If $$80$$ g of copper sulphate $$CuSO4$$ . $$5H2O$$ is dissolved in deionised water to make $$5L$$ of solution. The concentration of the copper sulphate solution is x ×$$10$$−$$3$$ mol L−$$1$$. The value of x is $$_____________$$.(nearest$$ whole $$number)[Atomic masses Cu : $$63.54u$$, S : $$32u$$, O : $$16u$$, H : $$1u$$]

Question

If $$80$$ g of copper sulphate $$CuSO4$$ . $$5H2O$$ is dissolved in deionised water to make $$5L$$ of solution. The concentration of the copper sulphate solution is x ×$$10$$−$$3$$ mol L−$$1$$. The value of x is $$_____________$$.(nearest$$ whole $$number)[Atomic masses Cu : $$63.54u$$, S : $$32u$$, O : $$16u$$, H : $$1u$$]

Infinity Learn · Accepted Answer

Given, mass of $$CuSO4$$ . $$5H2O$$ $$=$$ $$80$$ gThe concentration of copper sulphate solution is  x×$$10-3mol/L$$  Molarity $$=$$ Number of moles of soluteVolume of $$solution(L)$$ ..... (i)Molar$$ mass of $$CuSO4$$ . $$5H2O$$ $$=$$ $$63.54$$ $$+$$ $$32$$ $$+$$ $$16$$ × $$4$$                                    $$=$$ $$5$$ × $$18$$ $$=$$ $$249.54$$ $$g/molNumber$$ of moles of solute $$=$$ Weight of soluteMolecular mass of solute                            $$=$$ $$80g249.54g/mol$$ $$=$$ $$0.32$$ molVolume of solution $$=$$ $$5$$ LFrom Eq. $$(i),Molarity $$=$$ $$0.32055$$ $$=$$ $$64.11$$×$$10$$−$$3$$ $$mol/L$$∴ x $$=$$ $$64.11or$$ x ≈ $$64Hence$$, answer is $$64$$.

If 80 g of copper sulphate CuSO4 . 5H2O is dissolved in deionised water to make 5L of solution. The concentration of the copper sulphate solution is x ×10−3 mol L−1. The value of x is _____________.(nearest whole number)[Atomic masses Cu : 63.54u, S : 32u, O : 16u, H : 1u]

Detailed Solution

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