Potassium chloride, also known as KCl or potassium salt, is a 1:1 mixture of potassium and chlorine ions in a metal halide salt. It looks like a white or colorless and odorless vitreous crystal.
The molecular weight of KCl is 74.555 g/mol−1, its density is 1.984 g/cm3, and it is soluble in water, highly soluble in alcohols, and insoluble in ether.
Requirements of glassware, chemicals, and apparatus:
Beaker, volumetric flask, glass rod, funnel, distilled water, AR/LR grade potassium chloride (KCl), spatula, etc.
How to prepare saturated solution of KCl
Using KCl and water, you can make a supersaturated solution by the following procedure:
- Take a 250 ml beaker; add 100 ml of distilled water to it, then add KCl and mix well to dissolve.
- Once it has completely dissolved, add more salt to the mixture and keep stirring.
- At a temperature of 20°C, it can be noticed that 35.00 g of potassium chloride can be completely dissolved, and the solution becomes saturated.
- If we increase the temperature, more amount of the solute will be able to dissolve in the solution.
- If we increase the temperature of the solution to 80 °C the excess solute separates out in the form of crystals.
What is the concentration of saturated KCl?
The temperature-dependent solubility of saturated KCl determines its concentration.
- KCl solubility at 20°C: 0,340 g.cm-3 in water = 340 g/l = 4.56 mol/l (Saturated KCl at 20°C)
- KCl solubility at 30°C: 0,374 g.cm-3 in water = 374 g/l = 5.02 mol/l (Saturated KCl at 30°C)
How to store saturated KCl solution?
The saturated and supersaturated KCl solutions must be kept at room temperature in a closed container. There is no need to be concerned about the growth of microorganisms in the solution as it has a very high osmotic pressure.
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