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Chem Class > 3.1.2 Amount of Substance > Flashcards

3.1.2 Amount of Substance Flashcards

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1
Q

How many particles does 1 mole contain (i.e. what’s Avogadro’s constant)?

A

6.02 x 1023 particles

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2
Q

What is the formula for converting between no. of particles and no. of moles?

A
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3
Q

What formula do you use to calculate the no. of moles from mass?

A
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4
Q

What formula do you use to calculate the no. of moles from concentration?

A
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5
Q

Write the ionic equation for this reaction:

HNO3 + NaOH → NaNO3 + H2O

A
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6
Q

What does ‘aq’ mean?

A

Aqueous (solution in water)

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7
Q

When you’ve written an ionic equation, what should you do?

A

Check the charges & atoms are balanced

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8
Q

What is the formula for percentage yield?

A
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9
Q

What does percentage yield tell you?

A

Tells you how wasteful process is = based on how much product is lost

(Doesn’t measure how wasteful reaction itself)

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10
Q

What is atom economy?

A

Measure of proportion of reactant atoms that become part of desired product (rather than by-products)

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11
Q

What is the formula for atom economy?

A
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12
Q

Why do companies in the chemical industry try to use processes with high atom economies?

A
  • Better for environment
    • ∵ produce less waste
  • More efficient use of raw materials
    • More sustainable (use natural resources more slowly)
  • Less expensive
    • Spend less on separating desired product from waste products & less on treating waste
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13
Q

What is empirical formula?

A

Simplest whole number ratio of atoms of each element in a compound

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14
Q

What is molecular formula?

A

Actual no. of atoms of each element in a compound

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15
Q

What is a standard (volumetic) solution?

A

Solution that you know the exact concentration of

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16
Q

What does the making of standard solution involve?

A

Involves dissolving a known amount of solid in known amount of water to create known concentration

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17
Q

Describe how you would make 250 cm3 of a 2.00 mol
dm-3 solution of sodium hydroxide (8 steps)

A
  1. Work no. moles of sodium hydroxide needed (0.5 moles)
  2. Work out no. of grams of sodium hydroxide (20.0 g)
  3. Place weighing boat on digital balance & weigh out mass of solid
    1. Tip it into beaker
    2. Re-weight boat
    3. Subtract mass of boat from mass of boat and solid together = find precise mass of solid used
  4. Add distilled water to beaker (e.g. 100 dm3) & stir until sodium hydroxide dissolved
  5. Pour solution into large enough volumetric flask, using funnel
  6. Rinse beaker & stirring rod with distilled water & add that to flask
  7. Top flask up to correct volume with distilled water - make sure bottom of meniscus reaches the line
  8. Stopper the flask & turn it upside down a few times = makes sure it’s mixed
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18
Q

Making a standard solution:

Why do you re-weigh the boat?

A

∵ it may contain traces of solid

19
Q

Making a standard solution:

Why do you rinse the beaker & stirring rod with distilled water and add that to the flask?

A

Makes sure no solute clings to beaker/rod

20
Q

What do titrations allow you to do?

A

Allow to find out exactly the volume of acid needed to neutralise a measured quantity of alkali (& vice versa)

Use this data to work out concentration of alkali

21
Q

Describe a method for a titration

A
  1. Use pipette to measure set volume of solution that you want to find concentration of
    1. Put into flask
  2. Add drops of indicator
  3. Fill burette with standard solution of acid
  4. Use funnel to pour acid into burette
    1. Do this below eye level
  5. Do rough titration to get idea of end point
    1. Add acid to alkali using burette = give flask regular swirls
  6. Do accurate titration
    1. Take initial reading of acid in burette
    2. Run acid within 2 cm3 of end point
    3. Add acid dropwise until reach end point
  7. Work amount of acid used to neutralise alkali
    1. (Final reading - initial reading = volume of titre)
  8. Repeat titration few times - until have 3 concordant results
  9. Use results to calculate mean volume - leaving anomalous results
22
Q

What kind of indicators are used in a titration?

A

Indicators that change colour quickly over very small pH range = used so you know exactly when reaction has ended

23
Q

Name 2 indicators that could be used in a titration (for for acid/alkali reactions)

A
  • Methyl orange
  • Phenolphthalein
24
Q

What colour is methyl orange in acids?

A

Red

25
Q

What colour is methyl orange in alkalis?

A

Yellow

26
Q

What colour is phenolphthalein in acids?

A

Colourless

27
Q

What colour is phenolphthalein in alkalis?

A

Pink

28
Q

What do pipettes measure?

A

Only one volume of solution

29
Q

What do burettes measure and let you do?

A

Measures different volumes & lets you add the solution drop by drop

30
Q

What is the ideal gas equation?

A
31
Q

What is rule for volume of gases?

A

At room temperature and pressure, 1 mole of any gas occupies 24 dm3

32
Q

What formula is used to calculate the volume of gases?

A
33
Q

State the conversions for mg to g & vice versa

A

mg → g ÷ 1000

mg ← g x 1000

34
Q

What is the mass in grams of a single atom of silver?

The Avogadro constant = 6.02 x 1023

Ag = 107.9

A

1.79 x 10-22 g

35
Q

What is the mass in grams of a single molecule of water?

The Avogadro constant = 6.02 x 1023

Mr of water = 18.02

A

2.99 x 10-23 g

36
Q
A

13.3 g

37
Q
A

2.41 x 1022

38
Q
A
39
Q
A
40
Q

State why it’s important to fill the space below the tap in the burette before beginning an accurate titration (1)

A

(Will fill during titration and cause) titre value to be too high

41
Q

State why rinsing the inside of the conical flask with distilled water during a titration can improve the accuracy of the end point (1)

A

Returns reagent on the sides of the flask to the reaction mixture (to ensure that all of the acid/alkali reacts)

42
Q
A
43
Q
A
44
Q

State why rinsing doesn’t change the volume of base solution needed in a titration (1)

A

no effect on amount/moles of either reactant or water is not a reagent

Chem Class (34 decks)

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