Two related compounds, potassium chloride (KCI) and potassium chlorate (KCIO3) have precisely the same solubility of 57 grams per 100 g of water at 98oC. At lower temperatures, KCI is much more soluble in water than KCIO3.
Calculate the molarity of KCI at 98oC at its maximum solubility, assuming the density of water is 1.0 g mL -1.
When KCI dissolves in water, dissociation occurs. When HCI is added to water, ionisation occurs.
Explain the difference between ionisation and dissociation.
KCI is soluble in water because water molecules are able to keep both potassium ions and chloride ions in solution.
With the aid of a labelled diagram to show the interactions and bond type between the chloride ions and water molecules, explain how water molecules keep the chloride ions in solution.
Solutions of KCI conduct electricity because ions are free to move.
Outline the steps needed in a laboratory to determine the concentration of a solution of KCI using electrical conductivity.