1.3 - Concentration of Solutions (Molarity, ppm)
Enroll to start learning
You’ve not yet enrolled in this course. Please enroll for free to listen to audio lessons, classroom podcasts and take practice test.
Practice Questions
Test your understanding with targeted questions
What is the molarity of a solution with 2 moles of solute in 1 dm³ of solution?
💡 Hint: Use the formula M = n/V.
How many grams of NaCl are needed to prepare 1 liter of a 1 M solution?
💡 Hint: Remember the relationship of moles and grams.
4 more questions available
Interactive Quizzes
Quick quizzes to reinforce your learning
What is molarity defined as?
💡 Hint: Recall the definition given earlier.
Dilution affects the concentration of a solution.
💡 Hint: Consider how adding more solvent changes concentration.
2 more questions available
Challenge Problems
Push your limits with advanced challenges
You have a 0.25 M NaOH solution. How many grams of NaOH do you need to prepare 3 L?
💡 Hint: Find moles first: 0.25 moles x 3 L = 0.75 moles. Convert using molar mass: 0.75 moles x 40 g/mol.
Calculate the concentration in ppm if 2 mg of a pollutant is found in 100 L of water.
💡 Hint: Apply the conversion: 2 mg / 100L = (2 mg / 0.1 kg) x 1,000,000.
Get performance evaluation
Reference links
Supplementary resources to enhance your learning experience.