Question

Bob Cat is attempting to determine the molarity of an unknown solution of acetic acid. He began by mixing an aqueous NaOH solution and standardizing it by titration of KHP with phenolphthalein indicator. He then titrated the acetic acid solution with his standardized NaOH. The data from one of Bob’s trials is below, but he still needs to complete his calculations. The molar mass of KHP is 204.2 g.

Titration of KHP		Titration of Acetic Acid
mass of KHP (g)	3.261	volume of acetic acid (mL)	27.89
initial buret reading (mL)	2.87	initial buret reading (mL)	1.43
final buret reading (mL)	42.35	final buret reading (mL)	35.62
volume NaOH (mL)	39.48	volume NaOH (mL)	34.19

What is the concentration of his acetic acid solution?

["3.031 M", "0.4623 M", "0.4045 M", "0.1013 M", "0.4959 M"]      

What is the concentration of his NaOH solution?

["0.3771 M", "0.4045 M", "0.08260 M", "4.045 x 10^-4 M", "3.771 x 10^-4 M"]      

What is the color of the solution before the addition of NaOH?

["light pink", "colorless", "dark pink"]      

What is the color of the solution at the endpoint?

["light pink", "colorless", "dark pink"]      

INFO IN BRACKETS ARE ANSWER CHOICES

Answer 1