Definitions
Difference between monoprotic, diprotic and triprotic
Monoprotic- one ionizable proton (donate one H)
Diprotic- two ionizable protons (donate two H)
Triprotic- three ionizable proton (donate three H)
What is pH and how is it related to concentration of [H+]
-log[H+]
higher [H+]= lower pH= Acid
Lower [H+] = higher pH= Basic
pH less than 7, equal to 7, and greater than 7
less= Acid, More=basic, equal to 7 is neutral
If the [OH-] = 1*10^-11, what is the [H+]
1*10^-3
Strong acids vs weak acids difference in ionization
A strong acid ionizes alot (gives off alot of hydrogen) and a weak acid ionizes a little (gives off fewer hydrogen)
Formula for hydrogen ion
H+
If the [H+] = 1*10^-1, what is the [OH-]
1 *10^-13 M
The lab process of adding a known amount of solution of known concentration to determine the concentration of another solution
Titration
If pH=7 , what is the [H+]
1 *10^-7
What does a buffer do
Resist change in pH when small amounts of acid or base are added
Arrhenius Acids and Bases
Acids- produces H+ ions in water
Bases- produces OH- ions in water
If hydroxide concentration is 1*10^-12 M what is the pH
pOH=12 , pH =2
Compare and contrast Acids and Bases in different indicators
Acids- Red, Bases- Blue , Neutral-Green
Phenolphthalein
Acids/ Neutral- Clear , Bases- Pink
Litmus Paper
Acids always red, bases always blue, neutral doesnt change
Hydrogen ion concentration is 1*10^-13 what is the pOH
pH=13, pOH=1
The amount of acid or base you can add to a buffered solution before the pH changes drastically
Bronsted Lowery Acids and Bases
Acids- Proton Donor (hydrogen ion)
Base- Proton Acceptor
Conjugate Base- product formed when acid donates a proton
Conjugate Acid- product formed when base accepts a proton
If the hydroxide concentration is 2*10^-12, what is the pH
pOH = 11.69, pH=2.31
What is an indicator and what causes its color to change
an indicator is something that changes colors based on if it is in an acidic or basic solution. They are always weak acids or weak bases themselves and they change color by dissociating into ions (giving off the hydrogens or hydroxide)
If the [H+] = 1*10^-3 what is the Kw
Big Ka vs small Ka
Big Kb vs small Kb
Big Ka= strong acid
Big Kb= strong base
Little Ka= weak acid
Little Kb= weak base
Ka* Kb= Kw
Acid Dissociation Constant
ratio of the concentration of the dissociated to the undissociated form
If the [OH-] = 2.3*10^-2 , what is the [H+] , what is the pH?
[H+]=4.34*10^-13, pH=12.36
pOH=1.64 , pH=12.36 , [H+] = 10^-12.36=4.34 *10^-13
Lewis Acids and Bases
Lewis Acid- Electron pair acceptor
Lewis Base- Electron pair donor
In a titration if 10 mL of HCl are titrated with 20 mL of 0.1M NaOH, what is the molarity of the acid?
M1V1=M2V2
x(10)=(0.1)(20)
x=0.2
In a 0.1M solution of ethanoic acid [H+]= 1.34 *10^-3 , what is the Ka value
1.79 *10^-5