calculate the normality of the solution obtained by mixing 100 CC of 0.2N. H2So4 with 50 cc of 0.1 N HCL
Answers
Considering valancy 0.1 mol H2SO4 reacts with 0.2 mols of NaOH. Strong acid with strong acid in diluted condition reacts. Resultant Na2SO4 has a neutral pH.
Let us find the density of one decimolar Sulphuric acid. Density of Concentrated Sulphuric acid is 1.84 (18.4 molar) where 0.5 molar weighs 1.05g/ml.
Sodium hydroxide is 1.5 (17.4 molar) where a 0.5 molar is likely to weigh 1.02G/ml.
Sodium sulphate, resultant product weighs as 1g/ml at 25℃.
Water, byproduct is 0.997g/ml at 25℃.
Mass is neither generated nor destroyed but volume changes as per density. Molarity is the strength per litre and not the quantity left behind.
Hence the remaining solution may contain less than 0.1 molar Sulphuric acid, that the density being reduced by Na2SO4 and water, the result can be a value below 0.1 molar.
Answer:
Explanation:
Considering valancy 0.1 mol H2SO4 reacts with 0.2 mols of NaOH. Strong acid with strong acid in diluted condition reacts. Resultant Na2SO4 has a neutral pH.
Let us find the density of one decimolar Sulphuric acid. Density of Concentrated Sulphuric acid is 1.84 (18.4 molar) where 0.5 molar weighs 1.05g/ml.
Sodium hydroxide is 1.5 (17.4 molar) where a 0.5 molar is likely to weigh 1.02G/ml.
Sodium sulphate, resultant product weighs as 1g/ml at 25℃.
Water, byproduct is 0.997g/ml at 25℃.
Mass is neither generated nor destroyed but volume changes as per density. Molarity is the strength per litre and not the quantity left behind.
Hence the remaining solution may contain less than 0.1 molar Sulphuric acid, that the density being reduced by Na2SO4 and water, the result can be a value below 0.1 molar.