Unit 3: Chapter 6 - Acids and Bases Flashcards

1
Q

Empirical Properties of Strong Bases

A

Very high pH&raquo_space;7
High conductivity
Fast reaction rate

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2
Q

Empirical Properties of Weak Bases

A

Medium to high pH >7
Low conductivity (only if molecular)
Slow reaction rate

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3
Q

Modified Arrhenius Theory: Strong Acids

A

Completely react with water to form aqueous H3O+ ions (100%)

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4
Q

Modified Arrhenius Theory: Weak Acids

A

Partially react with water to form H3O+ ions (50%)

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5
Q

Modified Arrhenius Theory: Strong Bases

A

Completely dissociate to form OH- ions (100%)

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6
Q

Modified Arrhenius Theory: Weak Bases

A

Partially react with water to form OH- ions (50%)

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7
Q

Define: Monoprotic Acids

A

Acid with only one hydrogen atom and only react once to produce H3O+ ions

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8
Q

Define: Polyprotic Acids

A

Acids that contain more than one acidic hydrogen and react more than once with water to form H3O+ ions

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9
Q

Exemption to Polyprotic Acid Rule

A

Sulfuric Acid - Because the first reaction with water is essentially complete and the second is 50%

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10
Q

Modified Arrhenius Theory: Acids

A

Substance that react with water to produce hydronium ions

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11
Q

Modified Arrhenius Theory: Bases

A

Substance that react with water to produce hydroxide ions

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12
Q

Modified Arrhenius Theory: Neutralization

A

The reaction between hydronium and hydroxide to produce water

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13
Q

What’s the relationship between the pH and pOH and the ion concentration?

A

Inverse relationship

The higher hydronium ion concentration , the lower the pH

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14
Q

pH and pOH sig dig rule

A

Digits following the decimal point = sig digs

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15
Q

Hydronium concentration for neutral solution at SATP

A

1x10 -7 mol/L

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16
Q

Hydronium concentration for acidic solution

A

> 1x10 -7 mol/L

17
Q

Arrhenius’ Theory: Acids

A

Acids ionize with water to produce a hydrogen ion and an anion

18
Q

Arrhenius’ Theory: Bases

A

Bases are soluble ionic compounds that dissociate into a cation and a hydroxide ion

19
Q

pH Formulas

A

pH = -log [H3O+(aq)]

[H3O+(aq)] = 10 -pH

20
Q

pOH Formulas

A

pOH = -log [OH- (aq)]

[OH- (aq)] = 10 - pOH

21
Q

What’s an acid-base indicator?

A

Substances that change colour when the acidity of the solution changes

22
Q

Lower pH form of Indicator

A

HIn (aq)

23
Q

High pH form of Indicator

A

In- (aq)

24
Q

Empirical Properties of Weak Acids

A

Medium to low pH

24
Q

Empirical Properties of Acids In General

A

Taste sour
Turn blue litmus red
Have pH

24
Q

Empirical Properties of Bases in General

A
Taste bitter
Feel slippery 
Turn red litmus blue 
Have pH >7
Neutralize acids
24
Q

General Polyprotic Acid and Base Rule

A

Polyprotic bases and acids are weak, as each reaction with water causes their strength to decrease with each successive step

24
Q

Define: Amphiprotic

A

A substance that can become either an acid or a base (usually containing a negatively charged ion starting with H)