A 250.0 mL solution contains 4.6 g

copper

(II) chloride, CuCl2. Find the molarity of this

solution.

THE MOLARITY OF THE SOLUTION IS 0.1368 mol/dm3

Explanation:

Molarity is the number of moles of the solute per litre of the solution.

It is expressed as;

Molarity in mol/dm3 = Molarity in g/dm3 / Relative molecular mass

Step 1: obtain the molarity in g/dm3

4.6 g of CuCl2 in 250 mL solution

4.6 / 250 * 10^-3

= 4.6 / 0.25

= 18.4 g/dm3 of CuCl2

Step 2: calculate the relative molecular mass of CuCl2

( Cu = 63.5  , Cl = 35.5)

RMM = 63.5 + 35.5 *2

= 63.5 + 71

= 134.5 g /mol

Step 3: Calcullate molarity in mol/dm3

Molarity in mol/dm3 = molarity in g/dm3 / RMM

= 18.4 g/dm3 / 134.5 g/mol

= 0.1368 mol/dm3

So therefore, the molarity of CuCl2 is 0.1368 mol/dm3

3 hours because it is a decent distance.

the dependant variable is spilled water

the independent is the heat