answer with two places past the decimal point. Type your answer..

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#4 Could you circle or make answer visible please.

In the laboratory, a general chemistry student measured the pH of a 0.446 M aqueous solution of hydrofluoric acid to be -0.253. Use the information she obtained to determine the K, for this acid. Ka(experiment)

Solve only D ...   Don't provide handwriting solutions....