Question

please see experiment information below

(a) According to your experimental data, what volume of C6H8O7 represents the half-equivalence (a.k.a. half-neutralization) point in this titration?

(b) What is the pH of the solution at the half-neutralization point?

Mass of Beaker (Step 1; g)	Mass of Beaker + Citric Acid (Step 3; g)	Mass of Citric Acid (Step 1 - Step 3; g)	Mass of Beaker + Citric Acid After Cooling (Step 7; g)	Molarity of Citric Acid Solution (M)
108.7	110.7	2.00	110.74	0.104M

Syringe reading (mL)	Citric Acid Added (mL)	pH TRIAL 1
30	0.0	11.8
29.5	.5	11.5
29	1	11
28.5	1.5	10.7
28	2	10.5
27.5	2.5	10.3
27	3	10
26.5	3.5	9.6
26	4	9.3
25	5	8.9
24	6	8.7
23	7	8.4
22	8	8.2
21	9	8.1
20	10	7.4
19	11	7.2
18	12	6.9
17	13	6.5
16	14	6.2
15	15	5.5

Syringe reading (mL)	Citric Acid Added (mL)	pH TRIAL 2
30	0.0	_11.6___ initial pH
29.5	.5	11.3
29	1	10.2
28.5	1.5	10
28	2	9.7
27.5	2.5	9.3
27	3	8.7
26	4	7.9
25.5	4.5	7.5
25	5.0	7.2
24.5	5.5	6.9
24	6.0	6.4
23.5	6.5	6.3
23	7	6.1
22.5	7.5	6
22	8.0	5.6
21	9.0	5.3
20	10.0	4.7
19	11	4.2
18	12	4
17	13	3.6
16	14	3.5
15	15	3.2

Answer 1

The equivalence point is defined as the point where the moles of strong acid added = initial moles of base B in solution. Graphically, the equivalence point is where the curve is most vertical.

Half way between start and equivalence point is the half equivalence point.

At half equivalence point , there is a sam amount of original acid and conjugate base.

From the graph given above we get,

(a), 2 mL of C₆H₈0₇ Represents the half equivalence.

(b)9.7 pH of the solution is required for half equivalence point.