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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: ziczac on May 05, 2009, 10:24:36 PM

Title: Dilution problem
Post by: ziczac on May 05, 2009, 10:24:36 PM

I know this question is basic, but I am not sure my anwswer is right or not.

I was given a 37% w/w HCl which I have to dilute it to a 50 ml of 2 Mol/L HCl.

The way i am doing it is:

Mass of HCl present in the target solution, 50 ml of 2 Mol/L = ( 2 x 36.5) / (1000 / 50) = 3.65 g

As every 100g of the Concentrated acid contains 37g of HCl,

The amount need for dilution = (3.65 / 37) x 100 = 9.86g

i.e. Weight 9.86g of the conc. HCl and add water to 50 ml to get the target solution.


Is the above calculation correct or not?

Title: Re: Dilution problem
Post by: plankk on May 06, 2009, 12:02:54 AM

Correct.

Title: Re: Dilution problem
Post by: Borek on May 06, 2009, 03:17:44 AM

Quote from: ziczac on May 05, 2009, 10:24:36 PM

I know this question is basic

Quote

I was given a 37% w/w HCl

This makes the question acidic, not basic.

I would go one step further - take density tables and check what volume of concentrated HCl you need.