solutions parts of a solution molarity, molality, mole fraction, dilution
TRANSCRIPT
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Solutions
Parts of a SolutionMolarity, Molality, Mole Fraction, Dilution
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Types of Mixtures• Mixtures : a blend of two or more kinds of
matter, each of which retains its own properties and characteristics
• Homogeneous vs. Heterogeneous Mixtures• Homo = same Hetero =
varied
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Solutions• Solution : homogeneous mixture of two or more
substances in a single phase
Parts of a Solution :• Solute – dissolved particles EX. Salt,
sugar• Solvent – dissolving medium EX. Water,
alcohol
• Aqueous = capable of being dissolved
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Concentrated vs. Dilute
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What is Molarity?• Moles of solute per volume of solution• Equation is GIVEN on Reference Table!
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Moles of solute per volume of total SOLUTION
Mol of solute Liters of solution
mol L
M
Moles of solute per mass of SOLVENT
Mol of solute Kg of solvent
mol kg
m
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What is molality?• Moles of solute per mass of
solvent• Equation is NOT GIVEN on
Reference Table!
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Molarity Examples• EXAMPLE : 3.50 L of solution contains 90.0 g of NaCl.
What is the molarity of the solution?
• EXAMPLE : 0.800 L of a .500 M HCl solution. How
many moles of HCl does this solution contain?
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Molality Examples• EXAMPLE : Solution was prepared by dissolving 17.1
g of sucrose (C12H22O11) in 125 g of water. Find the molal concentration of solution.
• EXAMPLE : A solution iodine (I2) in carbon tetrachloride (CCl4) is used when iodine is needed for certain chemical tests. How much iodine must be added to prepare a 0.480 m solution of iodine in CCl4 if 100.00 g of CCl4 is used?
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What is mole fraction?• MOLE FRACTION () =
• EXAMPLE : What is the mole fraction of xenon in a mixture that contains 0.584 g of xenon 86.40 g of argon and 3.62 g of neon ?
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DilutionsHow many
solute parts?
13 13
What’s the only difference?
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How can you dilute a concentrated solution?
• DILUTION =• EXAMPLE : What volume of 16 M sulfuric acid must
be used to prepare 1.5 L of a 0.10 M H2SO4 solution?