How many grams of concentrated nitric acid solution should be used to prepare 250mL of 2.0M HNO3 ?The concentrated acid is 70% HNO3.
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Given,
Mass of whole solution = 100 g
Then,
Mass of HNO3 = 70 g
Volume of solution = 250 ml
Molarity = Moles of solute / Volume of solution *1000
2.0 M = ( Moles of HNO3 / 250) * 1000
Moles of HNO3 = 2.0 /4
MOLES OF HNO3 = 0.5
Moles of HNO3 = Mass of HNO3 / Molar Mass of HNO3
Mass of HNO3 = 0.5 * 63 = 32.5 gm
32.5 g of HNO3 is present in ( 100 * 31.5 / 70
Mass of HNO3 required = 45 g.
Mass of whole solution = 100 g
Then,
Mass of HNO3 = 70 g
Volume of solution = 250 ml
Molarity = Moles of solute / Volume of solution *1000
2.0 M = ( Moles of HNO3 / 250) * 1000
Moles of HNO3 = 2.0 /4
MOLES OF HNO3 = 0.5
Moles of HNO3 = Mass of HNO3 / Molar Mass of HNO3
Mass of HNO3 = 0.5 * 63 = 32.5 gm
32.5 g of HNO3 is present in ( 100 * 31.5 / 70
Mass of HNO3 required = 45 g.
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