Strong and Weak Acids Lab
Autor: Adnan • November 19, 2018 • 1,414 Words (6 Pages) • 527 Views
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x=1.34x10-3 = [H+]
pH =+] = -log[1.34x10-3] = 2.9[pic 8]
pH =2.9
Sample calculation for the Ph value for 0.1M HCl
pH = - log[H+]
pH = - log[0.1M]
pH = 1
Sample calculation for the % uncertainty of 0.1 Ethanoic acid (paper and meter)
% uncertainty = [pic 9]
Paper % uncertainty = [pic 10]
% uncertainty = 17%
Meter % uncertainty = [pic 11]
% uncertainty = 7%
Sample calculation for the % error of 0.1 Ethanoic acid (paper and meter)
% uncertainty = [pic 12]
Paper % error = [pic 13]
% error = 3%
Meter % error = [pic 14]
% error = 14%
Conductivity
Observations: In some solutions, the light bulb was brighter while in other solutions it was dim or not showing light at all.
Acid
Conductivity
Distilled water
No light
0.001M Hydrochloric acid
Very dim
0.01M Hydrochloric acid
Dim
0.1M Hydrochloric acid
Bright
1.0M Hydrochloric acid
Very bright
1.0M Ethanoic Acid
Dim
Action of Weak and Strong Acids on metals
Observations: In the CH3COOH the Magnesium solution was bubbling very rapidly; in the HCl solution it was bubbling, just not as much. The Zinc followed the same guidelines but overall in both solutions the bubbles were not as numerous. The copper was not bubbling with either solution
Metal
3M HCl
3M Acetic Acid
Copper
Slow
Slow
Zinc
Medium
Slow
Magnesium
Fast
Medium
Effect of Acid Concentration on Reaction Rate
Observations: in the solution with the higher molarity the magnesium was creating the most bubbles. In the solution with the smallest molarity there were close to no bubbles being produced.
Acid
Reaction Rate
0.01M Hydrochloric acid
Slow
0.1M Hydrochloric acid
Moderate
1.0M Hydrochloric acid
Fast
Titration
Observations: the solutions were very clear both the acid and the base solutions. After adding the phenolphthalein, the color of the acid solution did not change but every time the NaOH solution was added there would appear a pink color which then rapidly cleared up. Then near the end a few more drops of NaOH were added and the whole solution took on a light pink color.
HCl + NaOH = H2O + NaCl
CH3COOH + NaOH = CH3COONa + H2O
Acids
Volume of acid
(mL±0.02mL)
0.100M NaOH (mL±0.02ml)
Theoretical Volume needed of NaOH (mL)
Initial volume
Final Volume
Total Volume
Average Volume
0.2M HCL
10.0
20.0
2.00
24.00
22.0
23.50
0.2M HCl
10.0
20.0
0.00
25.00
25.00
0.2M CH3COOH
10.0
20.0
0.00
23.00
23.00
25.00
0.2M CH3COOH
10.0
20.0
0.00
27.00
27.00
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Sample Calculation for Theoretical volume
HCl + NaOH H2O + NaCl[pic 15]
10.00mL 0.1M
0.2M
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