Question

The final solution had a volume of 1.0L and a molarity of 0.925. How many moles of Nickel (II) chloride were present in the solution?

Answer 1

Answer: The moles of nickel (II) chloride were present in the solution are 0.925

Explanation:

Molarity is defined as the number of moles of solute dissolved per liter of the solution.

$Molarity=\frac{n}{V_s}$

where,

Molarity = 0.925

n= moles of solute  = 0.2

$V_s$ = volume of solution in L = 1.0 L

Now put all the given values in the formula of molarity, we get

$0.925=\frac{moles}{1.0L}$

$moles=0.925\times 1.0=0.925$

Therefore, the moles of nickel (II) chloride were present in the solution are 0.925