Chapter 9; Acids and Bases, pH, and Buffers Flashcards
what is the acid base homeostasis range
7.35 - 7.45
proper organ function requires blood pH
what is the pH balance range
0 - 14
what is the range of pH for blood pH
6.6 - 8.0
protons, H+, cause fluids to be
acidic
in blood pH what does having more than 7.4 pH lead to
7.4 - 7.8 = alkalosis
7.8 - 8.0 = death
in blood pH what does having less than 7.4 pH lead to
7.4 - 6.8 = acidosis
6.8 - 6.6 = death
what is the range of blood pH for it to be acidosis
pH < 7.35
what is the range of blood pH for it to be alkalosis
pH > 7.45
what is the blood pH ranges
6.6 - 8.0
what does cellular metabolism produce in acid base homeostasis in the blood
substances that affect blood pH such as CO2 and H+ ions
how is blood pH maintained in acid base homeostasis in the blood
- increasing respiration to exhale more CO2 or
- shifting buffer equilibrium to consume more H+
what do acids produce in aqueous solutions
hydronium ions, H subscript 3 O+ ; H3O+
what is the formula for hydronium ions
H3O+
what is the hydroxide ion formula
OH-
what do bases produce in aqueous solutions
hydroxide ions, OH-
according to the Arrhenius definition what are the two conditions
- an acid is a substance that produces hydronium ions, H3O+
- and a base is a substance that produces hydroxide ions, OH-, in aqueous solution
what are group 1A hydroxide salts in ionic compounds containing hydroxide ions being bases
NaOH, KOH
soluble in water
strong electrolytes
dissolve entirely to produce ions in water
(contains hydroxide ions, OH, are bases)
what are 2A hydroxide salts in ionic compounds containing hydroxide ions being bases
Ca(OH)2, Mg(OH)2
slightly soluble in water
weak electrolytes (not many ions)
dissolve slightly to produce few ions in water
(containing hydroxide ions, OH, are bases)
ionic compounds composed of hydroxide ion (OH-) are bases because they produce
solvated hydroxide ions in solution
are soluble hydroxide ion salts (group 1A salts strong or weak electrolytes
strong
are slightly soluble hydroxide ion salts (group 2A salts) strong or weak electrolytes
weak
in the Bronsted-Lowry theory of acids and bases, how are an acid and base differentiated
acid: a proton (H+) donor
base: a proton (H+) acceptor
hydrochloric acid, HCl, donates a proton to a water molecule, acts as a
base by accepting the proton
in bronsted lowry theory what is the term of neutral acid loses proton to form
conjugate base
(one fewer H+ and, a -1 charge; compared to formula of acid
in bronsted Lowry theory what is the term when water acts as a base, accepting proton to form
conjugate acid
(one more H+, a +1 charge; compared to formula of base)
observation; in the bronsted Lowry theory what differentiate an acid from a base
acid ; with water the acids are only two molecules typically with a hydrogen at the front. e.g. HCl + H20 -> H30+ + Cl-
base; the base has more than two elements when reacting with water.
e.g. NH3 + H2O <–> OH- + NH4+
what does a neutral base combine with/ accepts to produce its conjugate acid according to the bronsted Lowry theory
H+
base + H+ (<-,->) conjugate acid
neutral water donates a proton to form its conjugate base
H+
one fewer H+, and thus, a -1 charge
according to the Bronsted Lowry theory, can water accept and/or donate a proton
can accept or donate
can water act as an acid or a base according to the bronsted Lowry theory
both
what is the term under the bronsted Lowry theory for any substance that can act as an acid or a base
amphoteric compound
in a conjugate acid-base pair; an acid and its conjugate base or a base and its conjugate acid are called a conjugate acid-base pair
yes
can all H+ be donated
usually indicated at the beginning of the formula
e.g
HCl -> Cl- chloride ion
HC2H3O2 -> C2H3O2- acetate ion
the strength of an acid depends on the ….
extent to which the acid donates a proton to water
the strength of a base depends on the extent to which…
the base accepts a proton from water
strong acids dissociate in water […] to form a conjugate base and hydronium ions
completely
is HCl really strong
yes, the only strong acid produced in the human body
strong acids are highly […] when concentrated but are safe to handle as […] solutions
corrosive
dilute
what are the common strong acids
HNO3 nitric acid
H2SO4 sulfuric acid
HCLO4 perchloric acid
HCl hydrochloric acid
HBr hydrobromic acid
HI hydroiodic acid
in a solution, what does the strong acid contain mostly and very little of
mostly H3O+ and the conjugate base, and very little of the acid
why are strong acids strong electrolytes
base they produce many ions in solution
what groups make up strong bases
1A and 2A metal ions with hydroxide ions
do strong bases (groups 1A and 2A) completely dissociate in aqueous solutions
yes, producing hydroxide ions and cations (conjugate acids)
are strong bases (1A and 2A) strong electrolytes
if soluble
strong bases (1A and 2A) are […] corrosive when concentrated; can be handled safely as […] solutions
highly
dilute
what are common strong bases
Ba(OH)2 Barium hydroxide
Ca(OH)2 Calcium hydroxide
LiOH Lithium hydroxide
KOH Potassium hydroxide
NaOH Sodium hydroxide
Sr(OH)2 Strontium hydroxide
appear to contain OH
strong acids […] ionize, where weak acids only […] ionize
completely
partially
weak acids and weak bases are characterized
- little dissociation in water; produce ions in aqueous solution; are weak electrolytes
- reaction with water is reversible.
- at equilibrium reactants>products
a weak acid, and similarly a weak base, undergo a reversible reaction with water that, at equilibrium, favors the […]
reactants
what are e.g. of weak acids
CH3COOH
H3PO4
H2CO3
any acid not listed in the six common strong acids
what are some weak bases
NH3
CH3NH2
what is Le Chatelier’s principle
reaction shifts in direction that counteracts a disturbance
- forward reaction enhanced (a shift to the right) until a new equilibrium is attained)
- reverse reaction enhanced (a shift to the left) until a new equilibrium is attained
what is Le CHatelier’s principle important in reactions for
weak acid and weak base reactions
what are biochemical pathways in Le Chatelier’s principle
reactions are approaching equilibrium
how to identify a weak strong or non electrolyte through pictures
weak; some + and - charges while others have no indication of charge
strong; equal number of + and - charged particles
non; no indication at all of charges
e.g. of weak acids
- organic acids; acetic acid (HC2H3O2) & citric acid (H3C6H5O7)
- inorganic acids; carbonic acid (H2CO3), phosphoric acid (H3PO4), and hydrofluoric acid (HF)
- any acid not listed in the six common acids
is ammonia, NH3, a weak or strong base
weak
what does pH measure
concentration of hydronium ions (H3O+) in aqueous solution
Low pH levels indicate
High pH levels indicate
high or low acid concrentrations
- high acid concentration
- low acid concentration
H3O+ = molar concentration (mole/L) of
H3O+
OH- = molar concentration of
OH-
pH < 7 is
acidic
[H3O+] > [OH-]
brackets indicate concentration of hydroxide ions
pH > 7 is
basic (alkaline)
[H3O+] < [OH-]
brackets indicate molar concentration
PH = 7 is
neutral
[H3O+] = [OH-]
brackets indicate molar concentration
what is auto ionization of water
occurs when very few water molecules react with other water molecules to produce hydronium ions and hydroxide ions
e.g. H2O + H2O <–> OH- + H3O+
the increase or decrease of any reactant or product in the solid or liquid phase regarding equilibrium have any effect
no
what does a catalyst do to a reaction
speed it up
in pure water at 25 degrees celsius what is the power of 10 for M in H3O+
1.0 x 10^-7 M
In pure water at 25 degrees celsius what is the power of 10 in M for OH-
1.0 x 10^-7 M
what is the power of 10 for K subscript w Kw
Kw = 10^-14
which is
Kw = [H3O+] x [OH-]
Kw is
ion product constant for water
when acid or base is added to water, auto ionization of water shifts, but Kw is
constant. Kw = 10^-14
when hydronium ion […], hydroxide must […] under the ion product constant
increase
decrease
when adding acid to water; what does [H3O+] increases from 1x10^-7 M to
1x10^-6 M
how to calculate the pH from the hydronium ion concentration
pH = -log subscript 10 [H3O+]
for pure water,
pH = -log subscript 10 [1x10^-7]
when calculating pH from the hydronium ion concentration what is pH of an aqueous solution
the logarithm of the hydronium ion concentration multiplied by -1
to find the [OH-] hydroxide ion
pH + pOH = 14
pH decreases as what increases
hydronium ions;
H3O+
the more hydronium ions [H3O+] the more the solution is
acidic
the more hydroxide ions [OH-} the more the solution is
basic
for the pH to be more acidic or more basic what doe the pH reflect on
H3O+
what is the equation of finding the H3O+ concentration when only given pH
[H3O+] = 10^-pH
what is the equation of finding the OH- concentration when only given pH
14 - pH = pOH
[OH-] = 10^-pOH
when an acid is combined with a base, a neutral product is formed, and a […] reaction has occurred
neutralization
in an acid base neutralization reaction what type of replacement reaction occurs
double replacement
what reacts with stomach acid (HCl) and neutralizes the acid
antacids
what are the common bases used in neutralization reactions
ionic compounds containing
- hydroxide ion, OH-
- hydrogen carbonate ion, HCO3-
- carbonate ion, CO subscript 3 charge -2
sodium and chloride ions are unchanged during the reaction; they remain in solution as
spectator ions
acids with more than one acidic proton are known as
polyprotic acids
e.g.
sulfuric acid, H2SO4
phosphoric acid, H3PO4
citric acid, H3C6H5O7
in neutralization reactions with polyprotic acids,
- all acidic protons can be donated in a neutralization reaction
- one hydroxide ion is needed to neutralize each acidic proton
- combine the spectator ions in a ratio that forms a neutral salt for the ionic compound
in a hydrogen carbonate and carbonate ion containing bases; ionic compounds hydrogen carbonate, HCO3-, and carbonate ion, CO3-
- are weak bases
- are frequently used in neutralization reactions, and
- can react with acids to produce water an ionic compound and CO2 gas
in a neutralization reaction what do the reaction of an acid with a hydroxide ion containing base produce
water and a dissolved salt
what is the net reaction in a neutralization reaction that produces water and a salt
H+ + OH- -> H2O
in a neutralization reaction that produces water and a salt; how is the solution neutral
when an equal number of moles of hydroxide ions, OH-, and protons, H+, are combined
a buffer is a solution that […] change in pH when small amounts of acid or base are added
resists
what is pH range in buffer components
maintained by buffer depends on identity of the weak acid
what is buffer capacity in buffer components
depends on the concentration of the buffer components
in buffer components the strength of the acid + its conjugate base is in similar concentrations
yes
weak acid + conjugate base = conjugate base
strong acid + conjugate base = stronger buffer
a buffer resists changes in pH because the equilibrium shifts in response to the […] or […] of H3O+, maintaining the concentration of H3O+. the addition of hydroxide ion is equivalent to the removal of hydronium ion, H3O+
addition
removal
what is respiratory acidosis
breathing weak and shallow so CO2 is not exhaled
causes a shift to the right, increasing [H3O+] and decreasing pH
what is metabolic acidosis
kidneys do not release sufficient HCO3- to support normal shift to the left
leads to increasing [H3O+] and decreasing pH
for treatment what is respiratory or metabolic acidosis
IV infusion of HCO3- causing a shift to the left
what is respiratory alkalosis in treatment
breathing into a paper bag to increase blood CO2 and shift equilibrium to right
what is metabolic alkalosis in treatment
IV infusion of dilute HCl causing a shift to right
a buffer contains either a
weak acid and its conjugate base,
or
a weak base and its conjugate acid.
what is the charge of SO4
-2
what is the charge of NO3 (nitrate)
-1
what is the charge of PO3
-3
what is the charge of ClO
-1
what is the charge of HPO4
-2
what is the charge of NO2
-1
What is the charge of PO4 (phosphate)
-3
what is the charge of SO3
-2
what is the charge of NH4
+1
what is the charge H3O
+1
when finding the net ionic equation for the reaction
break down each molecule that is aquatic
A strong acid can react with a weak base in the buffer to form a weak acid, which produces
A few H+ ions in solution and therefore only a little change in pH
what are common buffers
CH3COOH - acetic acid/acetate buffer
H2CO3 - carbonic acid/hydrogen carbonate buffer
during exercise, [H3O+] increases or decreases, causing a shift to the left, producing more H2CO3, shifting left again to produce more CO2, which is exhaled by increasing ventilation
increase
kidneys can support the shift to the left by releasing additional HCO3- into the blood
