O-Exp 26 Class Data

	A	B	C	D	E	F	H	I	J
1	Experiment 26		Download and complete the spreadsheet by calculating all values in pink
2
3		mass of Na2S2O3 5H2O used to make 0.11 M solution	54.5764	grams	in 2.00 liters	to make a 0.11 M solution
4		Molarity of Na2S2O3 solution	6.770	M	This is an approximation of the concentration - The true value will be determined from the tiration of the thiosulfate solution with ferrocyanide solution.
5
6	PART I	Standardization of Thiosulfate: Complete and explain the following Calculations for your data and results.
7		Student's first name	Macaire
8		mass of K3Fe(CN)6 used (g)	0.6004g	0.6005g	0.6000g
9		volume of thiosulfate solution used (mL)	16.5 ml	17.2ml	17.2ml
10		Moles of K3Fe(CN)6 = Moles Fe(CN)6 3-
11		Moles of Na2S2O3 = moles S2O3 2-
12		Molarity of Na2S2O3 solution
13		average molarity
14		Standard deviation
15		percent error
16
17	Part II - Determining the concentration of a bleach solution
18		students in group
19	1	bleach used	Chlorox						Greater Value Bleach
20	2	Mass of 10 mL bleach aliquot (g)
21	3	volume of thiosulfate solution used in titration
22		Molarity of Na2S2O3 solution
23		moles of Na2S2O3 = moles of S2O3 2-
24		moles of OCl-
25		molarity of diluted bleach solution
26		molarity of concentrated bleach solution
27		moles of bleach (NaClO) in the 10 mL sample
28		mass of NaClO
29		percent mass of bleach solution
30		average % mass						average
31		standard deviation of % mass of bleach	0.1969
32		Reported % mass of A-1 Bleach	5.25%				Reported % mass of Chlorox Bleach		6.00%
33		Percent error	94.476						96.5
34
35
36
37
38
39
40
41
42
43
44
45
46
47
48
49
50
51
52
53
54
55
56
57
58
59
60
61
62
63
64
65
66
67
68
69
70
71
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
87
88
89
90
91
92
93
94
95
96
97
98
99
100