[arul]

Barium carbonate + nitric acid = barium nitrate + carbon di oxide + water.
Barium carbonate is in solid form but nitric acid is in liquid form.
what is the formula for equimolar reaction?
             I know this is simple calculation but i am confused.
some people suggested  to calculate using density, mass , vol formula by avoding purity nitric acid others suggested to use purity. dont know which is correct ?

Barium carbonate = M.w=197.34 g/mol
nitric acid = M.w= 63.01, density= 1.41 kg , purity = 69  %

solid + liquid  ----> equimolar formula = what?


       

[Archer]

Ignoring the question posted for now, what is your understanding of an "equimolar formula"?

[arul]

Ignoring the question posted for now, what is your understanding of an "equimolar formula"?

I guess I have not asked the question properly.

"Equimolar" represents equal number of moles in the given amount of the solution. 

For solid compounds
Eg. Barium carbonate ( M.w= 197.34g/mol)
 If I dissolve 197.34 grams in 1000 ml I will get 1 mole.
                 
But for liquid compounds
Eg. Nitric acid ( M.w=63.01, density= 1.51, purity=69% )
Here I cannot take nitric acid in grams because nitric acid is in liquid form. In these case how should I take 1 mole of nitric acid in 1000 ml.
What is the correct formula for this?


              If  I want to mix one mole of barium carbonate and one mole of nitric acid in 100 ml solution how many grams of barium carbonate and how many ml of nitric acid I should take? how to calculate this.

[Borek]

How many moles of nitric acid do you need?

What mass is it?

In what mass of solution is it?

What is volume of this solution?

[billnotgatez]

@arul
Are you starting with pure nitric acid or a aqueous solution of nitric acid of a designated concentration?
From the way you ask the question it is not clear.

[arul]

@arul
Are you starting with pure nitric acid or a aqueous solution of nitric acid of a designated concentration?
From the way you ask the question it is not clear.

The Nitric acid which I have is 69% of purity. In 100 ml of distilled water  how many ml of nitric acid should I add to get 1 mole of nitric acid aqueous soution.( Here concentration is not important for me)

[Archer]

@arul
Are you starting with pure nitric acid or a aqueous solution of nitric acid of a designated concentration?
From the way you ask the question it is not clear.

The Nitric acid which I have is 69% of purity. In 100 ml of distilled water  how many ml of nitric acid should I add to get 1 mole of nitric acid aqueous soution.( Here concentration is not important for me)

It is not common practice to measure the number of mols in 1ml of pure substance.

You provide 69% nitric acid, is this weight / volume or volume / volume?

Normally acid concentration is given as weight per unit volume i.e. the % is grams per 100 millilitres.

[arul]

@arul
Are you starting with pure nitric acid or a aqueous solution of nitric acid of a designated concentration?
From the way you ask the question it is not clear.

The Nitric acid which I have is 69% of purity. In 100 ml of distilled water  how many ml of nitric acid should I add to get 1 mole of nitric acid aqueous soution.( Here concentration is not important for me)

It is not common practice to measure the number of mols in 1ml of pure substance.

You provide 69% nitric acid, is this weight / volume or volume / volume?

Normally acid concentration is given as weight per unit volume i.e. the % is grams per 100 millilitres.

Yes 69 % represents weight/volume.

[Archer]

Great so every 1ml contains 0.69g of nitric acid.

How many mols of nitric acid in 0.69g?

[arul]

Great so every 1ml contains 0.69g of nitric acid.

How many mols of nitric acid in 0.69g?

moles = weight of the substance taken/ molecular weight

moles of nitric acid = 0.69/63.01 = 0.01095.

[Archer]

The Nitric acid which I have is 69% of purity. In 100 ml of distilled water  how many ml of nitric acid should I add to get 1 mole of nitric acid aqueous soution.( Here concentration is not important for me)

You should now be able to calculate this.

You haven't answered my original question

Ignoring the question posted for now, what is your understanding of an "equimolar formula"?

It is still not clear what you have been asked to calculate / report from your experiment.

[arul]

The Nitric acid which I have is 69% of purity. In 100 ml of distilled water  how many ml of nitric acid should I add to get 1 mole of nitric acid aqueous soution.( Here concentration is not important for me)

You should now be able to calculate this.

You haven't answered my original question

Ignoring the question posted for now, what is your understanding of an "equimolar formula"?

It is still not clear what you have been asked to calculate / report from your experiment.

Thanks much
My understanding for "equimolar formula" is equal mole calculation for  two compounds ( A & B ). If two  compounds are solid I know the method but for  solid(A) and liquid (B) combination Is there any "formula ".

[Archer]

Can you write a balanced equation for the reaction:

 Barium carbonate + nitric acid    barium nitrate + carbon dioxide + water.

[arul]

Can you write a balanced equation for the reaction:

 Barium carbonate + nitric acid    barium nitrate + carbon dioxide + water.

I didnt access my email for the last two days. Sorry for late reply

2HNO3 + BaCO3 ----------->Ba(NO3)2 + H2O + CO2

[Archer]

Ok so if your equation is correct

2HNO₃ + BaCO₃ Ba(NO₃)₂ +CO₂ + H₂O

Then this is not an equimolar reaction, you have two mols of nitric acid and only one mole of Barium carbonate.

So I am a bit confused by what you are asking, I apologise if I am being a bit slow on the uptake.

My understanding for "equimolar formula" is equal mole calculation for  two compounds ( A & B ). If two  compounds are solid I know the method but for  solid(A) and liquid (B) combination Is there any "formula ".

Let us assume that both are solids, replace any volumes in ml to grams. How would you solve this problem?