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3.6 Solubility

3.6 Solubility. Solution: homogeneous mixture or mixture in which components are uniformly intermingled Solute: substance that is being dissolved in solvent Solvent: substance that dissolves solvent and present in a large amount Aqueous solutions: solutions with water as the solvent.

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3.6 Solubility

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  1. 3.6 Solubility • Solution: homogeneous mixture or mixture in which components are uniformly intermingled • Solute: substance that is being dissolved in solvent • Solvent: substance that dissolves solvent and present in a large amount • Aqueous solutions: solutions with water as the solvent

  2. Solubility • Saturated: A solution in which the maximum amount of solvent has been dissolved. Any more solute added will sit as crystals on the bottom of the container • Unsaturated: A solution in which more of solute can be dissolved • Concentrated: a relative large amount of solute is being dissolved in solvent • Diluted: a relative small amount of solute is being dissolved in solvent

  3. Solution_Molarity • Molarity: the number moles of solute per volume of solution in liters moles of solute • Molarity = ------------------------ Liters of solution • unit = mol/L or M (molar) • Standard solution: is a solution whose concentration is accurately known.

  4. Example • What is the molarity of solution made by dissolving 2.355g of H2SO4 in water and dilutin to a final volume of 50.0mL • Calculate the molarity of a solution prepared by dissolving 11.5 g of solid NaOH in enough water to make 1.50 L of solution

  5. Calculating volume and mass • Determine how much volume (in ml) will be needed to dissolved 2.50 g of solid NaCl to make 0.050M solution. • How many grams of solute would you use to prepare 1.50L of 0.250 M glucose (C6H12O6)

  6. 3.8 Dilution • Reducing the original concentration of a chemical solution • A process of transferring solution to achieve a the desired molarity by diluting with solvent • Moles of solute after dilution = moles of solute before dilution • Formula  M1 V1 = M2 V2

  7. Example • What volume of 16 M sulfuric acid must be used to prepare 1.5L of 0.10 M of H2SO4 solution? • What is the final concentration if 75.0 mL of a 3.50M glucose solution is dilute to a volume of 400.0mL? • Calculate the new molarity if a dilution is made for: • 25.0 ml of water is added to 10.0 mL of 0.251 M CaCl2

  8. Examples • Stomach acid, a dilute solution of HCl in water, can be neutralized by reaction with sodium hydrogen carbonate, NaHCO3 NaHCO3, according to the equation HCl(aq) + NaHCO3(aq)  NaCl(aq) + H2O(l) + CO2(g) How many milliliters of 0.125M NaHCO3 solution are needed to neutralized with 18.0mL of 0.100M HCl?

  9. Examples • A 25.0mL sample of oxalic acid is titrated and found to react with 94.7 mL of 0.200M NaOH. What is the molarity of the oxalic acid solution? The reaction is 2NaOH(aq) + H2C2O4(aq)  C2O4Na2(aq) + 2H2O(l)

  10. Calculating the mass • When aqueous solutions of Na2SO4 and Pb(NO3)2 are mixed, PbSO4 precipitates. Calculate the mass of PbSO4 formed when 1.25 L of 0.0500 M Pb(NO3)2 and 2.00 L of 0.0250 M Na2SO4 are mixed Na2SO4(aq) + Pb(NO3)2(aq)  PbSO4(s) + 2NaNO3(aq)

  11. Example • What volume of 0.101 M HNO3 is required to neutralize with 24.9 ml of 0.00491 M Ba(OH)2(aq)?

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