Unit 3-Volumetric Analysis Flashcards

1
Q

What is a standard solution?

A

A solution of accurately known concentration.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Describe how a standard solution would be made from a primary standard.

A
  1. Accurately measure out required mass of primary standard
  2. Dissolve in a small volume of solvent.
  3. Transfer solution and rinsing into volumetric flask
  4. Make up to graduation mark w
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are 4 characteristics of a primary standard?

A

be available in high state of purity

be stable when solid and in solution

be soluble

have a reasonably high GFM

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Which of the following chemicals would not be suitable as a primary standard?

Sodium carbonate (Na2CO3)

Sodium hydroxide (NaOH)

Hydrated oxalic acid (H2C2O4.2H2O)

Explain your answer

A

Sodium hydroxide has a relatively low GFM, is unstable as a solid (absorbs moisture), unstable as a solution.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What must be carried out before using sodium hydroxide in a volumetric analysis?

A

Standardisation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

How would a solution of sodium hydroxide be standardised?

A

Titrate with standard solution/solution of known
concentration of a suitable chemical.

For example use oxalic acid for standardising sodium hydroxide or potassium permanganate.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are the four different types of volumetric analysis?

A

Acid/base titrations

Redox titrations

Complexometric titrations

Back titrations

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Give an example of the following types of titrations

  • Acid/base titrations
  • Redox titrations
  • Complexometric titrations
  • Back titrations
A

Acid/base titrations-Sodium hydroxide and hydrochloric acid or any non weak/weak pairing.
Redox titrations-Oxalic acid and potassium permanganate or any example based on reactions between oxidising and reducing agents.
Complexometric titrations-based on reactions in which complexes are formed — EDTA and metal ions
Back titrations-useful for solid substances with low solubility calcium carbonate.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Why does back titration sometimes need to be used?

A

For insoluble substances

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What are the steps in a titration calculation?

A

Calculate the average titre - 0.1cm3 concordancy

Calculate n using CV [V in litres]

Use mole ratio

Look to see if scaling up required

Calculate the unknown - either m, C, V or %

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What does EDTA determine in a complexometric titration?

A

The mass or % of a METAL ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly