Ksp for CuBr is 4.8 × 10⁻⁹.
<h3>Calculation:</h3>
Given,
Solubility = 0.01 g/L
Temperature = 25°C
The balanced equation is written as,
CuBr → Cu⁺(aq) + Br⁻(aq)
The solubility is converted to mol/L,
0.01 g/L = 0.01/143.45 mol/L
= 6.9 × 10⁻⁵ mol/L
[Cu⁺] = [Br⁻] = 6.9 × 10⁻⁵ mol/L
We know that Ksp is given as,
Ksp = [Cu⁺] [Br⁻]
= [6.9 × 10⁻⁵][6.9 × 10⁻⁵]
= 47.61 × 10⁻¹⁰
= 4.8 × 10⁻⁹
Hence, the Ksp for CuBr is 4.8 × 10⁻⁹.
I understand the question you are looking for is this:
The solubility of CuBr in water at 25°C is measured to be 0.010 g/L. Use this information to calculate Ksp for CuBr. Round your answer to 2 significant digits.
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