Chem chapter 16 Flashcards
Strong bases
Groups 1 and 2 hydroxides on Periodic table
Dissociate fully into water (goes from all HF to All H+ and F-)
Strong Base Kb is much larger than 1
Weak Base Kb is much smaller than 1
Acids
Lose H+ (in an ice chart subtract one H from, the solution)
Likely to have an H at the front of the Formula
Ex: HCl
Anything that loses H+ is a proton donor or Acid
PAY ATTENTION TO IF IT GAINS OR LOSES H+
Bases
Gain H+ (in ice chart add one H+ to solution)
Likely to have OH in it but not certain
Anything that reveives an H+ is a base
Ex: H3->H4
PAY ATTENTION TO IF IT GAINS OR LOSES H+
Brønsted Lowry Acids
A substance that donates and H+ in a reaction
Brønsted Lowry Bases
Receives an H+ in Solution
BL base SO3 2- would become HSO3- (loses one of the minuses)
Strong Acids Definition
Dissociate fully into water (goes from all HF to All H+ and F-)
Strong Base Ka is much larger than 1
Weak Base Ka is much smaller than 1
Strong Acids to Memorize
HCL - Hydrochloric acid
HBr - Hydrobromic acid
HI - Hydroiodic acid
HNO3 - Nitric acid
H2SO4 - Sulfuric acid
HClO3 - Chloric acid
HClO4 - Perchloric acid
In ICE charts
Weak acids/bases - ICE chart with x (only breaks down some)
Strong acids/bases - Change is the PH (all breaks down)
Buffer Definition
A solution that can resist pH change upon addition of acidic or basic components
Can neutralize small amounts of acids and bases to maintain stable pH solution
Buffers must include
A weak acid and its conjugate base
OR
A weak base and its conjugate acid
When looking at salts (buffers)
Can ignore alkaline metals
Why dont Strong Acid/Conjugate Bases work (buffers) - HCl <— —> H+ + Cl-
A buffer made of HCL and NaCl
If H+ is added Cl- is unable to combine with it (HCl would immediately break down
If OH- is added it would neutralize some H+ and there is no source to replace it
Buffered against Bases
HF <– –> H+ + F-
Some base (OH-) is introduced the H+ reacts with all of it
THe H+ originally in the buffer has been neutralized to water
To replace the lost H+ some of the HF dissociates THe pH still increases but only slightly
Buffered against Acids - HF <— —> H+ + F-
Some acid (H+) is introduced to the buffer solution
The F- (a base) reacts with much of the added H+
The pH will still drop but only slightly
Arrhenius
An Arrhenius acid is any species that increases the concentration of in aqueous solution.
An Arrhenius base is any species that increases the concentration of in aqueous solution.