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1. What are the two equations we have studied so far in this Unit?
2. How does a net ionic equation differ from a molecular equation?
Day 3 1-3
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1. Molarity, M or M
a. Most widely-used unit of __________________
b. Formula
concentration
M = # mols of solute # L of solution
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D. Dilution is adding more ________ to a solution to reduce the ________________. 1. Used to prepare solutions from
_______________ solutions.
2. Formula
solventconcentration
stock or conc.
VcMc = VdMd
(Volume of Conc.)(M Conc.) = (Volume of Dilute)(M of Dilute sol’n)
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First Solutions Lab
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A. A solute that forms ions in solution and
conducts ____________ is known as an _____________, while a solute that neither forms ions nor conducts ____________ is known as a ________________.
electricityelectrolyte
electricitynonelectrolyte
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B. Ionic compounds and some molecular compounds ____________ in water.
1. Strong electrolytes produce a _______ number of ions.
2. Weak electrolytes produce a _________ number of ions.
dissociate
larger
smaller
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C.Most molecular compounds _________ in water and are called _______________.
D. Solubility does not determine if a solute is a strong or weak electrolyte. 1. Acetic acid:
_____ solubility + ______ electrolyte
dispersenonelectrolytes
Only 1% is H+ + C2H3O2- in sol’n, rest is
HC2H3O2high weak
Equilibrium: HC2H3O2(aq) H+(aq) + C2H3O2
-(aq)
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2. Barium hydroxide:
____ solubility + ________ electrolyte
E. Solvation is the surrounding of _______ particles by particles of the ________. Known as ___________ when water is the solvent.
low strong
Not very soluble but
everything that dissolves dissociates
solutesolvent hydration
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ASSIGNMENT :
Page 548 #s 48, 50, 57, 58, 59, 60 (a and b), 61
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F. The Water Welcome Wagon!
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Was the Wicked Witch a good chemistry student?
Did she correctly and scientifically describe
her demise?
HW# 1 due tomorrow14
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A. Acids
1. Able to ionize and form ___ in aqueous solutions
2. Often referred to as ________ donors
3. Decrease the concentration of _____ in aqueous solutions
H+
proton
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OH-
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4. Monoprotic acids release ____ ___ per molecule of acid.
Ex:
5. Diprotic acids release _____ ___ per molecule of acid.
Ex:
one
H+
HCl, HNO3, HC2H3O2
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two H+
H2SO4H2SO4(aq) HSO4(aq) + H+
(aq)
HSO4(aq) SO-24(aq) + H+
(aq)
Only some of 2nd H+ come off
1st H+ always comes off
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6. Strong acids
7. Weak acids
- completely ionize in H2O chloric, hydrobromic, hydrochloric, hydroiodic, nitric, perchloric, sulfuric
- partly ionized in H2O, most acids are weak
acetic, hydrofluoric
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B. Bases
1. Able to ionize and form ____ in aqueous solutions
2. Often referred to as proton __________
3. Decrease the concentration of ___ in aqueous solutions
OH-1
acceptors
H+
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4. Metallic bases are called _____ ___________.
Ex:
5. Nonmetals can also form bases. Ex:
6. Strong bases
7. Weak bases
metal hydroxides
LiOH, NaOH
NH3
- Alkali + heavy alkaline earth metals: LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
19NH3, other metal hydroxides
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C. Salts
A salt forms when the __________ of an _____ is replaced by a different _______, generally from a _____. This usually occurs in a ________________ reaction.
Ex:
hydrogenacid cation
baseneutralization
HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)
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A. Metathesis reactions can also be called _______ ______________ reactions.
B.The mixing of 2 solutions will result in a chemical reaction if _____ are _________ from the solution.
double replacement
ions removed
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Metathesis (Exchange) Reactions
• Metathesis comes from a Greek word that means “to transpose.”
AgNO3 (aq) + KCl (aq) AgCl (s) + KNO3 (aq)
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Metathesis (Exchange) Reactions
• Metathesis comes from a Greek word that means “to transpose.”
• It appears the ions in the reactant compounds exchange, or transpose, ions.
AgNO3 (aq) + KCl (aq) AgCl (s) + KNO3 (aq)
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Solution Chemistry
• It is helpful to pay attention to exactly what species are present in a reaction mixture (i.e., solid, liquid, gas, aqueous solution).
• If we are to understand reactivity, we must be aware of just what is changing during the course of a reaction.
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Ions can be removed from solution by any of 3 processes:
1. The formation of an __________ solid, known as a _____________
2. The formation of either a weak
____________ or a ________________
3. The formation of a ____ that bubbles
out of the solution
insolubleprecipitate
electrolyte nonelectrolyte
gas
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Precipitation Reactions
When one mixes ions that form compounds that are insoluble (as could be predicted by the solubility guidelines), a precipitate is formed.
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C. ExamplesWrite the molecular, complete, and net ionic equations
for these reactions that occur in water.
1. Magnesium nitrate and sodium hydroxide
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C. ExamplesWrite the molecular, complete, and net ionic equations for
these reactions that occur in water.
2. Magnesium hydroxide and hydrochloric acid
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C. ExamplesWrite the molecular, complete, and net ionic equations
for these reactions that occur in water.
3. Chromium(II) acetate and nitric acid
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C. ExamplesWrite the molecular, complete, and net ionic equations
for these reactions that occur in water.
4. Iron(II) carbonate and hydrochloric acid
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Locate your lab paper for today!!!