To answer this question, refer to the titration curve shown above and the points labelled A-G.

Which of the following statements correctly describe the content of the solution being titrated at the different points during the titration?

Select all that apply. There is a penalty for each missed or incorrect selection.

Question 2 options:

	At point A, there are more H3O+ ions than any other species present in solution (apart from water).
	At point B, the solution in the beaker could be described as a buffer solution.
	At point C, the concentration of H3O+ ions in the solution is equal to the Kavalue of the acid being titration.
	At point D, there are equal amounts of A ions and HA molecules in solution.
	At point E, the concentration of H3O+ ions is the same as the concentration of OH ions.
	At points F and G, the number of A ions in solution is approximately the same.
	At points F and G, the concentration of A ions in solution is approximately the same.

Question 3 (2 points)

In Question 2, you analyzed a titration curve for a weak acid "HA-1".

Now, let's imagine what the titration curve of a different acid "HA-2" would look like.

Assume that this other acid has the same initial concentration as the "HA-1" solution but that it has a different K_a value:

K_{a HA-2} = 7.7 x 10^-7

Also assume that you start your titration experiment using the same volume of acid solution and using the same NaOH solution to titrate.

Determine whether the following values are expected to be larger, lower, or the same.

Question 3 options:

123	The pH value at point E
123	The volume of NaOH solution required to reach point E
123	The pH value at point C
123	The initial pH value for "HA-2" (point A)

1.	larger
2.	the same
3.	lower

> Apalyzing solutions using a titration experiment A weak acid HA-1 was titrated with 0.100 M NaOH to produce the graph below. 13 12 F G 11 10 9 E 8 00 Hd 7 6 CD B 5 4 3A 2 0 5 10 15 20 25 30 35 40 Volume 0.100 M NaOH added (mL) 1 day ago