# Solubility of Ammonium Chloride

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...

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