Question

How much copper is present in $50g$ of $CuS{O_4}$ ?
A. $19.90g$
B. $39.81g$
C. $63.5g$
D. $31.71g$

Answer 1

Hint:Anhydrous copper sulfate is a colorless, crystallized and powdered substance which has the capacity of retaining high value of water of crystallization. In one mole of copper sulfate, a maximum of five moles of water can be retained inside the crystal lattice of copper sulfate.

Complete step by step answer:
The molar mass which is also known as the molecular weight is the sum of the total mass in grams of all the atoms that make up a mole of a particular molecule/ substance. The unit that is used to measure the molar mass of any compound or substance is grams per mole ($gmo{l^{ - 1}}$ ). The molar mass of the anhydrous copper sulfate can be determined as the sum of the masses of one copper atom, one sulfur atom and four oxygen atoms.
Atomic mass of copper, $Cu = 63.5g$
Atomic mass of sulfur, $S = 32g$
Atomic mass of oxygen, $O = 16g$
Molar mass of copper sulfate, $CuS{O_4} = 63.5 + 32 + (4 \times 16) = 159.5g$
As we can see that, $159.5g$ of $CuS{O_4}$ will have = $63.5g$ of copper
$\therefore ,1g$ of copper sulfate will have = $\dfrac{{63.5}}{{159.5}}g$ of copper
Hence, $50g$ of copper sulfate will have = $\dfrac{{63.5}}{{159.5}} \times 50 = 19.90g$ of copper
Thus, the correct option is A. $19.90g$ .


Note:Copper sulfate is produced industrially on a large scale, by treating copper metal with hot concentrated sulfuric acid or its oxides with dilute sulfuric acid. For laboratory use, copper sulfate is usually purchased. Copper sulfate can also be produced by slowly leaching low grade copper ore in air; bacteria may be used to speed up the process. Whenever copper sulfate pentahydrate is heated, it loses its blue color slowly as during this process, it undergoes various phase transitions.