chapter 4b
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Chapter 4B. Solutions. Solutions. Homogeneous mixture Solvent – substance present in the largest amount Solute – substance present in the smallest amount Aqueous solution – solutions with water as the solvent. Types of Solutions. Solubility. - PowerPoint PPT PresentationTRANSCRIPT
CHAPTER 4BSolutions
SolutionsHomogeneous mixture
Solvent – substance present in the largest amount
Solute – substance present in the smallest amount
Aqueous solution – solutions with water as the solvent.
Types of SolutionsSolute Solvent ExampleGas Gas Air ( O2, CO2 in N2)
Liquid Gas Water in airGas Liquid Carbonated beverages (CO2 in
water)
Liquid Liquid Vinegar (acetic acid in water)
Solid Liquid Sugar watersolid Solid Stainless steel (Cr and Ni in Fe
SolubilityThe maximum amount of a solute that
can be dissolved in a given amount of solvent at a constant temperature.
Factors that affect rate of Solubility (increase the rate of dissolving).
Pressure Temperature Polarity
SolubilitySolutions can be classified into groups by how much
solute is in solution.
Saturated – contains as much solute as the solvent can hold at a given temperature.
Unsaturated – less the maximum amount of solvent at a given temperature.
Supersaturated – contains more solute than the solvent can hold at a given temperature.
Solution by Mass PercentSolutions are described by mass percent
mass of solutemass percent= 100mass of solution
x
grams of solutemass percent= 100grams of solute +grams of solvent
x
Solutions by Mass PercentA solution is prepared by mixing 2.50
grams of calcium chloride with 50.0 grams of water. Calculate the mass percent of calcium chloride in this solution.
Solutions by Mass PercentA 75.0 gram sample of a solution is known
to contain 23.8 grams of glucose. Calculate the mass percent of glucose in this solution.
Solutions by Mass PercentVinegar is a solution of acetic acid in water
and typically contains 5.00% acetic acid by mass. Calculate the mass of acetic acid in a 250.0 gram sample of vinegar.
Solutions by Mass PercentConcentrated hydrochloric acid solution
contains 37.2 % by mass HCl. What mass of HCl is contained in 35.5 grams of concentrated HCl.
MolarityMolarity – concentration of a solution
moles of solute mM=molarity=liter of solution Lt
MolarityCalculate the molarity of a solution
prepared by dissolving 15.6 gram of solid KBr in enough water to make 1.25 L of solution.
MolarityCalculate the molarity of a solution
prepared by dissolving 2.80 grams of solid NaCl in enough water to make a 135 ml of solution
MolarityWhat mass of NaNO3 is required to make
2.50 Liter of a 0.150 M solution of NaNO3?
MolarityWhat mass of (NH4)2SO4 is required to
make 1.25 liter of 0.250 M solution of (NH4)2SO4?
Molarity-Ion ConcentrationGive the concentrations of all ions in each
of the following solutions
1.20 M Na2SO4 0.750 M K2CrO4
Molarity-Ion ConcentrationHow many moles of Na+ ions are present
in 42.0 ml of a 0.350 M NaCl solution?
Molarity-Ion ConcentrationHow many moles of Na+ ions are present
in 42.0 ml of a 0.350 M of Na3PO4 solution?
DilutionsProcess of adding more solvent to a solution.
M1=molarity before dilutionV1=volume before dilutionM2=molarity after dilutionV1=volume after dilution
1 1 2 2M V M V
DilutionWhat volume of 19 M NaOH must be used
to prepare a 1.0 Liter of a 0.15 M NaOH solution?
DilutionWhat volume of water is needed to
prepare 500.0 ml of a 0.250 M Ca(NO3)2 solution from a 5.00 M solution of Ca(NO3)2?
TitrationsCombining a solution of know
concentration with a solution of unknown concentration to determine the unknown.
Equivalence point – when the reactants are equal molar.
Indicator – dyes used in titrations to indicate equivalence point.
Titrations What volume of 0.115 M HCO4 solution is needed
to neutralize 50.00 ml of 0.0875 M NaOH?
15.00 ml of acetic acid is titrated with 0.500 M NaOH. It takes 22.59 ml of NaOH. What is the molarity of the acetic acid?
How many grams of AgBr are formed when 35.5 ml of 0.184 M AgNO3 are mixed with an excess of aqueous hydrobromic acid?