Title | Lab 1 - Answers to the Lab |
---|---|
Course | Introductory Analytical Chemistry I |
Institution | Concordia University |
Pages | 2 |
File Size | 64.8 KB |
File Type | |
Total Downloads | 8 |
Total Views | 138 |
The first analytical chemistry lab is tricky, I found it helpful to go over other's calculations and work to understand the theory ...
1) Volume of H2O Delivered by Pipet (6 sig figs): T °=25 ℃ ± 0.5 ℃
ρH2O = 0.9972995g/ml Samples
Mass of Water (3 values selected by TA) 10.0096g 10.0041g 10.0055g 10.0064g
1 2 3 Average
10.0096 g+10.0041 g+10.0055 g X´ = =10.0064 g 3
Volume of pipet =
m of water 10.0064 g = =10.0335 ml ρ of water 0.9972995 g/ml
2) Density of unknown solution (4 sig figs):
Samples 1 2 3 Average
Mass of Unknown Densities Solution 10.8800g 1.0844g/ml 10.8732g 1.0837g/ml 10.8889g 1.0853g/ml --1.0857g/ml
ρUnk =
m Solution V solution
ρUnk =
10.8800 g =1.0844 g/ml 10.0335ml
1
2 ρUnk =
10.8732 g =1.0837 g/ml 10.0335ml
ρUnk =
10.8889 g =1.0853 g /ml 10.0335ml
3
1.0844 g /ml +1.0837 g /ml+1.0853 g/ml X´ = =1.0857 g 3
√
SD=
(1.0844−1.0857)2 +(1.0837−1.0857 )2 +( 1.0853−1.0857 )2 =0.008 g /ml 3−1
Deviation from Average: g 1) 1.0857−1.0844 =1.3E-3 ml g 2) 1.0857−1.0837 =2.0E-3 ml g 3) 1.0857−1.0853 =0.4E-3
ml
Average Of Deviation: 1.3E-3 + 2.0E-3 + 0.4E-3 =1.2E-3 g/ml 3
Precision in PPT: 1.2E-3 g /ml ∗1000=1.1053 1.0857 g /ml...