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Calculate the concentration of nitric acid in moles per litre in a sample which has a density 1.41 g mL^-1 and the mass per cent of nitric acid in it being 69% .
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![The molality of 90 % H2SO4 solution is [density = 1.8 gm/ml ]](https://haygot.s3.amazonaws.com/questions/1641200_1753377_ans_9b9835b877a84dfe8d010e65e1fb0a2d.jpg "The molality of 90 % H2SO4 solution is [density = 1.8 gm/ml ]")
The molality of 90 % H2SO4 solution is [density = 1.8 gm/ml ]
How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0 M HNO3 ? The concentrated acid is 70
![What is the molarity of H2SO4 solution that has a density of 1.84 g/cc and contains 98% mass of H2SO4 ? [Given: the atomic mass of S = 32]](https://haygot.s3.amazonaws.com/questions/1308069_771116_ans_de8785a7f08b42caa8f74797b87a094b.jpg "What is the molarity of H2SO4 solution that has a density of 1.84 g/cc and contains 98% mass of H2SO4 ? [Given: the atomic mass of S = 32]")
What is the molarity of H2SO4 solution that has a density of 1.84 g/cc and contains 98% mass of H2SO4 ? [Given: the atomic mass of S = 32]
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Concentrated aqueous sulphuric acid is 98
Dissolving 120 g of urea(mol. wt. 60 ) in 1000 g of water gave a solution of density 1.15 g/mL. The molarity of the solution is:
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If the density of methanol is 0.793 kg L^-1 , what is its volume needed for making 2.5 L of its 0.25 M solution?
