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Do all substances dissolve? - Coggle Diagram
Do all substances dissolve?
How to measure
Filter Paper Method
: This technique may be used to test solubility in a quantitative manner. The solution that consists of a solvent with dissolved solute will be filtered through filter paper. The remains sediment will then be carefully be weighed on a scale. The weight of the solute will determine the solubility of the mixture.
Visual Inspection
: The solubility of a solute in a solvent is evaluated through a visual process. The method can be carried out by simply stirring the solution with the solute added to the solvent. Through the detection of any remaining particles it can be determined as soluble or insoluable.
Solubility Test Strips:
Solubility test strips are accessible in certain stores and offers a quick and feasible manner to assess and evaluate. The method simply involves the coatings of the test strips to have a chemical reaction with the chosen solute to change colour. Then, the strip must be placed into the solvent to observe if the colour transforms. The solubility may be determined by the strength of the colour.
Chemistry behind solubility
The property of a substance that determines if the solute (the smallest component of the solution being dissolved) is dissolvable in a solvent(the larger component of the solution that dissolves solute) is defined as solubility. The molecules or ions of the solute interact with the molecules or ions of the solvent when a solute is added. The solute will dissolve in the solvent if the interactions between the two are strong enough.
Factors that the strength of the interaction between solute and solvent depend on:
(Potential DV)
Solute
Polarity
Polarity is a significant factor that must be taken into consideration when determining the solubility as non-polar solutes dissolve in polar solvents as they can interchange via weaker van der Waals forces. On the other hand, polar solutes dissolve in solvents as they have similar intermolecular forces and interact via dipole-dipole interactions.
- Size
The size of the solute/solvent molecules affects the solubility as solute ions that are too large to pass through between the solvent molecules may result in insolubility.
Solvent
Temperature
The fundamental rule for solutes dissolved in solvents is that the increase of temperature causes an increase in the solubility as the kinetic energy of the solvent molecules increases with temperature thus allowing the breaking of intermolecular interactions that keep the solute particles together easier. However, this rule has many exceptions as the solubility of gases and liquids decreases as temperature rises.
In the case of gases dissolved in liquids, the solubility decreases with increasing temperature. This occurs as when there is an increase in temperature. the kinetic energy of the gas molecules rise, allowing a more significant possibility to escape from the liquid phase and entering the gas phase.
Pressure
Pressure has a similar effect on the solubility of gases in liquids as the solubility increases as a result of increased pressure. When pressure is added more gas molecules transform into the liquid condition thus extending the interactions between solvent and gas molecules.
Control Variables
For consistent and reliable outcome the same amount of solvent and solute will be utlised in the experiment. When manipulating the amount it does not uphold a sense of uniformity.
.Throughout the experiment both the solvent and solute will be under room temperature. The experimenters will take control over temperature to isolate the effect of the IV on the DV
Each solution/mixture will receive the same amount of stirring to ensure that one doesn't get assisted further in dissolving than the rest.
Type of substances (Potential IV)
Solvents
Non-polar molecules
Hexane
(C6H14)
Benzene
(C6H6)
The evenly spread electronic density across the nonpolar molecule shapes it to serve as an excellent solvent for numerous organic molecules, suggesting no net dipole force.
Polar Molecules
Ethanol
(C2H5OH)
Acetone
(CH3COCH3)
Water
(H2O)
The polar H20 molecules guard around the positive and negatively charged sodium and chloride ions. This is prevalent in ionic compounds like NaCl, dissolving the ionic lattice structure.
Solutes
Non-polar molecules
Ethane
(C2H6)
Octane
(C8H18)
The weak intermolecular interactions and the lack of permanent dipoles cause non ploar molecules to dissolve rapidly in non polar solvents.
Polar molecules
- Water
(H20)
-Ammonia
(NH3)
Solubility is enhanced through network of hydrogen bonds between an electronegative atom from a solute that is attracted to a hydrogen atom derived from the solvent molecule.