Acids and Bases, pH

Definitions

100

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)

200

Formula for hydrogen ion

H+

300

Arrhenius Acids and Bases 

Acids- produces H+ ions in water

Bases- produces OH- ions in water

400

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

500

Acid Dissociation Constant

ratio of the concentration of the dissociated to the undissociated form 

Calculations

100

What is pH and how is it related to concentration of [H+]

-log[H+] 

higher [H+]= lower pH= Acid

Lower [H+] = higher pH= Basic

200

If the [H+] = 1*10^-1, what is the [OH-]

1 *10^-13 M

300

If hydroxide concentration is 1*10^-12 M what is the pH

pOH=12 , pH =2

400

If the hydroxide concentration is 2*10^-12, what is the pH

pOH = 11.69, pH=2.31

500

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

More Defintions

100

pH less than 7, equal to 7, and greater than 7

less= Acid, More=basic, equal to 7 is neutral

200

The lab process of adding a known amount of solution of known concentration to determine the concentration of another solution

Titration

300

Compare and contrast Acids and Bases in different indicators

pH / Universal  (ROYGBV)

Acids- Red,  Bases- Blue , Neutral-Green

Phenolphthalein

Acids/ Neutral- Clear , Bases- Pink 

Litmus Paper

Acids always red, bases always blue, neutral doesnt change

400

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)

500

Lewis Acids and Bases 

Lewis Acid- Electron pair acceptor 

Lewis Base- Electron pair donor

Calculatios

100

If the [OH-] = 1*10^-11, what is the [H+]

1*10^-3

200

If pH=7 , what is the [H+]

1 *10^-7

300

Hydrogen ion concentration is 1*10^-13 what is the pOH

pH=13, pOH=1

400

If the [H+] = 1*10^-3 what is the Kw

Kw is a constant, it never changes it is the ion product constant for water and will always be 1*10^-14 regardless of the concentration of [H+] and [OH-] , as the product remains the same

500

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 

Ka and Buffer

100

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)

200

What does a buffer do

Resist change in pH when small amounts of acid or base are added

300

Buffer Capacity

The amount of acid or base you can add to a buffered solution before the pH changes drastically 

400

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

500

In a 0.1M solution of ethanoic acid [H+]= 1.34 *10^-3 , what is the Ka value

1.79 *10^-5