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Offline arul

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simple but confusing
« on: November 07, 2013, 02:03:24 PM »
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?


       

Offline Archer

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Re: simple but confusing
« Reply #1 on: November 08, 2013, 08:43:55 AM »
Ignoring the question posted for now, what is your understanding of an "equimolar formula"?

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Offline arul

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Re: simple but confusing
« Reply #2 on: November 08, 2013, 10:19:07 AM »
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.

Offline Borek

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Re: simple but confusing
« Reply #3 on: November 08, 2013, 12:21:15 PM »
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?
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Offline billnotgatez

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Re: simple but confusing
« Reply #4 on: November 08, 2013, 06:09:50 PM »
@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.


Offline arul

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Re: simple but confusing
« Reply #5 on: November 09, 2013, 01:24:41 AM »
@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)

Offline Archer

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Re: simple but confusing
« Reply #6 on: November 09, 2013, 01:32:32 AM »
@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.
“ I love him. He's hops. He's barley. He's protein. He's a meal. ”

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Offline arul

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Re: simple but confusing
« Reply #7 on: November 09, 2013, 01:42:22 AM »
@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.

Offline Archer

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Re: simple but confusing
« Reply #8 on: November 09, 2013, 01:47:28 AM »
Great so every 1ml contains 0.69g of nitric acid.

How many mols of nitric acid in 0.69g?
“ I love him. He's hops. He's barley. He's protein. He's a meal. ”

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Offline arul

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Re: simple but confusing
« Reply #9 on: November 09, 2013, 02:01:02 AM »
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.

Offline Archer

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Re: simple but confusing
« Reply #10 on: November 09, 2013, 03:24:17 AM »

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.
“ I love him. He's hops. He's barley. He's protein. He's a meal. ”

Denis Leary.

Offline arul

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Re: simple but confusing
« Reply #11 on: November 09, 2013, 06:46:37 AM »

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 ".

Offline Archer

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Re: simple but confusing
« Reply #12 on: November 09, 2013, 11:25:50 AM »
Can you write a balanced equation for the reaction:

 Barium carbonate + nitric acid  :rarrow:  barium nitrate + carbon dioxide + water.
“ I love him. He's hops. He's barley. He's protein. He's a meal. ”

Denis Leary.

Offline arul

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Re: simple but confusing
« Reply #13 on: November 11, 2013, 12:02:00 AM »
Can you write a balanced equation for the reaction:

 Barium carbonate + nitric acid  :rarrow:  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

Offline Archer

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Re: simple but confusing
« Reply #14 on: November 11, 2013, 01:34:02 AM »
Ok so if your equation is correct

2HNO3 + BaCO3 :rarrow: 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?
“ I love him. He's hops. He's barley. He's protein. He's a meal. ”

Denis Leary.

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