Preparing 0.1M Nitric Acid (1000ml, 65% Nitric Acid)

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To prepare 1000ml of 0.1M Nitric acid using 65% Nitric acid, first calculate the required grams of pure HNO3 using the formula M = ((% x Specific gravity)/Molecular weight) x 10, which yields the concentration in moles. The specific gravity of 65% Nitric acid is 1.42g/ml, and its molecular weight is 63g/mol. By determining the number of moles needed and converting this to grams of pure HNO3, the dilution process can then be completed by accounting for the concentration of the starting solution. The final steps involve calculating the volume of 65% Nitric acid needed and diluting it appropriately with water. This method ensures accurate preparation of the desired concentration.
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how do I make 1000ml of 0.1M Nitric acid with 65% Nitric acide (specific gravity 1.42g) and Molecular weight 63g/mol
 
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Diluting acid with water

Homework Statement



To make 1000ml of 0.1M of Nitric acid with 65% Nitric acid.
Specific gravity= 1.42g/
Molecular weight= 63g/mol

Homework Equations


M = ((% x Specific gravity)/Molecular weight) x 10
cava = cfvf


The Attempt at a Solution

 


You presented a formula in your Relevant equations section. If you trust this formula then just substitute the values for the described information.
 
You could start with the number of moles of HNO3 you would want. If you know the moles of HNO3, then use formula weight to find number of grams of pure HNO3; but you know that your source is not pure, but instead is 65% w/w. so you have two more steps... can you derive them?
 

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