how many gram of concentrated nitric acid solution should be used to prepare 250 ml of 2 mole hno3 the concentrated acid is 70% Hno 3
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student-name Harshana asked in Chemistry
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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student-name Neha Thukral answered this
4166 helpful votes in Chemistry, Class XII-Science
To prepare 250mL of 2.0M HNO3 from 70% concentrated nitric acid:
Molarity of HNO3 = Moles of HNO3Volume of solution ×1000
2.0 = Moles of HNO3250×1000
Moles of HNO3 = 0.5 mol
Mass of 0.5 mol of HNO3 = Molar mass of HNO3 × Moles of HNO3 = 63×0.5 = 31.5 g
70% concentrated nitric acid means, 70g of HNO3 is present in 100g of HNO3 solution
Therefore, 31.5g of HNO3 is present in (100 ×31.5)/70 = 45g
Hence, 45g of HNO3 is required.
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ANSWER
The number of moles of nitric acid can be obtained by multiplying the molarity with volume
M×V=Moles of HNO
3
=
1000
250×2
=0.5
The mass of nitric acid can be obtained by multiplying the number of mols with molar mass and dividing with percentage concentration.
∴HNO
3
required =0.5×63×
70
100
=45g
Thus 45.0 g conc. HNO
3
of concentrated nitric acid solution should be used to prepare 250 mL of 2.0 M HNO
3
.