2.6 Chemical Reactivity
Equilibrium
Acids and Bases
Little Notes To Remember:
Horizontally on the periodic table is Period
Vertically on the periodic table is group
When a reaction doesn't only go forward, but some of the reactants that have been made go back to products.
Will not necessarily mean that it will be a 50:50 ratio in the test tube but it can be any ratio even not as a tidy number.
To change the ratio of the equilibrium, you can add a more concentrated acid, adding more pressure, or changing the temperature can favor one side of the reaction.
Equilibrium Constant; Kc
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Catalysts only speed up the equilibrium reaction but will not affect the overall ratio because it only is used to increase the rate of reaction, meaning more frequent collisions per unit of volume.
The more concentrated the acid, the more H3O atoms it has inside of the acid.
The more dilute an acid is, the more OH- particles in it.
Every strong acid has a conjugate base, Every strong base has a conjugate acid.
Acid = Anything that donates a proton, Base = Anything that accepts a proton.
Amphiprotic Substance = It can do either, It can act as any.
Acidic Solution = pH = <7 (More H3O+ than OH-). Neutral = pH = 7 (Balanced H3O+ and OH-). Basic (Alkaline) Solution = pH >7 (More OH- than H3O+).
Kw = Ionic Product of Water, 1x10^-14. Always results into that OVR.
Only applies for the eqilibrium equation H2O + H2O = H3O + OH-
Concentrated VS Dilute
Concentrated
Dilute
Less H2O
More H2O
Weak VS Strong
Weak
Strong
Less H3O+
More Hydrochloric Acid
More H3O+
Less Hydrochloric Acid
Salts
H2SO4 makes Sulfate Salt
CH3COOH makes Ethanoate Salt
HNO3 makes Nitrate Salt
HCl makes Chloride Salt
Reactions of Acids
Acid + Base -> Salt + Water
Acid + Carbonate -> Salt + Water + Carbon Dioxide
Acid + Metal -> Salt + Hydrogen