Chemistry unit 6 acids/bases/ph/equilibrium

characteristics of acids

ph below 7, sour, turns blue litmus paper red, reacts with metals to produce hydrogen gas, reacts with carbonates to produce carbon dioxide gas

characteristics of bases

ph above 7, bitter, feels slippery, turns red litmus paper blue

acids and bases neutralization reaction

acid + base = salt + water

Arrhenius definition of an acid

produces a proton (H+) when dissolved in water

Arrhenius definition of a base

produces a hydroxide ion (OH-) when dissolved in water

Bronsted lowry definition of an acid

proton donor

Bronsted lowry definition of a base

proton acceptor

Conjugate base

product formed when acid loses H+ (formerly acid)

conjugate acid

product formed when a base gains H+ (formerly base)

Kw concentration equation

Kw=(H+)(OH-) = 1×10^-14

ocean acidification

CO2 diffuses into the ocean water and forms carbonic acid when reacting with it. The carbonic acid gets disassociated and hydrogen ions (H+) are formed. Increase in H+ ions lowers the pH because ph=-log(H+). Lower pH causes less carbonate to form, so there’s less carbonate to form calcium carbonate to make up the shells of marine life

Effect of temperature on equilibrium

Increases in temperature push the reaction in the direction that absorbs the heat (endothermic), vice versa for exothermic. Endothermic means + heat on left and exo means + heat on the right.

Effect of pressure on equilbrium

pressure only affects equilibrium when there’s an unequal amount of moles of gaseous reactants and products. Increases in pressure (decrease in volume) pushes equilibrium to the side with fewer molecules

Effect of concentration on equilibrium

If reactants are added, shift to products. If products are added, shift to reactants

equilibrium expression

keq = product on top, reactants on bottom, exponents are coefficients