Concentration of Solutions
Chemistry ⇒ Solutions and Colloids
Concentration of Solutions starts at 9 and continues till grade 12.
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See sample questions for grade 11
A 0.5 M solution of KNO₃ is prepared by dissolving the salt in water. If the final volume is 2 L, how many moles of KNO₃ are present?
A chemist needs to prepare 250 mL of 0.1 M HCl from a 1 M stock solution. What volume of stock solution is required?
A laboratory technician adds 5 g of urea (molar mass = 60 g/mol) to 95 g of water. Calculate the mole fraction of urea in the solution.
A solution contains 0.2 mol of NaCl in 800 g of water. What is the molality of the solution?
A solution contains 20 g of glucose (C₆H₁₂O₆, molar mass = 180 g/mol) dissolved in 180 g of water. Calculate the molality of the solution.
A solution is labeled as 5% (w/v) NaCl. What does this mean?
A solution is prepared by dissolving 10 g of NaCl (molar mass = 58.5 g/mol) in enough water to make 500 mL of solution. What is the molarity of the solution?
Calculate the mole fraction of ethanol (C₂H₅OH, molar mass = 46 g/mol) in a solution containing 23 g of ethanol and 77 g of water (molar mass = 18 g/mol).
Define mole fraction and provide its formula.
Describe the difference between a concentrated and a dilute solution.
Explain why molality is preferred over molarity when studying colligative properties.
Explain why the concentration of a solution can be expressed in different units.
If 250 mL of a 2 M NaOH solution is diluted to 1 L, what is the new concentration?
