SOLUTION STOICHIOMETRY Part 1a Unit 2 Chapter 4 1.
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Transcript of SOLUTION STOICHIOMETRY Part 1a Unit 2 Chapter 4 1.
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SOLUTION SOLUTION STOICHIOMETRYSTOICHIOMETRY
Part 1aPart 1a
Unit 2 Chapter 4Unit 2 Chapter 41
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SolutionsSolutions
A solution is homogenous mixture of 2 or more pure substances
Solvent: most abundant substance in a solution (water is the universal solvent because of strong polar bonds and bent shape)
Solute: all other substances present
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Water
• Called the “universal solvent”
• Bent shape (angle = 105)
• O – H bonds are polar covalent resulting from the more electronegative O atom attracting the electrons toward itself
• The O is partially negative while the H’s are partially positive
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Dissociation
• When an ionic substance dissolves in water, the solvent pulls the individual ions from the crystal and solvates them.
• This process is called dissociation.
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Dissociation
• An electrolyte is a substances that dissociates into ions when dissolved in water and produces a solution that can conduct electricity.
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Electrolytes
• A nonelectrolyte may dissolve in water, but it does not dissociate into ions when it does so.
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Electrolytes and Nonelectrolytes
Soluble ionic compounds tend to be electrolytes.
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Electrolytes and Nonelectrolytes
Molecular compounds tend to be nonelectrolytes, except for acids and bases.
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Electrolytes
• A strong electrolyte dissociates completely when dissolved in water.
• A weak electrolyte only dissociates partially when dissolved in water.
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Strong Electrolytes Are…
• HCl H+ + Cl – • 100 molecules of HCl yields ?
• Strong acids• Strong bases
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Strong Electrolytes Are…
• Strong acids• Strong bases• Soluble ionic salts
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Molarity• Two solutions can contain the same
compounds but be quite different because the proportions of those compounds are different.
• Molarity is one way to measure the concentration of a solution.
moles of solute
volume of solution in litersMolarity (M) =
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Molarity
• Example 1: a chemist makes a 400 mL solution by adding 67.4 g of AgNO3 to some water. What is the molarity of this solution?– Step 1 – convert from grams to moles
33
33 AgNO mol 0.3965
AgNO g 170
AgNO molAgNO g 67.4
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Molarity
• Example 1: a chemist makes a 400 mL solution by adding 67.4 g of AgNO3 to some water. What is the molarity of this solution?– Step 2 – calculate molarity
33 AgNO M 1
solution L 0.4
AgNO mol 0.3965
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Molarity
• Example 2: how many moles of a solute are present in 34 mL of 3.64 M Ba(OH)2?
2OHBa mol 0.090L 0.034M 3.64
VMnV
nM
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Molarity• Calculate the molarity of a solution by dissolving 11.5 grams of
solid NaOH in enough water to make 1500 mL of solution.
• Give the concentration of each type of ion in the following solutionsl:– 0.5 M Co(NO3)2
– 1.0 M Fe(ClO4) 3
• Typical blood serum is about 0.14 M NaCl. What volume of blood contains 1.0 mg NaCl?
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Mixing a Solution• To create a solution of a
known molarity, one weighs out a known mass (and, therefore, number of moles) of the solute.
• The solute is added to a volumetric flask, and solvent is added to the line on the neck of the flask.
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How would you do this?
• How would I make 1.00 L of an aqueous 0.200 M K2Cr2O7 solution
– 1. – 2.– 3.– 4.
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Dilution of stock solutions• One can also dilute a more concentrated
solution by– Using a pipet to deliver a volume of the solution to
a new volumetric flask, and– Adding solvent to the line on the neck of the new
flask.
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DilutionThe molarity of the new solution can be determined from the equation
Mc Vc = Md Vd,
where Mc and Md are the molarity of the concentrated and dilute solutions, respectively, and Vc and Vd are the volumes of the two solutions.
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Making Dilutions
• Example: Suzie needs 3L of a 0.05M HCl. She only has 12M HCl available. How much does she need to dilute to make her solution?
mL 10L 0.01V
V12M3L0.05M
VMVM
2
2
2211
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How would you do this?
• How would I prepare 500 mL of 1.00 M acetic acid from a 17.4 M solution– 1. – 2.– 3.– 4.
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Classifying Chemical ReactionsClassifying Chemical Reactions
• SynthesisSynthesis
• DecompositionDecomposition
• Single replacementSingle replacement
• Double ReplacementDouble Replacement
• CombustionCombustion
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SynthesisSynthesis
• Two or more substances react to form Two or more substances react to form ONE productONE product
A + B A + B AB AB
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SynthesisSynthesis
• Reaction of two elementsReaction of two elements
___Al + ___Cl2 ___AlCl3
Al3+ Cl1-
22 2233
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DecompositionDecomposition
• One substance breaks down into two One substance breaks down into two or more simpler productsor more simpler products
AB AB A + B A + B
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DecompositionDecomposition
__ NaN3 (s) ___ Na (s) + ___ N2 (g)2 2 3
__ CaO (s) ___ Ca (s) + ___ O2 (g)2 2
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Single Replacement ReactionsSingle Replacement Reactions
• One element replaces another One element replaces another element in a compound to form a new element in a compound to form a new compound and elementcompound and element
A + BX A + BX AX + BAX + B
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Reactivity SeriesReactivity Series
• MetalsMetals
• A more reactive metal will replace a A more reactive metal will replace a less reactive metal in a solutionless reactive metal in a solution
Li K Ca Na Mg Al Mn Zn Fe Ni Sn Pb Cu Ag Au
most active least active
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examplesexamples
• aluminum + iron (III) oxidealuminum + iron (III) oxide
Al Fe2O3+
More reactive?
Al3+ O2-
Al2O3Fe +
Fe3+ O2-
2 2
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examplesexamples
• silver + copper (I) nitratesilver + copper (I) nitrate
Ag CuNO3+
More reactive?
Cu1+ NO31-
NO RXN
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Double ReplacementDouble Replacement
• Exchange of Exchange of cationscations between two ionic between two ionic compoundscompounds
A B + C D AD + CBswitch
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Will the Solutions React?Will the Solutions React?
• One of the following things must One of the following things must occur for a reaction to occur:occur for a reaction to occur:–Precipitate is produced [(Precipitate is produced [(ss) or () or ()])]–Gas is evolved [(Gas is evolved [(gg) or () or ()])]–Water is made [(Water is made [(ll) or () or (gg)])]
• Use the solubility table to Use the solubility table to determine if a solid is madedetermine if a solid is made
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Example ProblemExample Problem
• Lithium iodide and aqueous silver nitrate Lithium iodide and aqueous silver nitrate reactreact
Li1+ I1- Ag1+ NO31-
LiI AgNO3 LiNO3AgI+ +(aq)
Use a solubility table to determine state of each component.
(aq) (s) (aq)
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CombustionCombustion
• Compound reacts with OCompound reacts with O22
• HydrocarbonHydrocarbon – compound with only – compound with only carbon and hydrogencarbon and hydrogen
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CombustionCombustion
• Combustion of hydrocarbonsCombustion of hydrocarbons
ALWAYS produces ALWAYS produces COCO22 and and HH22OO
CxHy + O2 CO2 + H2O
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Example ProblemExample Problem
• Show combustion of propane (CShow combustion of propane (C33HH88) gas) gas
C3H8 O2 CO2 H2O+ +5 3 4