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24 Cards in this Set
- Front
- Back
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HCl
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Hydrocholric acid
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HBr
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Hydrobromic acid
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HI
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Hydroiodic acid
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HNO3
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Nitric acid
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H2SO4
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Sulfuric acid
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Weak acids
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Acetic Acid -CH3COOH
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KOH
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Potassium Hydroxide
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NaOH
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Sodium Hydroxide
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LiOH
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Lithium Hydroxide
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Ca(OH)2
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Calcium Hydroxide
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Mg(OH)2
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Magnesium Hydroxide
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Weak Bases
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Ammonia (NH3)
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pH scale. How to find it?
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pH = -log [H*]
[H]=[h30+]=10^=pH |
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Acids are characterized by
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dissolved in water produce H+ (arrhenious def). Proton donor (B/L def). turns indicator red. sour. dissolves metals sometimes.
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Neutralization reaction
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Strong acid + strong base = salt + water (or a ionic compound)
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Bases characterized by
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dissoved in water produce OH- (arrhenious def). Proton acceptor (B/L def). turns indicator blue. bitter. slippery
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Good bases
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group 1 & 2 hydroxides
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the more electronegative...
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the more acidic because the more stable with an electric charge and the more likely H+ will be donated.
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If concentration of H30+ > OH-...
If concentration of H30< OH-... |
Then it is acidic
then it is basic |
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Oxidation
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gain 0.
lose H lose e- |
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reduction
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lose O
gain H gain e- |
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rules for assigning oxidation/reduction states
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1. Free elements are assigned and oxidation state of 0.
2. Sum of all of the oxidation states of all the atoms in a compound or ions must equal the charge on that compound or ion. (ions are given and compounds always equal 0.) 3. Group I (alkali metals) are assigned oxidation state = +1 (H is not a metal so is not included in this group). 4. Flourine has ox. State = -1. No matter what paired with. 5. Group II (alkali earth metals) are assigned ox. State = +2. 6. Hydrogen is assigned ox. State = +1. 7. Oxygen is assigned an ox. State = -2. |
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oxidation agent
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the agent that is reduced is the agent becuase it causes other atom to be oxidized
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reduction agent
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the agen that is oxidized because it causes the other atom to be reduced
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