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10A-10C

QuestionAnswer
Acids - turns blue litmus paper red - corrosive - react with bases - low pH (0-6.9) - conduct electricity
Bases - turns red litmus paper blue - corrosive - react with acids - high pH (7-14) - tastes bitter - feel slippery
Bronsted-Lowry theory - describes acid base properties in terms of proton transfer - Bases Accept Acids Donates (BAAD)
Amphiprotic substances - can act as an acidor a base depending on what it is reacting with. eg. H2O, HSO4, HCO3. H2PO4, HPO4
Classification of acids - based on how many protons/hydrogens they can donate. > Monoprotic - acids that only donate one proton. > DIprotic - acids that donates two protons. > Triprotic - acids that donates three proton.
Strong vs weak strong - - will ionise fully - in a solution, will basically have no unreacted molecules. weak - - will ionise only a small amount - in a solution, there will be alot of unreacted molecules.
Strength vs Concetration strength: refers to the tendency to dissociate. concentration: refers to how much of a substance is present within a solution
Neutralisation reaction acid + base -> salt + water
Acid and metal hydroxides acid + metal hydroxide -> salt + water
Acid with metal carbonates acid + metal carbonate -> salt + water + carbon dioxide
Reactions of antacids - antacids are a type of medicine that neutralise the acid content in your stomach. - bases. - reaction will produce salt, water and SOMETIMES carbon dioxide. - some can form alginate (a salt of alginic acid)
Ionic product of water (Kw) - [H3O] = [OH] = 1.00 x 10^-7 M at 25 C - Because of this, the ionic productof water is 1.00 x 10^-14 M^2 and is represented by Kw.
pH - measeurement of acidity of a solution - pH of a solution (pH = -log10[H3O] - can be rearranged to [H3O] = 10^-pH
Need-to-know acids - HCL - H2SO4 - HNO3 - CH3COOH - H2CO3 - H3PO4
Need-to-know bases - NaOH - NH3 - Ca(OH)2 - Mg(OH)2 - Na2CO3
Created by: yaannica
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