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

Step-by-step explanation:

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

`Molarity=(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=(moles)/(1.0L)`

`moles=0.925* 1.0=0.925`

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