MCAT > Chemistry Chapter 10 > Flashcards

Chemistry Chapter 10 Flashcards

(48 cards)

Study These Flashcards
1
Q

What did Arrhenius acid or base mean

A

Acid meant something that disassociates to form excess H+
Bases means something that will disassociate to form excess OH-

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2
Q

Bronsted Lowry acid and bases meaning

A

Acid would donate a hydrogen ion

Bases would accept a hydorgen ion

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3
Q

Lewis’ acid and base meaning

A

Acid is the one electron pair acceptor

Base electron pair donor

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4
Q

Difference between bronsted lowry and Lewis definition of acids and bases

A

Bronsted Lowry is about protons

Lewis is about electrons

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5
Q

How do arrows face towards in Bronsted Lowry vs Lewis

A

Bronsted we do proton towards electron

Lewis we do electrons towards proton

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6
Q

What are amphoteric species

A

Species that acts like an acid in a base environment and acts like a base in an acid environment

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7
Q

What is the most common example of a amphoteric?

A

Water

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8
Q

difference between amphiprotic adn amphoteric

A

Amphiprotic is can give or accpet proton

Amphoteric is can act as an acid or base

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9
Q

If your anion ends in -ite, what will be your acid ending in

For example
Chlorite
Nitrite

A

Chlorous acid
Nitrous acid

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10
Q

If your anion ends in -ate, what will be your acid ending in

Nitrate sulfate

A

Nitric acid
Sulphuric acid

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11
Q

What is autoionization of water

A

It can react with itself to produce hydronium and hydroxide ion

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12
Q

Water dissociation constant so Kw is also what at 25 degrees

A

10^-14

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13
Q

Kw can only be changed if what is changed

A

Temperature

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14
Q

If temperature increases , does Kw increase or decrease

A

Increases

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15
Q

How do you calculate pH and pOH

A

PH = -log (H+) = log (1/H+)

POH = -log (OH-) = log (1/OH-)

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16
Q

Pure water pH and pOH is

A

7

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17
Q

If Ph increases by a certain amount. What happens to pOH

A

It decreases by same amount

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18
Q

If concentration of H+ is 0.001
If concentration of H+ is 10^-3

What is pH. And pOH for each scenario above

A

Both are pH of 3, pOH of 11

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19
Q

If Kb is 1x10^-12,, then pKB is what

A

12

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20
Q

If the Ka of an acid is 1.8 x 10^-5. What is the Pka

Study These Flashcards
A

-log (1.8 x 10^-5)
= 5 log - 1.8
= 5 -0.18
= 4.82

21
Q

Do strong acids and bases or weak ones completely disassociate into their ions in aqueous solutions

22
Q

How do you know when you just have to log it or when you have to care about the water inside

Study These Flashcards
A

Firstly you need to ask, is the concentration of acid bigger than 10^-7, if yes then you just do pH= -log(acid)

If not then the pH is slightly less than 7

23
Q

What is the pH of a solution with HCLO4 concentration of 10M

Study These Flashcards
A

-log(10)

= -1

Cuz you move 10 by one decimal place

24
Q

The smaller the Ka, the stronger or weaker the acid

The smaller the Kb, the strong or weaker the base

25
What is classified as a weak acid or base in terms of their Ka and Kb values
Ka is less than 1 Kb is less than 1
26
Conjugate acid and conjugate bases Which one gains and which one loses a proton
Conjugate acids gains a proton Conjugate bases loses a proton
27
Do strong acids have strong or weak conjugate bases
Weak
28
Calculate the concentration of H3O+ in a 2M aqueous solution of CH3COOh Pka is 1.8 x 10^-5
Write the equation Know that it is [h30][Ch3COO-]/Ch3cooh = Pka Acetic acid is weak acid so its concentration is just wat the initial concentration is 2M-x X^2 /2-x = Pka Since x is super small, denominator is just 2 Then we calculate and get 6* 10*-3
29
How do you know when to use initial or just initial -X depending on acid and base strength
If strong acid or base then you just use x If weak acid or base then you use initial -x
30
Strong acid and strong base yield Waht type of salt and water
Neutral salt and water Ph=7
31
Strong acid and weak base yield what type of salt and water
Acidic salt and no water Ph is less than 7
32
Weak acid and strong base yield what
PH will be in basic range Basic Salt and water
33
What does weak acid and weak base yield
Depends on relative strength of reactants
34
What species are considered the equivalent for acid and basis?
Moles of h+ Moles of OH-
35
Calculate the normality of 2M of Al(OH)3
2 times Oh number so 6
36
Calculate normality of 16M of H2SO4
16 M times 2 = 32 M
37
What are titrations
You add known volume of titrant to unknown volume of titrand until the reaction completes at equivalence point
38
What doles it mean when some acids and bases are polyvalent
Each mole of acid or base liberates more than acid and base equivalent
39
Indicators change colours when they shift between what
Conjugate acid adn base forms
40
If asked to pick which indicators to use for a titration what o you do
You end to know the pH,. Then find the closest Pka value to it and that’s the one you pick
41
How do you calculate pH is given Pka How do you calculate pOH if given PKB
Ph= PKA + log [product concentration]/[reactant concentration] Same for pOH
42
Equivalence point pH if they are Strong acid weak base Strong acid strong base Weak acid strong base
Lower than 7 Equal to 7 Higher than 7
43
During titration, how should i tell difference between the graphs of, strong acids vs strong base, strong acids weak base and weak acids strong base
Look at starting pH, that is the titrand See equivalence point area, if its at 7, its strong acid strong base. If it’s higher or lower, then you know if its stronger acid or strong base reacting in the equation. Because it will pull the curve towards more of its pH territory
44
How is buffer solution made
Weak acid and its salt or weak base and its salt
45
2 buffers on Mcat And are they acid or base buffers
Acetic acid and soidum acetate - acid buffer Ammonia and ammonium chloride - base buffer
46
What is the pH of a solution made from 1L of 0.05M acetic acid (Ka= 1.8 x10^-5) mixed with 500mL of 1M acetate (CH3COO-)
First find concentration of acetic acid and acetate Acetic acid = NVintiial = NV final= 0.033 Acetate= 0.33 Then we use equation to calculate pH Ph= Pka + log (concentration of acetate/ concentration of acetic acid ) PH= -log (1.8*10^-5) + log (0.033/0.33) PH = 4.8 +1 PH=5.8
47
When is the buffering region Half equivalence point Equivalence point Endpoint on graph
Buffering region : flattest portion of titration curve Half equivalence is the centre of the buffering region Equivalent point: steepest part of the curve where acid and base are equal Endpoint : the last point where indicator turns its final colour
48
What is the point of buffer solution
To resist pH changes
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