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Chemistry > Acids And Bases > Flashcards

Acids And Bases Flashcards

0
Q

What is a Brønsted-Lowry base?

A

Proton (H+) acceptor

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1
Q

What is a Brønsted-Lowry acid

A

Proton (H+) donor

HCl

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2
Q

What is a Lewis acid?

A

Electron pair acceptor

NH3

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3
Q

What is a Lewis base?

A

Electron pair donor

Cu2+

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4
Q

Are all Brønsted-Lowry acids Lewis acids?

A

Yes

Lewis acids do not have proton transfer

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5
Q

Litmus in acid and alkali

A

Acid - pink

Alkali-blue

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6
Q

Methyl orange color in acid and base

A

Acid-red

Alkali-yellow

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7
Q

Phenolphthalein colour in acids and alkali

A

Acid-colourless

Alkali-pink

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8
Q

What is a base?

A

Substance that accepts H+

Metal oxides/hydroxides
Ammonia
Soluble carbonates/ hydrogen carbonates

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9
Q

What is an alkali ?

A

Alkalis form OH- ions

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10
Q

Acid + metal –>

A

Acid + metal –> salt + hydrogen

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11
Q

Acid + base –>

A

Acid + vase –> salt + water

Neutralization reaction

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12
Q

Acid + carbonate –>

A

Acid + carbonate –> salt + water + carbon dioxide

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13
Q

How to distinguish between strong and weak acids and bases

3 ways

A

Electrical conductivity
Strong high

Rate of reaction

pH

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14
Q

Weak acids

A

Ethanoic (organic)

Carbonic (H2CO3)

Phosphoric (H3PO4)

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15
Q

Strong acids

A

Hydrochloric

Nitric (HNO3)

Sulfuric

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16
Q

Strong bases

A

Li/Na/K/Ba hydroxide

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17
Q

Weak acids

A

Ammonia

Ethylamine

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18
Q

How difference between strong and weak acids?

A

Strong acids/bases- almost complete dissociation in solution

Weak-partially dissociate in solution

19
Q

What is a change in 1 pH in H+?

20
Q

pH =

A

pH= - log [H+]

H+ = 10^-pH

21
Q

What is Kw?

A

Ionic product constant of water

Kc [H2O] = [ H+] [OH-]

22
Q

What affects KW?

A

Temperature dependent (equilibrium constant)

Increase temperature increases kW

  • more dissociation
  • endothermic
23
Q

Find H+ of pure water

A

H+ = square root KW

24
Q

At 25c

Find pOH knowing pH

A

pH + pOH = 14

25
Q

Find pH from pKw

A

pH + pOH = pKw

26
Q

What is Ka?

A

Ka = [H3O+] [A-] / [HA]

Concentration of ions/ dissociation
-acid dissociation constant

27
Q

What affects Ka?

A
  • temperature

- acid

28
Q

What is Kb?

A

Kb = [BH+] [OH-] / [B]

Base dissociation constant

29
Q

What is a larger pKa?

A

Weaker acid

30
Q

Relationship between acid and conjugate base

A

Strong acid = weak conjugate base

31
Q

Organize acid strong to weak:

32
Q

What is a buffer solution?

A

Resistant to change in pH

When adding a Small amounts if acid/alkali

33
Q

Composition of acidic buffers

A

Weak acid (ch3cooh)

Salt of weak acid+strong alkali (Nach3coo)
Fully Dissociates to CH3COO-

34
Q

What happens in acidic buffer adding H+

A

Reacts with base

H+ + CH3COO- CH3COOH

35
Q

What happens add OH- in acidic buffer?

A

OH- reacts with acid

CH3COOH + OH- CH3COO- + H2O

36
Q

Composition of basic buffer?

A

Weak base (NH3)

Salt of weak base+strong acid (NH4Cl)
Fully dissociates to NH4+

37
Q

Determine pH of buddy solution

A

Bffbdbgddb

38
Q

Find pH

A

pH =pKa + log[salt]/[acid]

39
Q

In buffer when does pH=pKa and pOH=pKb

A

[acid]=[salt]

[base]=[salt]

40
Q

How to make buffer

41
Q

Factors affect buffers

A

Temperature - change Ka/ kb, changes pH

Not dilution- not change pH but buffer capacity

42
Q

What is the equivalence point ?

A

In titration
Stoichiometrically equivalent amount avid and base

Salt and water only

43
Q

Strong acid and base

A

Equivalence - 7

Initial pH 1
PH changes gradually to equivalence
Ph jump 3-11 at equivalence
Curve flattens at high pH

44
Q

Weak acid strong base

A

Equivalence - >7

Initial pH girly high 3
Stays constant until equivalence
Jump form 7-11 at equivalence
Curve flattens at high pH 13

Chemistry (3 decks)

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