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With enough water molecules, a soluble ionic compound is completely dissolved into aqueous ions

With enough water molecules, a soluble ionic compound is completely dissolved into aqueous ions. “Like dissolves like” Ions become Hydrated Dissolution of compound Solute is written as aqueous ions Solvent is water Strong electrolytes, ionize completely Weak electrolytes,

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With enough water molecules, a soluble ionic compound is completely dissolved into aqueous ions

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  1. With enough water molecules, a soluble ionic compound is completely dissolved into aqueous ions • “Like dissolves like” • Ions become Hydrated • Dissolution of compound • Soluteis written as aqueous ions • Solventis water • Strong electrolytes, ionize completely • Weak electrolytes, • do not dissociate fully weak electricity. Non electrolytes - may dissolve, but do not form ions at all, such as sugar in water, or organic compounds in water.

  2. Ionic solids • (or salts) • composed of positive and negative ions, • held together by the strong force of attraction between particles with opposite charges. • ions are released water • solution conducts electricity • new association with the polar solvent molecules. • Why Do Some Solids Dissolve in Water? • sugar - molecular solid, • weak bonds between the individual sucrose molecules are broken, and released into solution. • the bonds within C12H22O11 molecules are not broken. • bonds with-in water molecules are not broken. • Energy is given off when the slightly polar sucrose molecules form intermolecular forces with the polar water molecules. • weak bonds that form between the solute and the solvent compensate for the energy needed to disrupt the structure of both the pure solute and the solvent. • Non-electrolyte because no ions are formed.

  3. Soluble compounds are written as Ions include the charge! Insoluble compounds are written as Molecules. • Soluble Compounds • All compounds containing alkali metal ions • compounds containing ammonium ion, NH4+ are soluble • compounds containing • NO3-, ClO4-, ClO3-, and C2H3O2- anions • chlorides, bromides, and iodides are soluble • - except with Ag+, Pb2+, or Hg22+. • sulfates are soluble • - except with Hg22+,Pb2+,Sr2+, Ca2+,Ba2+. • Insoluble Compounds • All hydroxides are insoluble • - except with alkali metals,Ca2+,Sr2+, and Ba2+ • All compounds containing PO43-, S2-, CO32-, and SO32- ions are insoluble • - except with alkali metals or NH4+.

  4. Composition of Solutions Molarity = moles of solute liters of solution moles Molarity liters grams Molar mass moles Dilutions; moles in beginning = moles at the end Molarityinitial x volumeinitial = Molarityfinal x volumefinal M1V1=M2V2

  5. Molarity Practice Problems • If 500.0 ml of a 1.00M KOH solution and 1500. ml of a 2.00M KOH solution are mixed, and the volume brought up to precisely 2500.0 ml by adding more water, what is the molarity of the final solution. • How many grams of KOH would 250.0 ml of this final solution contain? • When the 250.0 ml of solution above is added to 130.0 ml 2M HCl, how much salt is formed? What is the pH of the resulting solution?

  6. Solution Stoichiometry • A 0.350 g sample of solid Barium chloride is added to 125 mL of 0.0100 M Calcium sulfate solution. Assume no change in volume of the solution. • BaCl2(s) + CaSO4 (aq) BaSO4(s) + CaCl2(aq) • List an appropriate observation that provides evidence of a chemical reaction between the two compounds, write the net ionic equation. • Calculate the number of moles of each reactant. • Identify the limiting reactant. Show calculations to support your identification. • (d) Calculate the concentration of aqueous ions in the mixture after the reaction is complete.

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