Preparation of Solutions
Chemistry ⇒ Solutions and Colloids
Preparation of Solutions starts at 9 and continues till grade 12.
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See sample questions for grade 10
A laboratory technician needs to prepare 1 L of 0.2 M NaOH solution. What mass of NaOH (molar mass = 40 g/mol) is required?
A student dissolves 10 g of glucose (C6H12O6, molar mass = 180 g/mol) in enough water to make 200 mL of solution. What is the molarity of the solution?
A student needs to prepare 500 mL of 0.05 M HCl from a 1 M stock solution. What volume of the stock solution is required?
A student prepares a solution by adding 2 g of NaOH to 100 mL of water. What is the molarity of the solution? (Molar mass of NaOH = 40 g/mol)
A student prepares a solution by dissolving 5 g of KCl (molar mass = 74.5 g/mol) in 250 mL of water. Calculate the molarity of the solution.
A student wants to prepare 100 mL of 0.5 M H2SO4 from a 2 M stock solution. What volume of the stock solution should be used?
Describe the difference between a stock solution and a working solution.
Describe why it is important to transfer all of the dissolved solute into the volumetric flask when preparing a solution.
Explain the steps involved in preparing a 1 M solution of potassium nitrate (KNO3) in 500 mL of water.
Explain why solutions should be mixed thoroughly after preparation.
Explain why the final volume of a solution should be made up after the solute has completely dissolved.
A chemist needs to prepare 250 mL of 0.1 M AgNO3 solution. Calculate the mass of AgNO3 (molar mass = 170 g/mol) required for this preparation.
A laboratory technician needs to prepare 1 L of 0.5 M K2SO4 solution. Calculate the mass of K2SO4 (molar mass = 174 g/mol) required.
A student is given a 2 M stock solution of H2SO4 and is asked to prepare 100 mL of 0.25 M H2SO4. Calculate the volume of the stock solution needed and describe the steps to prepare the diluted solution.
Describe the potential errors that can occur if the temperature of the solution is significantly different from the calibration temperature of the volumetric flask during preparation.
Explain why it is important to use a volumetric flask rather than a measuring cylinder when preparing a standard solution of a precise concentration.
