A 0.15 M Solution of BaCl<sub>2</sub> Contains
A 0.15 M solution of BaCl<sub>2</sub> (Barium Chloride) contains 0.15 moles of BaCl<sub>2</sub> per liter of solution. This is based on the definition of molarity (M), which is the number of moles of solute per liter of solution.
Here's a breakdown of what this means:
- Solute: The substance being dissolved, in this case, BaCl<sub>2</sub>.
- Solvent: The substance that dissolves the solute, usually water in this case.
- Solution: The homogeneous mixture formed when the solute dissolves in the solvent.
To understand the composition of a 0.15 M BaCl<sub>2</sub> solution further, consider these points:
- Barium Ions (Ba<sup>2+</sup>): Since BaCl<sub>2</sub> dissociates into one Ba<sup>2+</sup> ion and two Cl<sup>-</sup> ions when dissolved, a 0.15 M BaCl<sub>2</sub> solution will contain 0.15 moles of Ba<sup>2+</sup> ions per liter.
- Chloride Ions (Cl<sup>-</sup>): The solution will contain 0.30 moles of Cl<sup>-</sup> ions per liter, as each mole of BaCl<sub>2</sub> produces two moles of chloride ions.
Calculations:
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Moles of BaCl<sub>2</sub> in a specific volume: If you have, for example, 500 mL (0.5 L) of the solution, the number of moles of BaCl<sub>2</sub> can be calculated as follows:
- Moles = Molarity × Volume
- Moles = 0.15 M × 0.5 L = 0.075 moles
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Mass of BaCl<sub>2</sub> in a specific volume: To find the mass of BaCl<sub>2</sub> in the solution, you would need to convert moles to grams using the molar mass of BaCl<sub>2</sub> (208.23 g/mol).
In summary, a 0.15 M solution of BaCl<sub>2</sub> is a solution where 0.15 moles of BaCl<sub>2</sub> are dissolved in every liter of solution. This solution contains 0.15 moles of Ba<sup>2+</sup> ions and 0.30 moles of Cl<sup>-</sup> ions per liter.
