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? Read more

Steps to Solve

1. 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:

$$ V_f = 100 , \text{mL} + 400 , \text{mL} = 500 , \text{mL} $$

2. Calculate the Moles of H₂SO₄

Using the initial molarity and volume, calculate the moles of sulfuric acid in the original solution:

$$ \text{Moles of } H_2SO_4 = M \times V = 1 , \text{M} \times 0.1 , \text{L} = 0.1 , \text{mol} $$

3. 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:

$$ \text{Final Molarity} = \frac{0.1 , \text{mol}}{0.5 , \text{L}} = 0.2 , \text{M} $$

4. 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.