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CHEMISTRY as - ocr a > Chapter 4 > Flashcards

Chapter 4 Flashcards

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1
Q

What are strong acids

A

Releases all of its hydrogen atoms into a solution as h+ ions and completely disassociates in aqueous solution

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2
Q

Common acids formulas

Hydrochloric acid
Sulfuric acid
Nitric acid
Ethanoic acid

A

HCl
H2SO4
HNO3
CH3COOH

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3
Q

What are weak acids

A

Only releases a small proportion of its available hydrogen atoms into solution as H+ ions, and partially dissociates in aqueous solution

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4
Q

What is a base

A

A base can neutralise an acid to form a salt

NH3

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5
Q

What is an alkali

A

A base that dissolved in water

Releasing hydroxide ions OH- into the solution

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6
Q

Neutralisation equation

A

Acid (aq) + metal oxide/hydroxide (s) —> salt (aq) + water (l)

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7
Q

Acid (aq) + alkali (aq) —>

A

Salt (aq) + water (l)

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8
Q

Acid + carbonate (s) —>

A

Co2 (g) + H2O (l) + salt (aq)

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9
Q

What are titrations

A

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

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10
Q

What are titrations useful for

A

Finding the concentration of a solution

Identifying an unknown solution

Finding the purity of a substance

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11
Q

How to prepare standard solutions

A
  • solid is weighed
  • solid is dissolved using less distilled water than needed to fill the volumetric flask
  • solution is transferred to volumetric flask
  • remaining solution is rinsed into flask with more distilled water
  • more distilled water is added drop-wise to reach meniscus
  • flask is slowly inverted to make sure the solution is mixed
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12
Q

Acid base titration procedure

A
  • add a measured volume of 1 solution to a conical flask
  • add other solution to burette, record initial reading (0.05)
  • add indicator
  • when the indicator changes colour at the end point stop the tap
  • record final burette reading
  • calculate titre by subtracting initial from final
  • further titrations are carried out until titres are concordant (0.1)
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13
Q

Oxidation number definition

A

A measure of the number of electrons an atom uses to bond with atoms of another element

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14
Q

Special cases of oxidation number

H - metal hydrides (NaH)

O - peroxide’s (H2O2)

O - F (F2O)

A

H = -1

O = -1

O = +2

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15
Q

Redox reactions

A

Involves reduction and oxidation

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16
Q

Metal + acid (aq) —>

A

Salt + hydrogen

CHEMISTRY as - ocr a (15 decks)

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