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Chemistry 110 > (Ch.14) Acids & Bases > Flashcards

(Ch.14) Acids & Bases Flashcards

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1
Q

What are the two primary definitions of Acids & Bases?

A
  1. The Arrhenius Definition
  2. The Bronsted-Lowry Definition
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2
Q

How does Arrhenius define acids and bases?

A
  1. An acid produces H+ ions in an aqueous solution.
  2. A base produces OH- ions in an aqueous solution.
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3
Q

How does Brownsted-Lowry define acids and bases?

A
  1. An acid is a proton donor.
    (H+ ion donor)
  2. A base is a proton acceptor.
    (H+ ion acceptor)
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4
Q

What does it mean to be Amphoteric?

A

An amphoteric substance is a substance that can act as both an acid and a base. All conjugate acid-base pairs are amphoteric.

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5
Q

What are Conjugate Acid-Base pairs?

A

These are acid-base pairs that are, firstly, amphoteric, and secondly, they differ by one proton.

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6
Q

What is a Neutralization Reaction?

A

A reaction between an acid and a base.

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7
Q

What forms when:
1. Metal + Acid
2. Metal Oxide + Acid

A
  1. Gas + Salt
  2. Water + Salt
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8
Q
  1. What is a Strong Acid?
  2. What is a Weak Acid?
A
  1. An acid that completely ionizes in a solution.
  2. An acid that does not completely ionize in a solution.
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9
Q

How can you tell the difference between a Strong and Weak acid?

A

A weak acid is usually found in a reversible equation.
Strong Acids: HCl, HBr, HI, HNO3, NClO4, H2SO4

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10
Q

What is a Dissociation Reaction?
What is an Ionization Reaction?
How are they different?

A
  1. The separating of charged particles that already exist.
  2. Producing newly charged particles.
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11
Q
  1. What is a Strong Base?
  2. What is a Weak Base?
A
  1. A base that completely dissociates in a solution.
  2. A base that does not completely ionize in a solution.
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12
Q

How can you determine the difference between a Weak or Strong Base?

A

If the base starts with any element from the first two columns of the periodic chart- it is STRONG.

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13
Q

EX.
Determine the concentration of OH- in the following base solutions.
1. 0.25 M NaOH
2. 0.25 M NH3
3. 0.25 M Sr(OH)2
4. 1.25 M KOH

A
  1. [OH-]= 0.25 M (strong base)
  2. [OH-]< 0.25 M (weak base)
  3. [OH-]= 0.50 M (strong base & 2 OH-)
  4. [OH-]= 1.25 M (strong base)
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14
Q

EX.
Determine the concentration of H3O+ in each of the following acid solutions.
1. 0.50 M HCHO2
2. 1.25 M HI
3. 0.75 M HF

A
  1. [H30+]< 0.50 M (weak acid)
  2. [H30+]= 1.25 M (strong acid)
  3. [H30+]< 0.75 M (weak acid)
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15
Q

What do we mean when we say water is capable of Self-Ionization?

A

Water can be both a base and an acid and can react with itself to form low concentrations of the ions OH—and H3O+.

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16
Q

What is the ion product constant for water?

A

Kw= 1.0 (10^-14) at 25 degrees Celsius

17
Q

What is a:
1. Neutral Solution
2. Acidic Solution
3. Basic Solution

A
  1. The ion product for both OH- and H3O+ is equal to 1.0 (10^-7)
  2. There is more H3O+ product than OH-.
  3. There is more OH- product than H3O+.
18
Q

How do you calculate H3O+ concentration from pH?
How do you calculate pH from H30+ concentration?

A
  1. H30+ = 10^(-pH)
  2. pH= -log(H30+)
19
Q

How do you determine the concentration of [H30+] given [OH-] or [OH-] given [H30+]?

A
  1. Use the solution:
    [OH-][H30+]= 1.0 (10^-14)
20
Q

Describe the pH scale.
Describe the pOH scale.

A
  1. (pH):
    1-6.9 is acidic, 7 is neutral, 7.1-14 is basic
  2. (pOH):
    1-6.9 is basic, 7 is neutral, 7.1-14 is acidic
21
Q

How would you calculate the [OH-] or [H30+] concentration given a solution’s pOH?

A

[OH-]= 10^-pOH

22
Q

How would you calculate pOH given the [OH-] or [H3O+] concentration?

A
  1. pOH= -log[OH-]
  2. Determine [OH-] concentration from [H30+], then run it through the above equation to find pOH.
23
Q

How would you determine the pH of a solution given the pOH? The pOH given the pH?

A
  1. The same, using the equation:
    pH+pOH=14.00
24
Q

What is:
1. pH =
2. pOH =
3. [H30+] =
4. [OH-] =

A
  1. -log[H30+]
  2. -log[OH-]
  3. 10(^-pH)
  4. 10(^-pOH)
25
Q

What is:
1. pH+ pOH=
2. [H30+] + [OH-]=

A
  1. 14.00
  2. 1.0(10^-14)

Chemistry 110 (15 decks)

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