Titrations-Required Practical

Question 1

What apparatus do you need for the practical to commence?

Answer 1

Pipette, pipette filler, conical flask, burette

Question 2

What is the method used for carrying out the practical?

Answer 2

Use the pipette and pipette filler to add 25 cm3 of alkali to a clean conical flask.
Add a few drops of
indicator
and put conical flask on white tile.
Fill the burette with acid, note the starting volume.

Slowly add the acid from the burette to the alkali in the conical flask, swirling to mix.
Stop adding the acid when the solution begins to become colourless and slowly add until completely transparent. Note the final volume reading.

Question 3

What is the formula to work out the number of moles in a titration experiement?

Answer 3

Number of moles = concentration*volume

Question 4

What is the formula you use to work out the concentration of a solution?

Answer 4

Concentration = number of moles/volume

Question 5

You have 25cm^3 of HCl and you need 30cm^3 of Sodium Hydroxide to neutralise it as well as 5.4mol/dm^3. What would the concentration of HCl be?

Answer 5

6.48 g/dm^3

Question 6

0.5 mol of a solution is dissolved in 250cm^3 of solution. Calculate concentration.

Answer 6

2

Question 6

How do you turn cm^3 into dm^3?

Answer 6

Divide by 1000

Question 7

What is the formula to calculate the amount of solute dissolved in 2dm^3 of a 0.1mol/dm^3?

Answer 7

Amount = concentration*volume

Question 8

How much solute is dissolved in 2dm^3 of a 0.1mol/dm^3?

Answer 8

0.2mol

Question 9

Calculate the volume of a 2 mol/dm^3 solution that contains 0.5 mol of a solute.

Answer 9

0.25dm^3