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? Show your work.

Answer 1

Answer:

0.925 moles of Nickel (II) chloride

Explanation:

Now, we know that the number of moles in a solution is given by;

n=CV

n= number of moles

C= molar concentration of solution = 0.925 M

V= volume of solution= 1.0 L

So having known all the parameters except the unknown (number of moles of Nickel (II) chloride) we can now proceed to find the unknown.

n= 0.925M ×1.0L

n= 0.925 moles of Nickel (II) chloride

Answer 2

Answer:

There are 0.925 moles of nickel (II) chloride present in the final 1 L volume solution.

Explanation:

The solutions are homogeneous mixtures (that is to say that their properties and composition are uniform) of two or more substances. We call the substance in the highest proportion: solvent, and the substance or substances in the smallest proportion: solute.

Molarity describes the relationship between the moles of a solute and the volume of a solution. Then, the molarity is equal to the number of moles of a solute divided by the volume of the solution in liters:

$Molarity (M)=\frac{number of moles of solute}{dissolution volume}$

Molarity is expressed in units ($\frac{moles}{liter}$).

If the solution has a molarity of 0.925, it indicates that there are 0.925 moles of nickel (II) chloride present in the final 1 L volume solution.