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SOLUTIONS

SOLUTIONS. A homogeneous mixture in which the components are uniformly intermingled. Terms. Solvent – The substance present in the largest amount in a solution. The substance that does the dissolving. Solute – The other substance or substances in a solution.

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SOLUTIONS

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  1. SOLUTIONS A homogeneous mixture in which the components are uniformly intermingled

  2. Terms Solvent – The substance present in the largest amount in a solution. The substance that does the dissolving. Solute – The other substance or substances in a solution. The substance that is dissolved.

  3. ELECTROLYTES • Substances that break up in water to produce ions. • These ions can conduct electric current • Examples: Acids, Bases and Salts (ionic compounds)

  4. SOLUBILITY • Is the amount of a substance that dissolves in 100 g of water at a given temperature to produce a saturated solution • “Like dissolves Like” • Polar molecules dissolve polar molecules • Nonpolar molecules dissolve nonpolar molecules

  5. SOLUBILITY RULES • All common salts of Group I elements and ammonium are soluble • All common acetates and nitrates are soluble • All binary compounds of Group 7 (other than F) with metals are soluble except those of silver, mercury I and lead • All sulfates are soluble except those of barium, strontium, calcium, silver, mercury I and lead • Except for those in Rule 1, carbonates, hydroxides, oxides, sulfides and phosphates are insoluble

  6. Terms • Saturated • When a solution contains the maximum amount of solute • Unsaturated • When a solvent can dissolve more solute • Supersaturated • When the solution contains more solute than a saturated solution will hold at that temperature • Concentrated • When a relatively large amount of solute is dissolved • Dilute • When a relatively small amount of solute is dissolved

  7. Factors Affecting the Rate of Dissolution • Surface Area • Stirring • Temperature

  8. Temperature vs Solubility

  9. MOLARITY • Molarity-the number of moles of solute per liters of solution • M = molarity = moles of solute liter of solution

  10. Calculate the molarity of a solution prepared by dissolving 11.5 g of NaOH in enough water to make a 1.50 L solution.

  11. Calculate the molarity of a solution prepared by dissolving 1.56 g of HCl into enough water to make 26.8 ml of solution.

  12. DILUTIONS • M1 x V1 = M2 x V2 • What volume of 16 M sulfuric acid must be used to prepare 1.5 L of a 0.10 M H2SO4 • What volume of 12 M HCl must be used to prepare 0.75 L of a 0.25 M HCl?

  13. MASS PERCENT • A unit of concentration equal to the mass of solute per mass of solution part x 100 whole

  14. A solution is prepared by mixing 1.00 g of ethanol with 100.0 g of water. Calculate the mass percent of ethanol in this solution. • A 135 g sample of seawater is evaporated to dryness, leaving 4.73 g of salt. Calculate the mass percent of salt in the saltwater.

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