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A Level Chemistry Ocr > Module 2 Chapter 4 (part 1) > Flashcards

Module 2 Chapter 4 (part 1) Flashcards

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1
Q

What do all acids contain in there formula

A

They all contain hydrogen in their formulae

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2
Q

What happens when acids are dissolved in water

A

They release H+ ions into the water

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3
Q

What is the Bronstead Lowry definition of an acid

A

They are proton donors

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4
Q

What is the formula of ethanoic acid

A

CH3COOH

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5
Q

What is a strong acid

A

A strong acid completely disassociates when dissolved in water. All molecules release H+ ions

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6
Q

What is a weak acid

A

A weak acid partially dissociates when dissolved in water. Only a small proportion of the molecules release H+ ions.

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7
Q

What happens to the H+ ions released

A

The H+ ion will then join with a water molecule making a hydroxenium ion.

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8
Q

What is the equation for a hydroxenium ion forming

A

H+ (aq) + H2O (l) <-> H3O +

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9
Q

What happens when the acid is stronger

A

The more free H+ ions are released into solution. The greater the number of free H+ ions.

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10
Q

What does a greater number of H+ ions in the solution mean

A

It means that the PH value of the acid will be lower.

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11
Q

What are most organic acids

A

They are weak acids

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12
Q

What is the definition of a base

A

A base neutralises an acid to form a salt

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13
Q

What is the definition of an alkali

A

An alkali is a soluble base that releases OH- ions into solution.

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14
Q

what happens in a neutralisation reaction

A

H+ ions react with a base to form a slat and water.

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15
Q

What is the ionic equation for all neutralisation reactions

A

H+ + OH- -> H2O

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16
Q

What is the word equation for an acid and base

A

Acid + base -> salt + water

17
Q

What is the work equation for an acid and base

A

Acid + base -> salt + water

18
Q

What is the word equation for an acid and alkali reacting

A

Acid + alkali -> salt + water

19
Q

What is the word equation for an acid and metal reacting

A

Acid + metal -> salt + hydrogen

20
Q

What is the word equation for an acid reacting with a carbonate

A

Acid + carbonate -> salt + water + carbon dioxide

21
Q

what do you call a salt made form hydrochloric acid

A
  • Chloride
22
Q

what do you call a salt made form sulphuric acid

A

Sulfate

23
Q

what do you call a salt made form nitric acid

A
  • Nitrate
24
Q

what do you call a salt made form ethanoic acid

A

Ethanoate

25
Q

What is the ethanoate ion

A

CH3COO +

26
Q

What happens when an acid is neutralised by metal oxides and hydroxides

A

Only a salt and water is formed

27
Q

What is a titration used for

A

Finding the concentration for a solution
Identification of unknown chemicals
Finding the purity of substances - important for quality control in pharmaceutics

28
Q

What is a standard solution

A

A solution of a known concentration

29
Q

What is the titre volume

A

The minimum volume of solution needed to reach the end point in a titration

30
Q

How do you make a standard solution (1-3)

A

1) The solid is weighed accurately
2) The solid is dissolved in a. Beaker using less distilled water than will be needed to fill the volumetric flask to the mark
3) Solution transferred to a volumetric flask. The last traces of solution are rinsed into the flask with distilled water

31
Q

What is steps 4-5 of making a standard solution

A

4) Flask is carefully filled to the graduation line by adding distilled water a drop at a time until the bottom of meniscuses lines exactly up with the mark at eye level
5) Slowly invert the volumetric flask several times to mix the solution this step is important for consistency.

32
Q

What are two possible errors that can occur when making a standard solution

A
  1. The flask is filled with water over the graduation line
  2. The flask is not inverted
33
Q

What are the first 4 steps when conducting a titration

A
  1. Use a volumetric pipette to measure the volume of standard solution into a conical flask
  2. Add the other solution into brunettes, record the initial burette reading to nearest +- 0.5cm cubed
  3. Add indicator to solution in conical flask
  4. Run the solution in burette into the solution in conical flask, swirling the flask as you do so mix the solutions together.
34
Q

What are the steps when doing a titration (5-8)

A

5) The end point is when the indicator changes colour. this indicates when the volume of one solution that exactly reacts with the volume of the second solution.
6) Record final burette reading. the difference is the titre volume
7) A quick run is done to get an approximation
8) Titration is repeated at least 3 or 2 times until two or more concordant readings are measured.

35
Q

What values do you choose for the mean titre

A

Only use your two closest titres

36
Q

What are concordant titre values

A

Within 0.10cm cubed of each other

A Level Chemistry Ocr (8 decks)

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