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Bronsted Acid
proton donor
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Bronstead base
proton acceptor
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conjugate base
the species that remains after the acid has donated its proton
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conjugate acid
the species formed when a base accepts a proton
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amphoteric
can be an acid or a base (example: water)
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ion constant of water
Kw = [H+] [OH-] = 1.0 x10 -14 at 25deg C
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pH & pOH equations
- pH = - log [H30+] or [H+]
- pOH = - log [OH]
- pH + pOH = 14
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strong acids
- HCl, HBr, HI, HNO3, HClO4, H2SO4
- the congugate base has no measureable stregnth
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strong bases
- bases that ionize completely in water
- soluble hydroxides fit this description
- LiOH, NaOH, KOH, Ba(OH)2, & Ca(OH)2
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percent ionization
- ionized acid concentration at equilibrium / initial concentration of acid x 100%
- [H3O+] / [HA]initial x 100%
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salts that produce basic solutions
- a weak acid and a STRONG base
- cation is neutral - alkali metal or alkaline earth metal
- anion is the conjugate base of a weak acid (HCOONa)
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salts that produce neutral solutions
- strong acid and a strong base
- cation is alkali metal or alkaline earth metal - can neither accept or donate a proton (Na+)
- anion is the conjugate base of a strong acid - has no measureable strength (only 5 choices)
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salts that produce acidic solutions
- strong acid and a weak base
- anion is neutral (the conjugate base of a strong acid)
- cation is acidic - conjugate acid of a weak base (NH4+)
- OR cation is a small highly charged metal (Al3+, Cr3+, Fe3+, Bi3+, Be2+) indirectly through water molecule
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the relationship between Ka and Kb
Ka x Kb = Kw
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salt
- an ionic compound formed by the reaction between an acid and a base
- strong electrolytes - they completely dissociate when dissolved in water
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salt hydrolysis
the reaction of the anion and/or cation of a salt with water
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Lewis acid
electron pair acceptor
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Lewis base
electron pair donor
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Lewis acid-base reaction
- does not produce a salt and water, it produces a new bond
- everything in bronsted would fit here, but reverse isn't true
- oxidation-reduction reactions (redox)
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Ka
[H30+] [CH3COO-] / [CH3COOH]
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Kb
[CH3COOH] [OH-] / [CH3COO-]
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hydrohalic acids
- acids of the halogens
- weakest to strongest goes down periodic table: HF, HCl, HBr, HI
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oxoacids
- acids that have oxygen in them
- 1. different central atoms in the same group and same oxidation # increases bottom to top (HClO3 is stronger than (HBrO3)
- 2. same central atom, but different # of attached groups (HClO4>HClO3>HClO2>HClO) increases with more attached
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