CHEM1112 Lecture Notes - Lecture 14: Intravenous Sodium Bicarbonate, Sodium Hydroxide, Baking Powder
19 May 2018
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List common acids and bases
Acids
Acetic acid CH3COOH
Flavouring and preservative
Citric acid C6H8O7
flavouring
Phosphoric acid H3PO4
Rust remover
Boric acid B(OH)3
Mild antiseptic, insecticide
Hydrochloric acid HCl
Brick/ceramic tile cleaner
Many common acids have proton attached to O
Screen clipping taken: 28/10/2017 1:54 PM
Bases
Sodium hydroxide NaOH
Oven cleaner
Ammonia NH3
Household cleaner
Sodium carbonate Na2CO3
Water softener, grease remover
Sodium hydrogen carbonate NaHCO3
Fire extinguisher, baking powder
Many bases have a free OH- ion or N with a lone pair
e.g. LiOH, NaOH, KOH etc.
Screen clipping taken: 28/10/2017 1:55 PM
Strong acids and bases
Acids - H2SO4, HCl, HBr, HI, HNO3, HCl04
Bases - All hydroxides of groups 1 and 2 (except Be), NaOH, Ca(OH)2
Ch 11 sections 11.1-3
14.1
Saturday, 28 October 2017
1:36 PM
14. Strong Acids and Bases Page 1
Define acids and bases according to the Arrhenius and Bronsted-
Lowry models
Arrhenius
Screen clipping taken: 28/10/2017 1:55 PM
Acid = H+ producer in aqueous solution e.g. HCl
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Base: OH- producer e.g. NaOH
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Bronsted-Lowry
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Acid: proton DONOR e.g. HCl
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Base: proton ACCEPTOR e.g. NH3
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14.2
Saturday, 28 October 2017
1:37 PM
14. Strong Acids and Bases Page 2
Document Summary
Many common acids have proton attached to o. Sodium hydrogen carbonate nahco3 fire extinguisher, baking powder. Many bases have a free oh- ion or n with a lone pair e. g. lioh, naoh, koh etc. Acids - h2so4, hcl, hbr, hi, hno3, hcl04. Bases - all hydroxides of groups 1 and 2 (except be), naoh, ca(oh)2: strong acids and bases page 1. Define acids and bases according to the arrhenius and bronsted- Acid = h+ producer in aqueous solution e. g. hcl. Base: proton acceptor e. g. nh3: strong acids and bases page 2. A strong acid e. g. hcl = equilibrium to the right, so ha is completely ionised. If 1. 0 mols of acid added to enough water to make a 1. 0l solution, the solution will have. A weak acid e. g. ch3cooh = equilibrium to left, ha only partially ionised. Equilibrium given by ka, the acid dissociation constant. Conjugate base has one less proton than its conjugate acid e. g. hso4-
