Solubility of Ammonium Chloride
Objective
The objective of this laboratory is to calculate the solubility of a substance under a variety of temperatures and construct a solubility curve based on experimental data to see the effect of temperature on solubility.
Data collection and quantitative observation
VOLUME H2O/ml/±0.05
TEMPERATURE/°C/±0.1
5.00
71.3
6.00
59.3
7.00
52.4
8.00
47.2
9.00
41.8
Mass of NaCl: 3.0±0.05 g
Data Processing
To calculate the solubility, we need to use the formula:
Solving for x, the solubility of salt, we get the formula:
Where x is the solubility of salt in units of g/100 g water
Analysis and presentation
As we can see in the graphic according to the values given, solubility of NH4Cl increases with increasing temperature, because the dissolution of Nh4Cl is an endothermic process, which means that it will absorb heat. Also after we recorded each temperature at which crystallization of salt occurs, the start of this crystallization indicates that the solution has become statured. This means that at each temperature recorded the solution contains the maximum quantity of solute that can be dissolved in that amount of solvent.
Standard solubility table of Ammonium chloride
Solubility g/100gH2O
Temperature /°c/±0.1
60,3
71,3
55,5
59,3
51.3
52,4
47,7
47,2
43,4
41,8
Uncertainties and errors of volume and temperature
VOLUME H2O/ml/±0.05
Percentage uncertainty/%
Temperature/°c/±0.1
Percentage uncertainty/%
5.0
1.0
71.3
0.1
6.0
0.8
59.3
0.2
7.0
0.7
52.4
0.2
8.0
0.6
47.2
0.2
9.0
0.5
41.8
0.2
Process
To find the percentage uncertainty
A. Example for volume
B. Example for temperature
A. Example for solubility
Uncertainties and errors of solubility
Experimental solubility g/100gH2O
Theoretical Solubility g/100gH2O
Percentage uncertainty (experimental solubility)/%
Percentage error/%
60.0
61,0
1.6%
50.0
54,9
8.9%
42,9
The objective of this laboratory is to calculate the solubility of a substance under a variety of temperatures and construct a solubility curve based on experimental data to see the effect of temperature on solubility.
Data collection and quantitative observation
VOLUME H2O/ml/±0.05
TEMPERATURE/°C/±0.1
5.00
71.3
6.00
59.3
7.00
52.4
8.00
47.2
9.00
41.8
Mass of NaCl: 3.0±0.05 g
Data Processing
To calculate the solubility, we need to use the formula:
Solving for x, the solubility of salt, we get the formula:
Where x is the solubility of salt in units of g/100 g water
Analysis and presentation
As we can see in the graphic according to the values given, solubility of NH4Cl increases with increasing temperature, because the dissolution of Nh4Cl is an endothermic process, which means that it will absorb heat. Also after we recorded each temperature at which crystallization of salt occurs, the start of this crystallization indicates that the solution has become statured. This means that at each temperature recorded the solution contains the maximum quantity of solute that can be dissolved in that amount of solvent.
Standard solubility table of Ammonium chloride
Solubility g/100gH2O
Temperature /°c/±0.1
60,3
71,3
55,5
59,3
51.3
52,4
47,7
47,2
43,4
41,8
Uncertainties and errors of volume and temperature
VOLUME H2O/ml/±0.05
Percentage uncertainty/%
Temperature/°c/±0.1
Percentage uncertainty/%
5.0
1.0
71.3
0.1
6.0
0.8
59.3
0.2
7.0
0.7
52.4
0.2
8.0
0.6
47.2
0.2
9.0
0.5
41.8
0.2
Process
To find the percentage uncertainty
A. Example for volume
B. Example for temperature
A. Example for solubility
Uncertainties and errors of solubility
Experimental solubility g/100gH2O
Theoretical Solubility g/100gH2O
Percentage uncertainty (experimental solubility)/%
Percentage error/%
60.0
61,0
1.6%
50.0
54,9
8.9%
42,9