What is the normality of a solution containing 3 moles of H2SO4 in 2 liters of solution? (H2SO4 is a diprotic acid)
Practice Questions
1 question
Q1
What is the normality of a solution containing 3 moles of H2SO4 in 2 liters of solution? (H2SO4 is a diprotic acid)
3 N
6 N
1.5 N
1 N
Normality (N) = equivalents of solute / liters of solution. H2SO4 has 2 equivalents per mole, so 3 moles = 6 equivalents. Normality = 6 equivalents / 2 L = 3 N.
Questions & Step-by-step Solutions
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Q
Q: What is the normality of a solution containing 3 moles of H2SO4 in 2 liters of solution? (H2SO4 is a diprotic acid)
Solution: Normality (N) = equivalents of solute / liters of solution. H2SO4 has 2 equivalents per mole, so 3 moles = 6 equivalents. Normality = 6 equivalents / 2 L = 3 N.
Steps: 6
Step 1: Understand that normality (N) is calculated using the formula: Normality (N) = equivalents of solute / liters of solution.
Step 2: Identify that H2SO4 (sulfuric acid) is a diprotic acid, meaning it can donate 2 protons (H+) per molecule.
Step 3: Calculate the number of equivalents for H2SO4. Since there are 3 moles of H2SO4 and each mole provides 2 equivalents, the total equivalents = 3 moles * 2 equivalents/mole = 6 equivalents.
Step 4: Determine the volume of the solution, which is given as 2 liters.
Step 5: Plug the values into the normality formula: Normality = 6 equivalents / 2 liters.
Step 6: Perform the calculation: 6 equivalents / 2 liters = 3 N.
