acid-base, pH, buffers

alkalemia (alkalosis)

pH higher than 7.45

acidemia (acidosis)

pH lower than 7.35

normal pH

between 7.35-7.45

how is blood pH managed?

• increasing respiration (to exhale more CO2)

• shifting buffer to consume more H+

in aqueous solutions, what do acids produce?

hydronium ions

(=poyatomic ion - water + proton(H+))

in aqueous solutions, what do bases produce?

hydroxide ions (OH)

(base + water → sodium + hydroxide)

ionic compounds containing hydroxide ions are what?

bases; OH

• also soluble in water, dissolve, strong/weak electrolytes

which of the ionic compounds are bases?

a) Ba(OH)2

b) NaBr

c) LiOH

d) CaBr2

A and C because they have OH-

what is the Bronsted-Lowry theory of acids and bases?

acid: a proton (H+) donor

base: a proton (H+) acceptor

acids according to the Bronsted-Lowry theory, using HCl and water

hydrochloric acid HCl, donates a proton to a water molecule, which acts as a base by accepting the proton

conjugate base

forms when a neutral acid loses a proton

• one fewer H+, so, -1 charge 

• HCl → Cl-

conjugate acid

forms when water acts as a base, and accepts a proton

• one more H+, so, +1 charge 

• H2O → H3O+

which have the extra proton, acids or bases?

acids

bases according to the Bronsted-Lowry theory, using HCl and water

HCl donates a proton to a water molecule, which acts as a base by accepting the proton

conjugate acid (neutral)

forms when a neutral base accepts a proton, +1 charge

conjugate base (neutral)

neutral water donates a proton to become this, -1 charge 

water according to Bronsted-Lowry theory

can accept or donate a proton, can act as an acid or a base

amphoteric compound

any substance that can act as an acid or a base (WATER)

what does pH measure 

the concentration of hydronium (H30+) ions in aqueous solution

common bases

compounds including hydroxide, carbonate, and bicarbonate; OH-, CO3 2-, HCO3-

buffer

solution that resists changes in pH when small amounts of acid or base are added

pH range

maintained by buffer, depends on identity of the weak acid

buffer capacity

depends on the concentration of the buffer components

respiratory acidosis

breathing weak and shallow so CO2 not exhaled, pH gets to low (acidic)

respiratory alkalosis

rapid breaking removes too much CO2, pH gets too high (basic)