I have 1litre of concentrated nitric acid and i need 1 litre of 1 molar. how to calculate how much to use?

Question

the concentrated acid is 69% with an sg of 1.42. Is there a formula to calculate dilutions

sg stands for specific gravity

Kennyb can you show me the hard way

Answer 1

First we calculate the mass of HNO3 in a litter

A liter of that solution has a mass of 1420g

of that the mass of nitric acid is 1420*69/100=979.8g
the molar mass of HNO3 is 1+14+48=63 and so the molarity of your solution is 979.8/63 =15.55M
to have a liter of 1M you must dilute the solution by 15.55=0.0643

so you must take 0.0643L = 64.3 ml and complete with water to 1 Liter

Answer 2

What does sg stand for? And if 69% means that 69% is the acid and 31% is water then that is very concentrated. You will need to figure out what the actual concentration is mol l-1 (moles per litre) of the concentrated acid. For example, 500 ml of 2 mol l-1 is equivalent to 1 l of 1 mol l-1.

Answer 3

% concentrations refer to the mass percent of the solute in 100 ml of the solvent. So 69% nitric is 69g of HNO3 in 100 ml of water, the formula weight of nitric acid is 63 g per mole so there are 69/63 moles in 100 ml (1.095 moles), making the conc solution 10.95 molar, you need 1 molar which is 1 mole per 1000 ml, so dilute the conc solution by making up 1/10.95ml (91ml) in 1 litre.

Answer 4

molar mass nitric acid (solid) X 1Molar =63g/mol..

1000mL water -63=937

so,you add 937mL of water to the solid nitric acid just now.
and you will get 1molar of nitric acid in 1litre.