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Solutions

Solutions. IB Chemistry. A solution is a homogeneous mixture of 2 or more substances . It is made of a solvent and a solute. SOLUTE – the part of a solution that is being dissolved (usually the lesser amount)

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Solutions

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  1. Solutions IB Chemistry

  2. A solution is a homogeneous mixture of 2 or more substances . It is made of a solvent and a solute.

  3. SOLUTE – the part of a solution that is being dissolved (usually the lesser amount) • SOLVENT – the part of a solution that dissolves the solute (usually the greater amount) • Solute + Solvent = Solution

  4. moles solute ( M ) = Molarity liters of solution Concentration of Solution The amount of solute in a solution is given by its concentration. M = n/V mol dm-3

  5. Concentration • If something is concentrated it has more moles/grams of solute per amount of solvent. • Ex: 12 M HCl • If something is dilute it has less moles/grams of solute per amount of solvent Ex: 0.10 M HCl

  6. PROBLEM: Dissolve 5.00 g of NiCl2 in enough water to make 250 mL of solution. Calculate the Molarity. Step 1: Calculate moles of NiCl2•6H2O Step 2: Calculate Molarity

  7. PROBLEM: Dissolve 5.00 g of NiCl2 in enough water to make 250 mL of solution. Calculate the Molarity. Step 1: Calculate moles of NiCl2•6H2O Step 2: Calculate Molarity [NiCl2•6 H2O] = 0.0841 M

  8. What mass of oxalic acid, H2C2O4, is required to make 250. mL of a 0.0500 M solution?

  9. Dilutions M1 V1 = M2 V2 Where:M1 = concentration of the first solutionV1 = volume of the first solutionM2 = concentration of the second solutionV2 = volume of the second solution Examples: 1.Howmanymililitersof a solution of 4M KI are needed to prepare 400 mL of a 0.76 M ?

  10. 1.Howmanymililitersof a solution of 4M KI are needed to prepare 400 mL of a 0.76 M ?

  11. IB Note • Square brackets [0.60] means • 0.60 M or • 0.60 mol/L or • 0.60 mol dm-3 This is what IB uses!

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