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Acids and Bases

QuestionAnswer
Acid Properties sour, corrosive, reacts with indicators and bases, electrolytes
Base Properties bitter, caustic (skin, hair, protein), slippery, react with indicators and acids, electrolytes
Strong Acids HCl, HBr, HI, HNO3, HClO4, H2SO4
HCl Hydrochloric
HBr Hydrobromine
HI Hydroiodic
HNO3 Nitric
HClO4 Perchloric
H2SO4 Sulfuric
Strong Bases w/ OH Li, Na, K, Rb, Cs, Fr
Strong Bases w/ (OH)2 Ca, Sr, Ba
Arrhenius Acids contain H+ ions and bases contain OH- ions
Bronsted Acids donate protons (H+) and bases accept protons
Polyprotic Acids that can donate more than 1 proton per molecule
Self Ionization of water HOH <-> H+ + OH-
Equilibrium Constant K=[H+] {OH-] = 1 E -14
pH using H pH = -log [H+]
pOH using OH pOH = -log [OH-]
OH with pOH [OH-] = 10^-pOH
pH + pOH pH + pOH = 14
Strong Acid with Strong Base H+(aq) + OH-(aq) -> H2O
Strong Acid with Weak Base H+(aq) + XXOH(aq) -> H2O(l) + X+(aq)
Weak Acid with Strong Base HX(aq) + OH-(aq) -> H20(l) + X-(aq)
Molarity equation M = mol/V (L)
acid mol and base mol mols of acid = mols of base
acid and base MV = MV
Titrating Strong Acid and Strong Base pH ~ 7, about any indicator works
Titrating Strong Acid and Weak Base <7, methyl orange / red
Titrating Weak Acid and Strong Base >7, phenolphthalein / phenol red
Molar Mass equation MM = g/mol
Hydronium Ion Acidic, H3O+
Amphoteric Can be base or acid
pH value meaning How acidic (<7) or basic (>7) something is
What is in pure water H2O
Dissociation equation <-> when Weak, -> when strong break into cation and anion
Acid, Base, Conjugate acid, and Conjugate base Remove one H+ from Acid to turn to Conjugate Base Add one H+ to Base to turn to Conjugate Acid
Endpoint of titration When color changes, moles of acid and base are equal
Indicator meaning To tell when the moles are equal
Phenophthalein in acid/base Colorless in acid, Pink in base
Bromthymol blue in acid/base Yellow in acid, Blue in base
Acid Rain SO3 comes from burning of coal 2NO2 comes from burning of gasoline
Created by: Hola0205
 

 



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