50ml of 20.8% bacl2 and 100ml of 9.8% h2s04 solutions are mixed. molarity of cl ions in the resulting solutions is At.wt of ba = 137
100ml of h2s04 solution having molarity 1M and density 1.5g/ml is mixed with 400ml of water. Calculate final molarity of h2s04 solution if final density is 1.25g/ml
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To find the molarity of the Cl ions in the resulting solution, we can follow these steps:
1. Determine the moles of BaCl2 in the solution.
- Volume of BaCl2 solution = 50 ml = 0.05 L
- Concentration of BaCl2 solution = 20.8%
This means 20.8 g of BaCl2 is present in 100 g of the solution.
So, the amount of BaCl2 in the solution = (20.8/100) * (50/1000) * 137 g/mol (since At.wt of Ba = 137)
Convert the amount to moles by dividing it by the molar mass of BaCl2.
2. Determine the moles of H2SO4 in the solution.
- Volume of H2SO4 solution = 100 ml = 0.1 L
- Concentration of H2SO4 solution = 9.8%
This means 9.8 g of H2SO4 is present in 100 g of the solution.
So, the amount of H2SO4 in the solution = (9.8/100) * (100/1000) * 98 g/mol (since At.wt of H2SO4 = 98)
Convert the amount to moles by dividing it by the molar mass of H2SO4.
3. Calculate the total moles of Cl ions in the resulting solution.
Since 1 mole of BaCl2 yields 2 moles of Cl ions, multiply the moles of BaCl2 by 2.
Add the moles of Cl ions from BaCl2 and H2SO4 to get the total moles.
4. Calculate the total volume of the resulting solution.
The total volume is the sum of the volumes of the BaCl2 and H2SO4 solutions.
5. Calculate the molarity of Cl ions in the resulting solution.
Divide the total moles of Cl ions by the total volume of the solution in liters.
Regarding the second question, to calculate the final molarity of the H2SO4 solution, follow these steps:
1. Calculate the total amount of H2SO4 in the initial solution.
- Volume of H2SO4 solution = 100 ml = 0.1 L
- Molarity of the H2SO4 solution = 1 M
Using the formula Molarity = Moles of solute / Volume of solution in liters, we can rearrange it to find the moles of solute.
Moles of H2SO4 = Molarity * Volume of solution in liters.
2. Calculate the amount of H2SO4 before dilution.
- Density of the H2SO4 solution = 1.5 g/ml
- Volume of H2SO4 before dilution = 100 ml = 0.1 L
Amount of H2SO4 before dilution = Density * Volume = 1.5 g/ml * 0.1 L.
3. Calculate the final volume of the solution after dilution.
- Final density of the solution = 1.25 g/ml
- Volume of water added = 400 ml = 0.4 L
We can assume that no significant volume change occurs during dilution, so the final volume of the solution is the sum of the initial volume of the H2SO4 solution and the volume of water added.
4. Calculate the final amount of H2SO4 in the solution.
The final amount of the solute (H2SO4) remains the same before and after dilution.
5. Calculate the final molarity of the H2SO4 solution.
Divide the final amount of H2SO4 by the final volume of the solution in liters.