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Acids and Bases

Acid pH 0-6
Base pH 8-14
pH scale sale from 0-14 to indicate the acidity or alkalinity of a substance
H3O+ The chemical formula for a hydronium ion; produced by acids in water
Neutralization Reaction the reaction of an acid and base to form a neutral solution of water and salt
Strong Acids HCl, HClO, HI, HNO3, HBr, H2SO
acid properties sour taste, burns skin
base properties slippery on skin, bitter taste
Strong Bases Soluble compounds containing the hydroxide ion
Neutral same amount of H+ and OH- ions; 7 on pH scale
Buffer solutions in which the pH remains relatively constant, even when small amounts of acid or base are added
Neutral Salt salt formed from reaction of a strong acid and strong base
Acidic Salt a salt formed from a reaction of a strong acid with a weak base
Basic Salt a salt formed from a reaction of a weak acid with a strong base.
Lewis Acid electron pair acceptor
Lewis Base electron pair donor
Arrhenius Acid H+ producer
Arrhenius Base OH- producer
Bronsted-Lowry Acid Proton (H+) donor
Bronsted-Lowry Base H+ acceptor
amphoteric Compound that can act as a proton donor or acceptor
conjugate base original acid after it donates its hydrogen ion
conjugate acid original base after it gains a hydrogen ion
equivalence point in a titration, where equal amounts of H+ and OH- have reacted
titration formula M1V1=M2V2
Indicators weak acids or bases that have a different color from their original acid and base
Naming rules for Binary Acids Hydro_____ic Acid
Naming rules for oxyacids that contain -ate ions _____ic Acid
Naming rules for oxyacids that contain -ite ions ____ous Acid
Naming rules for oxyacids that contain one less oxygen than the compounds –ite ion Hypo_______ous Acid
Naming rules for oxyacids that contain more oxygen than the compounds –ate ion Per_______ic acid
Created by: laurenmccarthy


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