100 mL of H2SO4 solution having molarity 1 M and density 1.5 g/mL is mixed with 400 mL of water. Calculate final molarity of H2SO4 solution, if final density is 1.25 g/mL. What is... 100 mL of H2SO4 solution having molarity 1 M and density 1.5 g/mL is mixed with 400 mL of water. Calculate final molarity of H2SO4 solution, if final density is 1.25 g/mL. What is the density of solution for a liquid (mol. wt. = 50) if molarity is 9 and molality is 10?
Understand the Problem
The question is asking to calculate the final molarity of a sulfuric acid solution after mixing it with water and to determine the density of a solution based on its molarity and molality. This involves applying principles of solution concentration and dilution.
Answer
The final molarity of the H₂SO₄ solution is \(0.2 \, \text{M}\).
Answer for screen readers
The final molarity of the H₂SO₄ solution after mixing with water is (0.2 , \text{M}).
Steps to Solve
- Understand the Mixing Process
We start with 100 mL of a sulfuric acid solution with a molarity of 1 M. When mixed with 400 mL of water, the final volume becomes:
$$ V_f = 100 , \text{mL} + 400 , \text{mL} = 500 , \text{mL} $$
- Calculate the Moles of H₂SO₄
Using the initial molarity and volume, calculate the moles of sulfuric acid in the original solution:
$$ \text{Moles of } H_2SO_4 = M \times V = 1 , \text{M} \times 0.1 , \text{L} = 0.1 , \text{mol} $$
- Calculate the Final Molarity
To find the final molarity after dilution, use the formula for molarity:
$$ \text{Final Molarity} = \frac{\text{Total Moles}}{\text{Final Volume in Liters}} $$
Substituting the values we have:
$$ \text{Final Molarity} = \frac{0.1 , \text{mol}}{0.5 , \text{L}} = 0.2 , \text{M} $$
- Density Confirmation
The problem states that the density of the final solution is 1.25 g/mL, but it does not affect the molarity calculation. We will use it to double-check our understanding of density.
The final molarity of the H₂SO₄ solution after mixing with water is (0.2 , \text{M}).
More Information
The calculation demonstrates the dilution of a solution and how molarity changes with the addition of solvent. Molarity is a key concept in solution chemistry, reflecting the concentration of solute in a given volume of solvent.
Tips
- Confusing volume measurements (mL vs. L) can lead to incorrect final molarity calculations. Always convert mL to L when required.
- Forgetting to account for the total volume after mixing can lead to errors in final concentration.
