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 solution is labeled as 5% (w/v) NaCl. What does this mean?
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.
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?
Which of the following concentration units is temperature dependent? (1) Molarity (2) Molality (3) Mole fraction (4) Mass percent
Which of the following expresses concentration as a ratio of mass of solute to mass of solution? (1) Molarity (2) Molality (3) Mass percent (4) Mole fraction
Which of the following is NOT a colligative property? (1) Boiling point elevation (2) Freezing point depression (3) Molarity (4) Osmotic pressure
Which of the following is NOT a way to express the concentration of a solution? (1) Molarity (2) Density (3) Molality (4) Mass percent
Fill in the blank: A solution with a concentration of 1 ppm contains 1 part solute per __________ parts solution.
Fill in the blank: The concentration of a solution expressed as moles of solute per kilogram of solvent is called __________.
Fill in the blank: The formula to calculate molarity is M = __________.
Fill in the blank: The process of adding more solvent to a solution to decrease its concentration is called __________.
True or False: A 1 molal solution contains 1 mole of solute in 1 liter of solution.
True or False: Parts per million (ppm) is commonly used to express very low concentrations.
True or False: The mass percent of a solution is calculated as (mass of solute / mass of solution) × 100%.
True or False: The mole fraction of all components in a solution always adds up to 1.
