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Chem 115 > Chapter 5- Acids and Bases > Flashcards

Chapter 5- Acids and Bases Flashcards

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1
Q

What are the properties of acids compared to bases?

A

Acids- sour, dissolve metals, neutralize bases

Bases- bitter, slippery, neutralize acids

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2
Q

What are alkaloids?

A

Organic bases found in plants that are often poisonous

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3
Q

What is the Arrhenius definition of acids and bases?

A

Acid: a substance that produces H+ ions in aqueous solution
Base: a substance that produces OH- ions in aqueous solution

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4
Q

What is the brønsted-Lowry definition of acids and bases?

A

Acid: proton (H+ ion) donor
Base: proton (H+ ion) acceptor

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5
Q

What does amphoteric mean?

A

Substances that can act as acids and bases

Brønsted-lowry definition is amphoteric

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6
Q

What is a conjugate acid and a conjugate base?

A

Conjugate acid: the product that receives an H+ (ion) (it is the base with an extra H)
Conjugate base: the product that loses an H+ (ion) (it is the acid with a taken away H)

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7
Q

What is a strong electrolyte compared to a weak electrolyte?
What about acids?
What about bases?

A

Strong electrolyte- completely dissociates into ions in solution
Weak electrolyte- only partially dissociates
Strong acid- completely ionizes in solution
Weak acid- only partially ionizes
Strong base- completely dissociates in solution
Weak base- only partially dissociates

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8
Q

What are the 6 strong acids?

A 
HCl- hydrochloric acid
HBr- hydrobromic acid
HI- hydroiodic acid
HNO3- Nitric Acid
HClO4- Perchloric acid
H2SO4- Sulfuric acid
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9
Q

The stronger the acid, the _________ the conjugate base.

A

Weaker

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10
Q

What do HA and A- symbolize?

A

HA- acid

A- - conjugate acid

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11
Q

What is the acid ionization constant (Ka)?

A

Same formula as all K’s just doesn’t include H2O in reactants
FOR ACIDS
Kb is for bases

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12
Q

What is autoionization?

What is it’s constant?

A

When water acts as a base and an acid and can react with itself

Has an ion product constant for water (Kw) instead of Ka
Which always equals 1.0x10^-14

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13
Q

How do you know an acidic solution is acidic?

What about a basic solution?

A

Acidic- [H3O+] > [OH-]
pH < 7

Basic- [OH-] > [H3O+]
pH > 7

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14
Q

If [H3O+] goes up, what does Ka, pH, pKa?

A

Ka goes up
pH goes down
pKa goes down

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15
Q

What is the formula for finding pH?
pOH?
pKa?

A 
pH= -log[H3O+]
pOH= -log[OH-]
pKa= -logKa

pH+pOH=14.00

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16
Q

Is the concentration of H+ equal to the concentration of the strong acid in a strong acid solution?

A

Yes

17
Q

How do you solve a questions with weak acids concentrations given? (Since the weak acids concentration does not equal H3O’s concentration)

A

You create an ICE table and then solve for x by searching up the Ka and creating an equation
(Use small x approximation)

18
Q

How do you find the percent ionization of a weak acid?

NM

A

Percent ionization= concentration of ionized acid (usually x) / initial concentration of acid
All multiplied by 100

[H3O+] (equilibrium) / HA (x100)

19
Q

How is the percent ionization of a weak acid affected by the concentration of the acid?

A

The percent ionization of a weak acid decreases with increasing concentration of the acid

20
Q

What are the 6 strong bases?

A 
LiOH- lithium hydroxide
NaOH- sodium hydroxide
KOH- potassium hydroxide
Sr(OH)2- strontium hydroxide
Ca(OH)2- calcium hydroxide
Ba(OH)2- barium hydroxide
21
Q

What is Cl- the conjugate base of?
What about F-?
What about NO3-?

A

Cl- HCl
F- HF
NO3- HNO3

Anion A- is the conjugate base of acid HA

22
Q

What is an anion what is the conjugate base of a weak acid?

A

A weak base

25
Q

What is the pH of the anions (conjugate base) of a strong acid?

A

They are pH neutral so neither acidic or basic

26
Q

What type of pH (acidic, basic neutral) can salts form?

A

They came form acidic, basic, or neutral solutions when dissolved in water since they contain a cation and an anion

27
Q

What are the four possibilities in salts pH of the solution?
(Chart on page 285)
(NM)

A
  1. Salts where neither the cation or the anion act as an acid or base form pH neutral (cation is counterion of strong base, anion is conjugate base of strong acid) not equilibrium
  2. Salts where cation does not act as an acid and the anion act as a base form basic solution
    (Cation is counterion of strong base, anion is conjugate base of weak acid) NaHCO3
  3. Salts where the cation acts as an acid and the anion does not act as a base form acidic solution (cation is conjugate acid of weak base or metal ion, anion is conjugate base of strong acid) NH4Cl
  4. Salts where cation acts as acid and anion acts as base form solutions in which the pH depends of strengths of acid and base (cation is conjugate acid of weak base or metal ion, anion is conjugate base of a weak acid)
28
Q

What is the Lewis model of acids and bases?

A

Lewis acid: electron pair acceptor (has empty orbital or rearranges to create empty orbital so it can accept electron pair)
Lewis base: electron pair donor

29
Q

What is the equation connecting Ka, Kb, Kw?

A

Ka x Kb = Kw

30
Q

What are the three sections cations are divided into when considering them as weak acids?
(NM)

A

Cations that are counterions of strong bases- (one of the 6 strong bases) pH neutral
Cations that are the conjugate of weak bases- NH4+ to NH3, weak acid
Cations that are small, highly charged metals- Al Fe, weakly acidic solutions

31
Q

What does pKa affect the strength of a base and an acid?

A

Base- stronger

Acid- weaker

32
Q

How do the equations differ for weak acids/bases and strong acids/bases?

A

Weak- add water to weak acid/base then add OH- or H3O+ as product
Strong- it is just the strong base or acid dissociating or ionizing into the OH- or H3O+ and it’s by-product

33
Q

How do sig figs work with logs?

A

However many sig figs are in the log calculation are how many decimal places after the decimal in the answer

34
Q

When do you classify a salt as pH neutral?

A

If the anion and cation are both from strong acids and bases
Ex: NaCl
Ca(NO3)2

35
Q

When do you classify a salt as basic?

A

Where the cation is from a strong base but the anion is from a weak acid
Ex: NaF
KNO2

36
Q

When do you classify a salt as acidic?

A

Where the cations are from weak bases and is small highly charged metal atom (conjugate acids of weak bases) and the anions are from strong acids
Ex: FeCl3
Al(NO3)3
NH4Br

37
Q

When do you classify a salt as a pH that is dependant on relative strengths?

A

When the cation is from a weak base or a highly charged metal ion and the anion is from a weak acid

Chem 115 (8 decks)

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