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Understanding Solutions: Solute, Solvent, Concentration, and Dilutions in Chemistry

This guide explores the fundamental concepts of solutions in chemistry, including the definitions of solute, solvent, and solution. It explains how concentration is calculated using formulas like g/dm³ and mol/dm³. Through practical examples, you will learn how to determine the concentration of solutions, perform dilutions while conserving the number of moles of solute, and apply relevant equations such as C1V1 = C2V2. Ideal for students looking to solidify their understanding of solutions and their properties.

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Understanding Solutions: Solute, Solvent, Concentration, and Dilutions in Chemistry

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  1. Solutions (1.5) Year 11 DP Chemistry Rob Slider

  2. Solute: the substance that dissolves in another substance (solvent) to create a solution Solvent: the substance (usually a liquid) that dissolves another substance (solute) to form a solution Solution: the homogeneous mixture of one or more solutes in a solvent. Definitions

  3. Concentration: the amount of solute per volume of solution. Expressed as: g.dm-3 mol.dm-3 (M) If I have 25g of a substance in 500mL of solution, what is the concentration? Answer: 50 g.dm-3 Concentration What if I have 58.5 g of NaCl in 500mL? What is the concentration in mol.dm-3 or M? 2M

  4. C1 V1 = C2 V2 When diluting a solution, we change the concentration and the volume, but the number of moles of the solute (n) does not change (i.e. n = cv) Example: How much 10M HCl do we need to make up 1L of 2.5M HCl? Dilutions Notice that the # of moles (n) stays the same Answer: C1=10M, C2= 2.5M, V2=1000mL (10M)(V1) = (2.5M)(1000mL) V1 = 250mL

  5. How would you prepare 1dm3 of 2M NaCl? • Which is greater? • 1M hydrogen gas • 2 g.dm-3 hydrogen gas • I have a litre of 5M H2SO4 and I want to make up some 2M H2SO4. Explain how can this be done? Exercises

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