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Definition
homogeneous (uniform) mixture of two or more substances, consisting of:
1. solvent
2. solute(s)
3. aqueous soln |
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| the bulk medium, ex: H2O (usually the larger amount) |
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| the dissolved substance(s), ex: NaCl (usually present in lesser quantities) |
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| measure of relative solute/solvent ratio |
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| accurately known concentration |
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| contains maximum amount of solute |
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concentration of a saturated solution, ex:,
solubility of NaCl is about 36 g NaCl/ 100 g H2O ("soluble")
solubility of CuS is about 10^-5 CuS/ 100 g H2O ("insoluble") |
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Term
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Definition
an "insoluble" reaction product
Ex: a precipitation reaction where the precipitate is AgCl:
NaCl (aq) + AgNO3 (aq) --> AgCl (s) + NaNO3 (aq) |
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Definition
solutes that produce ions in solution via dissociation (these solutions can conduct electricity)
Ex: NaCl (s) --> Na+ (aq) + Cl- (aq)
(NH4)2SO4 (s) --> 2 NH4+ (aq) + SO42- (aq) |
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| process of surrounding ions by H2O |
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Definition
100% ionized
-salts and acids can be electrolytes
HCl (g) --> H+ (aq) + Cl- (aq) |
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Definition
substances that are partially ionized (<100%)
weak acid (acetic acid) |
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substances that are not ionized and do not conduct electricity
C6H12O6 + H2O --> C6H12O6 + H2O (No ions are present!) |
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Definition
HCl
HBr
HI
HNO3
HClO4
H2SO4
soluble bases with OH- (i.e., NaOH, Ba(OH)2 |
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Definition
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Definition
C6H12O6 (glucose)
C12H22O6 (sucrose)
CH3OH (methanol)
C2H5OH (ethanol)
(NH2)2CO (urea) |
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Definition
| occur when aqueous solns are mixed and the reaction produces insoluble product (precipitate so ions are tied up) |
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| maximum amount of solute that will dissolve in a given quantity of solvent |
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| How does formation of insoluble product make a reaction occur? |
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Definition
| Because it prevents the products from reforming the original reactants |
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Definition
Soluble:
Acetates
Bicarbonates
Chlorates and perchlorates
Group 1
Ammonium
Nitrates
Group 7 (halides)
-EXCEPT
Ag+
Hg2 2+
Pb 2+
Sulfates
- Except
Ag+
Ca 2+
Sr 2+
Ba 2+
Pb 2+
Hg2 2+
Insoluble
Carbonates
Phosphates
Chromates
Sulfides
Except Group I and NH4+
OH : hydroxides
Except: Grop I and Ba 2+ |
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Term
| Metathesis Reaction ("double displacement") |
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Definition
Ions from two different reactants simply trade partners, Ex: ,,
NaCl (aq) + AgNO3 (aq) --> AgCl (s) + NaNO3 (aq) |
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Definition
appear uncharged on both sides of the equation
do not participate in the chemically important part of the reaction |
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Term
what is the net ionic equation?
What does it show?
Why is it useful? |
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Definition
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- The net ionic equation shows that, in general, a precipitate of BaCO3 will form whenever the ions Ba 2+ and CO 3 2- are combined in aqueous solution, regardless of their sources
- The essential chemical process can be written without the spectator ions in the net ionic equation |
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Definition
shows all compounds with complete,, neutral molecular formulas
useful in planning experiments and stoichiometry calculations |
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| Ionic Equation (complete) |
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Definition
- All strong electrolytes are show in their dissociated, ionic forms
- insoluble substances and weak electrolytes are shown in their molecular form
- spectator ions are included
- useful for showing all details of what is happening in the reaction |
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Definition
- "spectator ions" are omitted
- only the essential chemical process is shown, ex: formation of it
- solid precipitate
- gaseous product, or
- weak electrolyte (ex: water)
- useful for generalizing the reaction--the same important part can often be formed from different sets of reactants |
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| Occur when aqueous solns are mixed and the reaction produces a weak electrolyte (so ions are tied up) |
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Definition
Acids give H+ when dissolved in water and bases give OH-
Common acids: vinegar, lemon juice, aspirin
Common bases: milk of magnesia, lye |
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Definition
- taste sour
- cause color changes in dyes (litmus: blue to red)
- react with metals (Zn, Mg, Fe) to form H2 gas
2 HCl (aq) + Mg (s) --> MgCl2 (aq) + H2 (g)
- react with carbonates and bicarbonates to form CO2 gas
2 HCl (aq) + CaCO3 (s) --> CaCl2 (aq) + H2O (l) + CO2 (g)
- aqueous solutions conduct electricity (because there are ions present)
- react with bases to form salts and water
HCl (aq) + NaOH (aq) --> NaCl (aq) + H2O |
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Definition
- taste bitter
- feel slippery (ex: soaps)
- cause color changes in dyes (litmus: red to blue)
- aqueous solutions conduct electricity (because there are ions present)
- react with acids to form salts and water
HCl (aq) + NaOH (aq) --> NaCl (aq) + H2O |
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| Bronsted definition (broader) |
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Definition
Acid- proton (H+) donor
Base- proton acceptor |
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Definition
HCl (aq) --> H+ (aq) + Cl- (aq)
more correctly
HCl (aq) + H2O (l) __> H3O+ (aq) + Cl- (aq)
H3O+ is a hydrated proton called the hydronium ion |
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Term
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Definition
donate one hydrogen ion upon ionization
HCl (aq) --> H+ (aq) + Cl- (aq) |
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Definition
donate two hydrogen ions upon ionization
H2SO4 (aq) --> H+ (aq) + HSO4- (aq)
HSO4- (aq) ---> H+ (aq) + SO4 2- (aq)
<---
2 steps with the second being incomplete |
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| donate three hydrogen atom (H3PO4) |
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acid + base --> salt + water
(Neutralization reaction)
HCl (aq) + NaOH (aq) --> NaCl (aq) + H2O (l) |
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| Occur when aqueous solns are mixed and the reaction produces gaseous product (gas so ions are tied up) |
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| Oxidation-Reduction Reactions |
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Definition
electron transfer reactions
Ex: burning fossil fuels, bleach, rusting, some occur in water, others don't
2 Na + Cl2 --> 2 NaCl
2 half reactions
oxidation---loss of electron(s)
reduction---gain of electron(s)
half reactions:
Na ---> Na+ + e- (oxidation)
Cl2 + 2e- ---> 2 Cl- (reduction) |
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| the substance that is reduced |
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Definition
| the substance that is oxidized |
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Term
Oxidation Number
Rules for assigning oxidation numbers |
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Definition
a "charge" that is assigned to an atom to aid in a lancing redox reactions
- Generally, oxidation number is the charge that would result if all of the bonding electrons around an atom were assigned to the more electronegative element(s).
1. Free elements--oxidation number = 0
2. Ions of one atom: oxidation number= charge
3. Oxygen--usually -2; in peroxides (H2O2), O= -1
4. Hydrogen is usually +1, except when bonded to metals, ex: LiH, NaH in which H= -1
5. F= -1; Cl, Br, I (ions) = -1, but as molecular compounds, the charge varies and is positive
6. Sum of oxidation numbers = 0 in neutral compounds and equals the charge in polyatomic ions
7. Oxidation numbers are not always integers, ex: O2- (superoxides) = -1/2
Thus for
S (s) + O2 (g) --> SO2 (g)
- S (s) =0
- O2 (g)- 0
- SO2 (g): S= +4 and O = -2 |
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