|Temperature (°C) | |Mass of solute in 5ml (g) |Mass of solute in 100ml (g) | |1st set of data |2nd set of data |Average | | | |23.5 |24.0 |23.8 |4.5 |90.0 | |31.0 |29.0 |30.0 |5.0 |100.0 | |42.0 |40.0 |41.0 |5.5 |110.0 | |44.0 |55.0 |49.5 |6.0 |120.0 | |69.0 |71.0 |70.0 |6.5 |130.0 |
(On the sheet attached)
According to the solubility curve we plotted, solubility is proportional to temperature because the temperature of the solvent at which all of the solute was able to dissolve increased with the mass of the solute. This can be explained by the fact that increased temperature means a grater average velocity of the particles, which helps them to change their state more easily, in this case from solid to liquid.
There are several things we could have done better in our experiment to obtain more accurate results. One of the potential errors was the part of our experiment during which we looked for the first signs of crystallization because we often missed the first signs due to the crystals...