What is the molar mass of copper ii sulfate cuso4


Asked by admin @ in Chemistry viewed by 359 People


An aqueous solution is 15.0% by mass of copper(II) sulfate pentahydrate, CuSO4∙5H2O.What

is the molarity of CuSO4 in this solution at 20°C?The density of this solution at 20°C is1.167g/mL(molecular weight of CuSO4∙5H2O = 249.5, molecular weight of CuSO4 = 159.5)​

Answered by admin @



0.702 mol / dm³.

Explanation

Consider a 1,000 mL sample of this solution. Mass of the sample:

m = \rho \cdot V = 1.167 \;\text{g}\cdot\text{mL}^{-1}\times1,000\;\text{mL} = 1,167\;\text{g}.

The mass ratio of copper(II) sulfate pentahydrate in this sample is 15 %. In other words, 1,167 \times 15\;\% = 175.1\;\text{g} among that 1,167 grams of the solution is \text{Cu}\text{SO}_4\cdot(\text{H}_2\text{O})_5.

Number of moles of \text{Cu}\text{SO}_4\cdot(\text{H}_2\text{O})_5 in that 175.1\;\text{g} of the hydrate:

n(\text{hydrate}) = \dfrac{m(\text{hydrate})}{M(\text{hydrate})} = \dfrac{175.1}{249.5} = 0.702\;\text{mol}.

Concentration of the hydrate:

c(\text{hydrate}) = \dfrac{n(\text{hydrate})}{V} = \dfrac{0.702\;\text{mol}}{1,000\;\text{mL}}=\dfrac{0.702\;\text{mol}}{1\;\text{L}} = 0.702\;\text{mol}\cdot\text{dm}^{-3}.


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