Standardise a solution of HCL using a standard solution of Na2CO3

Draw a diagram of the experiment

Step 1

Wash out the apparatus with a washbottle

Step 2

Pour acid into a beaker and repeat for the base

Step 3

Rinse out pipette and pipette Na2CO3 into a conical flask

Step 4

Add drops of methyl orange to conical flask

Step 5

Clamp burette with a retort stand and fill it with HCl using a funnel

Step 6

Open tap of burette into a spare beaker until HCl reaches the bottom of the meniscus

Step 7

Open tap again and swirl meniscus until solution turns from orange to pink

Step 8

Note volume of acid required and repeat 2 more times

Step 9

Calculate average from last two readings

Why is the first result of a titration ignored?

High chance it's inaccurate since it gives you the approximate end point

What gas is produced during this titration?

Carbon dioxide

Why does HCl have to be standardised?

HCl is not a primary standard

Why should you not add too much indicator?

They are weak acids/bases and too much could affect the results

Why shouldn't you pipette directly from the volumetric flask?

Impurities from pipette would contaminate entire solution in the volumetric flask