Chem chapter 16 Flashcards

1
Q

Strong bases

A

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

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2
Q

Acids

A

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+

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3
Q

Bases

A

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+

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4
Q

Brønsted Lowry Acids

A

A substance that donates and H+ in a reaction

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5
Q

Brønsted Lowry Bases

A

Receives an H+ in Solution
BL base SO3 2- would become HSO3- (loses one of the minuses)

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6
Q

Strong Acids Definition

A

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

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7
Q

Strong Acids to Memorize

A

HCL - Hydrochloric acid
HBr - Hydrobromic acid
HI - Hydroiodic acid
HNO3 - Nitric acid
H2SO4 - Sulfuric acid
HClO3 - Chloric acid
HClO4 - Perchloric acid

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8
Q

In ICE charts

A

Weak acids/bases - ICE chart with x (only breaks down some)
Strong acids/bases - Change is the PH (all breaks down)

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9
Q

Buffer Definition

A

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

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10
Q

Buffers must include

A

A weak acid and its conjugate base
OR
A weak base and its conjugate acid

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11
Q

When looking at salts (buffers)

A

Can ignore alkaline metals

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12
Q

Why dont Strong Acid/Conjugate Bases work (buffers) - HCl <— —> H+ + Cl-

A

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

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13
Q

Buffered against Bases
HF <– –> H+ + F-

A

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

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14
Q

Buffered against Acids - HF <— —> H+ + F-

A

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

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15
Q

Arrhenius

A

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.

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16
Q

Molarity equation

A

M = Moles/Liter

17
Q

cooh whatever grouop

A

only

18
Q
A