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Chemistry > Chapter 4 Acids and Redox > Flashcards

Chapter 4 Acids and Redox Flashcards

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1
Q

What is an Acid

A
  • Contain Hydrogen
  • PH<7
  • Release H⁺ ions into the solution when dissolved in water
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2
Q

Show Hydrochloric Acid dissociating in water

A

HCl → H⁺₍ₐᵩ₎ + Cl⁻ ₍ₐᵩ₎

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3
Q

What is a strong acid

A

A strong acid completely dissociated in an aqueous solution

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4
Q

What is a weak acid

A

A weak acid partially dissociates in an aqueous solution

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5
Q

Name 2 strong acids

A

Hydrochloric Acid
Nitric Acid

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6
Q

Name a weak acid

A

Ethanoic Acid

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7
Q

What is the formula for Hydrochloric Acid

A

HCl

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8
Q

What is the formula for Sulfuric Acid

A

H₂SO₄

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9
Q

What is the formula for Nitric Acid

A

HNO₃

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10
Q

What is the formula for Ethanoic Acid

A

CH₃COOH

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11
Q

Show Ethanoic Acid dissociating (partially) in an aqueous solution

A

CH₃COOH₍ₐᵩ₎ ⇌ H⁺₍ₐᵩ₎ + CH₃COO⁻₍ₐᵩ₎

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12
Q

How does Sulphuric Acid behave

A

Dissociation happens in 2 steps

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13
Q

Show the dissociation of Sulfuric Acid

A
  • First behaves like a strong acid
    H₂SO₄₍ₐᵩ₎ → H⁺₍ₐᵩ₎ + HSO₄⁻₍ₐᵩ₎
  • Then the HSO4- ions behave as a weak acid
    HSO₄⁻₍ₐᵩ₎ ⇌ H⁺₍ₐᵩ₎ + SO₄²⁻₍ₐᵩ₎
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14
Q

What is a base

A

A base neutraises an acid to form a salt

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15
Q

Give examples of bases

Generic

A
  • Metal Oxides
  • Metal Carbonates
  • Metal Hydroxides
  • Alkalis
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16
Q

What is an Alkali

A

An Alkali is a base that dissolves in water releasing OH⁻ ions

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17
Q

Acid + Alkali →

A

Salt + Water

18
Q

HCl₍ₐᵩ₎ + NaOH₍ₐᵩ₎ →

Acid + Alkali

A

NaCl₍ₐᵩ₎ + H₂O₍ₗ₎

19
Q

Ionic equation of
HCl₍ₐᵩ₎ + NaOH₍ₐᵩ₎ → NaCl₍ₐᵩ₎ + H₂O₍ₗ₎

A

H⁺₍ₐᵩ₎ + OH⁻₍ₐᵩ₎ → H₂O₍ₗ₎

20
Q

Metal oxide/hydroxide + acid →

What is the observation

A

salt + water

Solid Metal Oxide Disappears

21
Q

Metal hydroxide + acid →

A

salt + water

22
Q

H₂SO₄₍ₐᵩ₎ + MgO₍ₛ₎ →

Acid + Metal Oxide

A

MgSO₄₍ₐᵩ₎ + H₂O

23
Q

Ammonia + Acid →

A

Ammonium salts containg an ammonium ion

24
Q

Carbonate + acid →

A

salt + water + carbon dioxide

25
Q

What is a titration

A

A technique used to accurately measure the volume of one solution that reacts exactly with another solution

26
Q

What are titrations used for

A
  • Finding the concentration of a solution
  • Identification of unknown chemicals
  • Finding the purity of a substance
27
Q

What are concordant results

A

Results within 0.10 cm^3 of each other

28
Q

Ammonia + Acid →

A

Salt containing an ammonium Ion

29
Q

How do you prepare a standard solution

(e.g. NaOH)

A
  1. Find mass of solid you want
  2. Dissolve solid in a beaker using less distilled water than needed
  3. Transfer to volumetric flask and rinse with distilled water
  4. Fill up to the graduation line with distilled water
  5. Invert the flask several times to mix
30
Q

Evplain the effect of adding too much distilled water to the standard solution

A

The solution will be too dilute

31
Q

What is a standard solution

A

A solution of known concentration

32
Q

What is the oxidation number for any element

A

0

33
Q

In a compound, what is the oxidation number for

Group 1 Elements

A

+1

34
Q

In a compound, what is the oxidation number for

Group 2 Elements

A

+2

35
Q

In a compound, what is the oxidation number for

F

Fluorine

A

-1

36
Q

In a compound, what is the oxidation number for

H

Hydrogen

A

+1
-1 in metal hydrides eg NaH or MgH₂

37
Q

In a compound, what is the oxidation number for

O

Oxygen

A

-2
-1 in Peroxides (H₂O₂)
+2 in Oxygendifluorides (OF₂)

38
Q

In a compound, what is the oxidation number for

Cl

Chlorine

A

-1
Except when combined with O or F

39
Q

What is the uncertainty of a burette?

A

0.05

40
Q

What do the roman numerals next to an element tell you

A

The oxidation number of the element

41
Q

What is a redox reaction

A

A reaction involving both reduction and oxidation

42
Q

Metal + Acid →

A

Salt + Hydrogen

Chemistry (16 decks)

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