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 12
A chemist needs to prepare 1 L of 0.05 M HCl from a 1 M stock solution. What volume of stock solution is required?
A chemist needs to prepare 250 mL of 0.1 M AgNO3 solution. Calculate the mass of AgNO3 required. (Molar mass = 170 g/mol)
A laboratory technician needs to prepare 250 mL of 0.2 M NaOH solution. Calculate the mass of NaOH required. (Molar mass of NaOH = 40 g/mol)
A solution is prepared by dissolving 5 g of glucose (C6H12O6, molar mass = 180 g/mol) in enough water to make 100 mL of solution. Calculate its molarity.
A student accidentally uses 100 mL of water instead of 250 mL to dissolve a solute for a 0.1 M solution. What will be the effect on the concentration?
A student needs to prepare 100 mL of 0.5 M H2SO4 from concentrated H2SO4 (18 M). Calculate the volume of concentrated acid required.
A student prepares a solution by dissolving 2.5 g of NaCl in 200 mL of water. What is the molarity of the solution? (Molar mass of NaCl = 58.5 g/mol)
Describe the difference between a stock solution and a working solution.
Describe the importance of using a clean and dry volumetric flask in solution preparation.
Describe the precautions to be taken while preparing a solution from a hygroscopic solute.
Describe the procedure for preparing 500 mL of 0.2 M KNO3 solution from solid KNO3.
Explain why distilled water is preferred over tap water in the preparation of solutions.
Explain why it is important to cool a solution to room temperature before making up to the mark in a volumetric flask.
Explain why it is important to label solutions with concentration, date, and name of the preparer.
Explain why some solutions are prepared by dilution rather than direct weighing of solute.
