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Chemistry > EL 9: How salty? > Flashcards

EL 9: How salty? Flashcards

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1
Q

What is an acid?

A

A compound that disassociates in water to produce hydrogen ions

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2
Q

What is a base?

A

A compound that reacts with an acid - is a proton acceptor - to produce water and a salt

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3
Q

What is neutralisation?

A

When an acid and alkali react and a salt is formed

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4
Q

What is an alkali?

A

A base that dissolves in water to produce hydroxide ions (OH-)

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5
Q

What is a salt?

A

Is a product of neutralisation (when a H+ of an acid is replaced by a metal ion)

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6
Q

What is a strong acid?

A

Fully dissociates in an aqueous solution

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7
Q

What is a weak acid?

A

Partially dissociates in an aqueous solution

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8
Q

What is a key property of the group 2 oxides and hydroxides?

A

They are bases, they react with acids to produce salts

Acid + Base = Salt + Water

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9
Q

What is the general definition of an acid?

A

A substance that donates H+ in a chemical reaction

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10
Q

What is the general definition of a base?

A

A substance that accepts the H+ in a chemical reaction

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11
Q

What do you need before you can start a titration?

A

A standard solution

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12
Q

What is a standard solution?

A

Any solution that you know the concentration of

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13
Q

What does an acid + metal carbonate =?

A

Salt + H2O + CO2

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14
Q

What does an acid + Metal =?

A

Salt + H2

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15
Q

What does an acid + Metal oxide =?

A

Salt + H2O

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16
Q

What does an acid + Metal hydroxide =?

A

Salt + H2O

17
Q

When making a standard solution must the bottom of the meniscus reach the line?

A

To make sure its accurate, you need to carry out every technique to the same level of precision

18
Q

When making a standard solution must you invert the volumetric flask with the solution when its done?

A

To make sure its all mixed and to check the level of the meniscus again

19
Q

Why must you make sure the standard solution is a suitable concentration compared to the solution you’re titrating it against?

A

If its too dilute, you’ll have to add loads before you reach an end point. If its too concentrated then tiny amounts will cause large changes in pH and your results may be inaccurate. So you should therefore make you standard solution to a similar concentration to the solution you’re titrating it against

20
Q

What do titrations allow you to do?

A

Find put exactly how much acid is needed to neutralise a quantity of alkali

21
Q

Why is it a good idea to do a rough titration?

A

To get a rough idea where the end point of the titration is, (the point where the alkali is exactly neutralised and the indicator changes colour).

22
Q

Why do you need to do more than one accurate titration?

A

To calculate a mean titre and to see if your results are accurate

23
Q

Why do you need to use a mean titration value (0.1 leeway)

A

To get an accurate mean titre

24
Q

How do you work out the titre?

A

The final reading on the burette minus the initial reading on the burette (2 decimal places)

25
Q

Why must you wash out the conical flask between titrations?

A

To remove any acid or alkali left in it

26
Q

what does an indicator show you?

A

When a reaction has finished. In titrations, indicators that change colour quickly over a very small pH range are used so you know exactly when the reaction has ended.

27
Q

Indicator: METHYL ORANGE

A

Turns YELLOW to RED when adding acid to alkali

28
Q

Indicator: PHENOLPHTHALEIN

A

Turns RED to COLOURLESS when adding acid to alkali

29
Q

Where is the best place to place the solution with the indicator?

A

On a white surface so the colour change is easy to see

30
Q

Why can’t universal indicator be used?

A

Its colour change is too gradual

31
Q

When a solution is made, what will its concentration depend on?

A

The amount of solute and the final volume of the solution

32
Q

How is concentration calculated?

A

Concentration = amount (moles) / Volume

33
Q

How is volume calculated?

A

Volume = amount (moles) / concentration

34
Q

How are moles calculated?

A

Moles = concentration x volume

Chemistry (11 decks)

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