Week 4 Day 1

can be used to predict the affect of change in conditions on a chemical equilibrium Keq= [Ceq]c * [Deq]d/[Aeq]a * [Beq]b

[H+]=[OH-] = 1.0 x 10-7

molecule that donates a H+

molecule that accepts an H+

what is left after an acid has donated a proton

formed by a base accepting a hydrogen

pH = pKa + log([A-] / [HA]) Used to calculate the pH of a buffer and states the pH of a buffer is equal to the pKa of the weak acid plus the log of the ratio of the concentration of the conjugate base [A-], divided by the concentration of the acid [HA]

a solution that can resist change in pH upon addition of acidic or basic components Usually consists of a weak acid and its conjugate base

pH: 7.4 (7.35-7.45) CO2: 40 mmhg (35-45) HCO3: 24 mM (20-28)

Increased CO2 decreased pH increased HCO3- normal BE

increased CO2 close to normal pH very increased HCO3- > +2 BE

decreased CO2 decreased HCO3- or increased H+ decreased pH negative <-2 BE

decreased CO2 decreased HCO3- about normal pH negative <-2 BE

decreased CO2 decreased HCO3- increased pH normal BE

decreased CO2 very decreased HCO3- about normal pH negative <-2 BE

increased CO2 increased HCO3- increased pH positive >+2 BE

increased CO2 increased HCO3- about normal pH positive >+2 BE

Na+ - (Cl- + HCO3-) high anion gap = addition of acid normal anion gap = loss of base

Hydrochloric acid strong acid

hydrobromic acid

hydroiotic acid

nitric acid

chloric acid

perchloric acid