Copper(II) bromide is used as a wood preservative. What mass of CuBr2 is needed to prepare 750.0 mL of a 1.25 M solution?

2 answers:

8 0

Calculation yields 209.53. The molar concentration is calculated by moles divided by volume. Given the volume of 750 mL, which translates to 0.75 L, the moles of CuBr₂ can be determined as molar concentration multiplied by volume, resulting in 1.25 × 0.75 = 0.9375. Mole count is derived from the mass of CuBr₂ divided by its molecular mass. The molecular mass of CuBr₂ is computed as 63.5 + 80 × 2 = 223.5, where the mass of Cu is 63.5 and that of Br is 80. Consequently, the mass needed amounts to 223.5 × 0.9375 = 209.53 g.

eduard [2.7K]2 months ago

4 0

The necessary mass of CuBr₂ is 238.2 g. This calculation involves molarity and volume to derive the mass of solute, with the steps shown as follows. The formula yields moles from the product of 1.25 mol/L and 0.750 L, which results in 0.9375 moles. When multiplied by the molar mass (223.35 g/mol), it equates to 238.2 g of salt.

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