Problem with titration problem Please HELP

[philipisaia]

Problem with titration problem Please HELP!

Hi,

In our AS level chemistry coursework we have performed the following experiment.

We took 2.00g of MHCO3 where M stands for a group 1 metal.
We put it in 250ml volumetric flask and we produced our standard solution.

Then in a conical flask we put 25ml of MHCO3 and 4 drops of methyl orange indicator.
Using aqueous sulphuric acid of concentration 0.050 mol/dm3 we performed three titrations.
My mean titre value came out to be 25.225ml


Here are the questions I have to solve.

a) Calculate the amount (number of moles) of sulphuric acid in the mean titre.
b) Calculate the amount (number of moles) of MHCO3 in 25ml of solution X where X stands for the standard solution in the volumetric flask.
c) Calculate the concentration of MHCO3 in solution X in mol/dm3. Use this value to calculate the relative molecular mass of MHCO3 and then identify M.


Please help me and try to solve this for me as soon as possible. For any question put a reply on this forum or send me and e-mail to philip@philippos.net


Thanks

 

[Ouabache]

Threre a lot of helpful people here. In order to get some replies you need to show your thoughts first.
I would check out this post: https://www.physicsforums.com/showthread.php?t=94384

 

[Blueshift5]

Hi there,

I understand that you are having trouble with a titration problem. Titration problems can be tricky, but with a little bit of practice and understanding of the concepts, you will be able to solve them easily.

Firstly, to calculate the amount of sulphuric acid in the mean titre, we need to use the formula:

Number of moles = concentration (in mol/dm3) x volume (in dm3)

In this case, the concentration of sulphuric acid is given as 0.050 mol/dm3 and the volume used is 25.225ml, which is equal to 0.025225dm3. Plugging these values into the formula, we get:

Number of moles = 0.050 mol/dm3 x 0.025225dm3 = 0.00126 moles

This is the amount of sulphuric acid in the mean titre.

Next, to calculate the amount of MHCO3 in 25ml of solution X, we need to use the same formula:

Number of moles = concentration (in mol/dm3) x volume (in dm3)

However, in this case, we do not know the concentration of solution X. To find it, we need to use the concept of stoichiometry. From the balanced chemical equation, we know that the ratio of sulphuric acid to MHCO3 is 1:1. This means that for every 1 mole of sulphuric acid used, 1 mole of MHCO3 is consumed.

Since we know the number of moles of sulphuric acid (0.00126 moles), we can also say that the number of moles of MHCO3 is also 0.00126 moles. Now, plugging this value into the formula, we get:

Number of moles = concentration (in mol/dm3) x volume (in dm3)

0.00126 moles = concentration (in mol/dm3) x 0.025dm3

Solving for concentration, we get:

Concentration = 0.00126 moles / 0.025dm3 = 0.0504 mol/dm3

This is the concentration of solution X.

To calculate the relative molecular mass of MHCO3, we need to use the formula:

Relative molecular mass = mass (in grams) / number of moles

We know the mass