Studied by 4 people
In the Acid-Base Theory, what is an acid?
A proton/H= ion donor
In the Acid-Base Theory, what is a base?
A proton/H+ acceptor
What is the species formed when a proton is added to a base
A conjugate acid
what is the species formed when a proton is removed from an acid
a conjugate base
What is the name of a species that can either accept or donate a proton?
Amphiprotic
What makes a species amphiprotic?
Has an H+ ion, but can also accept H+
What is H2O
amphiprotic
what is HCO3-
Amphiprotic
what is H2SO4
amphiprotic
what is H2PO4
amphiprotic
What is HPO4 2-
amphiprotic
what is the conjugate base of nitric acid
NO3-
What is the conjugate acid of cyanide
HCN
what is the conjugate base of bicarbonate
CO3 2-
what is the conjugate acid of bicarbonate
H2CO3
What is the ion product constant of water
1.0 × 10^-14
What makes a solution neutral
[H+] = [OH-]
if [H+] > 1.0 × 10^-7 M, then [OH] is ___ 1.0 × 10^-7
[OH] < 1.0 × 10^-7 M
if [H+] > 1.0 × 10^-7 M, then the solution is _______
acidic
if [H+] < 1.0 × 10^-7 then [OH] is ___ 1.0 × 10^-7 M
[OH] > 1.0 × 10^-7 M
if [H+] < 1.0 × 10^-7, then the solution is _______
basic
What is Kw = to
[H+][OH-]
The higher the pH, the ________ acidic the solution
less acidic
the lower the pH, the _______ acidic the solution
more
What is pH = to
-log(H+)
To get to [H+] from pH, what do you do?
10^-pH, or 10^-pOH
To get from pOH to pH
14 - pOH = pH
what is HCl
strong acid
what is HBr
strong acid
what is HI
strong acid
What is HClO4
strong acid
what is HNO3
strong acid
what is H2SO4
strong acid
what is LiOH
strong base
what is NaOH
strong base
what is KOH
strong base
what is Ca(OH)2
strong base
what is Sr(OH)2
strong base
what is Ba(OH)2
strong base
what is H3PO4
weak acid
what is HNO2
weak acid
what is CH3COOH
weak acid
what is H2SO3
weak acid
what is NH3
weak base
what is C5H5N
weak base
What is CH3NH2
weak base
what is the formula for nitric acid
HNO3
What is the formula for barium hydroxide
Ba(OH)2
how can you measure pH
pH meter, indicators, or pH paper
we can predict that solutions with transition metal cations are _____
acidic
stronger weak acids have a ____ kA in comparison to weaker weak acids
higher
stronger weak acids have a _______ Pka in comparison to weaker weak acids
lower
weaker acids have a ________ k in comparison to stronger acids
lower
weaker acids have a _______ Pka in comparison to stronger acids
higher
what does % ionization depend on
Ka value, initital concentration of the acid
the higher the starting concentration of an acid, the _________ % ionization
lower
the lower the starting concentration of an acid, the ______ % ionization
higher
the “-x” can be ignored in an ice diagram if % ionization is __________
less than 5%
how to calculate % ionization
[H+] divided by starting [acid] x 100
in a diprotic weak acid, what happens to the conjugate acid from step 1?
it becomes the acid of step 2
what is the equation for [H+] of a diprotic acid
the square root of (Ka1 x [acid])
what is the equation for the concentration of a base for a diprotic acid
[B] = Ka2
What kind of anion would make a compound neutral
anions of strong acids/spectator ions
what kind of cation would make a compound neutral
group I and II cations
what anion would make a compound basic
conjugate bases of weak acids
what cation would make a compound basic
none
what anion would make a compound acidic
amphiprotic acids
what kind of cation would make a compound acidic
the conjugate acids of weak bases, or transition metal cations (ex. NH3)
A has a KB of 1, B has a KB of 2, which is a stronger base?
B
A has a PKb of 1, B has a PKB of 2, which is a stronger base?
A
How to calculate pOH?
-log([OH-]
how to calculate pH from pOH
14 - (-log[OH-])
how strong/weak is the conjugate base of a stronger acid
very weak
what is the relationship between the strength of acids and the strength of their conjugate bases
inverse (one goes up the other goes down)
what is a salt
an ionic solid containing a cation other than H+ and an anion other than OH or O2-
What happens when a salt dissolves in water?
the cation and anion seperate from one another
in a salt, what does it mean if Ka > Kb
the salt is acidic
in a salt, what does it mean if Ka < Kb?
the salt is basic
how to determine whether an amprotic compound is acidic or basic
see if the Ka or Kb is higher
what does a lewis acid do
accepts an electron pair
what does a lewis base do
donates an electron pair
how to determine the [H+] in water if given the [OH-]
1.01 × 10^-14 = [H+][OH-]
what is the formula for acetic acid
HC2H3O2
how to calculate the Ka of a weak acid
[H+][B-]/[HB]
how to calculate PKa if given molarity of reactant
set up ice diagram, solve for x (x2/[]), calc Ka ([A][B-]/[HB]), calc pKa (-log(ka))
how to solve for pKA from Ka
-log(Ka)
what makes an acid stronger/weaker
longer bonds to H (increasing atomic radius), or more polar bonds to H
practice question: is NaI acidic, basic, or neutral?
neutral
practice question: is LiH2PO4 acidic, basic, or neutral?
acidic
practice question: is KOH acidic, basic, or neutral?
basic
practice question: is Cr(NO3)3 acidic, basic, or neutral?
acidic
practice question: is KNO2 acidic, basic, or neutral?
acidic
practice question: is NaCN acidic, basic, or neutral?
basic
practice question: is FeCl3 acidic, basic, or neutral?
acidic
This acid is an H+ donor. It’s named after two famous chemists.
Brønsted-Lowry acid
Note: This is also an Arrhenius acid.
This base is an H+ receiver. It’s also named after two famous chemists.
Brønsted-Lowry base
This base is an OH- donor. It’s named after one famous chemist.
Arrhenius base
This acid only donates one proton (H+) when it dissociates.
Monoprotic acid
What is the opposite of a monoprotic acid? What is its main property?
Polyprotic acid; gives more than one H+ in solution
True or False? Water itself auto-ionizes through the reaction below without any real effect on pH.
2H2O(l) ⇌ H3O+(aq) + OH-(aq)
True
Note 
Flashcard (108)