Solutions. 15.1 Solubility Solution: homogeneous mixture or mixture in which components are...
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Solutions
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15.1 SolubilitySolution: 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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Table 15.1 – Various Types of Solutions
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15.2 Solution Composition: An IntroductionSaturated: 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
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15.3 Solution Composition: Mass Percent
mass of soluteMass percent (m/m%) = ------------------------
x 100 mass of solution
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ExamplesA solution is prepared by mixing 1.00 g of
ethanol, C2H5OH, with 100.0 g 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 solid residue (the salts formerly dissolved in the seawater). Calculate the mass percent of solute present in the original seawater
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Example: Determine Mass of SoluteAlthough milk is not a true solution (it is
really a suspension of tiny globules of fat, protein, and other substrates in water), it does contain a dissolved sugar called lactose. Cow’s milk typically contains 4.5 % by mass of lactose, C12H22O11. Calculate the mass of lactose present in 175 g of milk
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15.4 Solution CompositionMolarity: the number moles of solute per
volume of solution in litersmoles of solute
Molarity = ------------------------Liters of solution
unit = moles/L or M (molar)
Standard solution: is a solution whose concentration is accurately known.
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ExamplesCalculate the molarity of a solution prepared
by dissolving 11.5 g of solid NaOH in enough water to make 1.50 L of solution
Calculate the molarity of a solution prepared by dissolving 1.56 g of gaseous HCl into enough water to make 26.8 mL of solution
Determine how much volume (in ml) will be needed to dissolved 2.50 g of solid NaCl to make 0.050M solution.
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E.g Solution Composition: Calculating Ion ConcentrationGive the concentration of all the ions in each
of the following solutions:0.50 M Co(NO3)2
1.0 M FeCl3
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E.g Solution Composition: Calculating Number moles from MolarityHow many moles of Ag+ ions are present in
25.0 mL of a 0.75 M AgNO3 solution?
How many moles of Na+ ions are present in 42.0 mL of 0.350M NaCl?
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Examples: Calculating mass from molarityTo analyze the alcohol content of a certain
wine, a chemist needs 1.00L of an aqeuous 0.200 M K2Cr2O7 (potassium dichromate) solution. How much solid K2Cr2O7 (molar mass = 294.2 g) must be weighed out to make this solution?
Formalin is an aqueous solutions of formaldehyde, HCHO,, used as a preservative for biological speciments. How many grams of formaldehyde must be used to prepare 2.5 L of 12.3 M formalin?
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15.5 DilutionReducing the original concentration of a
chemical solutionA 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
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ExamplesWhat volume of 16 M sulfuric acid must be
used to prepare 1.5L of 0.10 M of H2SO4 solution?
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
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15.6 Stoichiometry of Solution ReactionsSteps for solving stoichiometric problems
involving solutionsStep 1: Write a balanced equation for the
reaction. For each reactions involving ions, it is best to write the net ionic equation.
Step 2: Calculate the moles of reactantStep 3: Determine which reactant is limitingStep 4: Calculate the moles of other reactants
or products, as requiredStep 5: Convert to grams or other units, if
required
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ExamplesWhen Ba(NO3)2 and K2CrO4 react in aqueous
solution, the yellow solid BaCrO4 is formed. Calculate the mass of BaCrO4 that forms when 3.50 x 10-3 mole of solid Ba(NO3)2 is dissolved in 265 mL of 0.0100 M K2CrO4 solution
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ExamplesWhen 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
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Neutralization ReactionUse stoichiometry to determine how much of
acid or base must be used to reach neutralization
Strong acid: HCl(aq) H+(aq) + Cl-(aq)
Strong base: NaOH(s) Na+(aq) + -OH(aq)
Net equation: H+(aq) + -OH(aq) H2O(l)
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ExampleWhat volume of a 0.100 M HCl solution is
needed to neutralize 25.0 mL of a 0.350 M NaOH?
Calculate the volume of 0.10 M HNO3 needed to neutralize 125 mL of 0.050 MKOH
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15.8 Solution Composition: NormalityNormality is another unit of concentration
sometime used when dealing with acid and base
H+ and –OHEquivalent of an acid: the mount of acid that
can be furnish 1 mol of H+ ionsEquivalent of a base: the amount of that base
that can furnish 1 mol of –OH ions
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EquivalentE.g 1 mol HCl = 1 equiv HCl molar mass (HCl) = equivalent weight
(HCl)1 mol KOH = 1 equiv KOHmolar mass KOH = 1 equiv KOH½ mol H2SO4 = 1 equiv H2SO4
½ molar mass H2SO4 = 1 equiv H2SO4
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Solution Stoichiometry: Calculating Equivalent WeightPhosphoric acid, H3PO4 can furnish three H+
ions per molecule. Calculate the equivalent weight of H3PO4.
Calculate the equivalent weight of HBr
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Normality (N)Normality (N) = number of equivalent of
solute per liter of solution
Knowing Normality can help us calculateThe number of equivalentsThe volume of solution
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Calculating NormalityA solution of sulfuric acid contains 86 g of
H2SO4 per liter of solution. Calculate the normality of this solution
Calculate the normality of a solution containing 23.6 g of KOH in 755 ml of solution
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Neutralization The number of H+ ions furnished by the
sample of acid is the same as the number of –
OH ions furnished by the sample of base reacts exactly with
n equiv acid --------------- n equiv baseNacid x Vacid = Nbase x Vbase