Question

5.35 grams of sodium chloride are dissolved to make 150 milliliters of solution. What is the molarity of the solution?

Answer 1

0.61 M

Explanation:

In order to find molarity we must use the following equation:

`M=(mols)/(L)`

First we need to convert our grams into mols using the molar mass of sodium chloride. The molar mass of sodium chloride is calculated by adding the masses of both sodium and chlorine which can be found on the Periodic Table.

Molar mass of NaCl = 58.44 `g/(mol)`

We can now convert to mols of NaCl by dividing our mass (5.35 g) by our mm (58.44 g/mol)

`5.35 g((1mol)/(58.44g))=0.092 mols`

Now we need to convert our milliliters of solution into liters of solution. There are 1000 milliliters to every 1 liters. So need to divide our milliliters by 1000.

`150mL((1L)/(1000mL))=0.15L`

Now using the original equation:

`M=(0.092mol)/(0.15L)=0.61(mol)/(L)`

Answer 2

`[NaCl(aq)]~=0.60*mol*L^-1`

Explanation:

`"Molarity"-="moles of solute"/"volume of solution"`

`=((5.25*g)/(58.44*g*mol^-1))/(150*mLxx10^-3*L*mL^-1)-=0.599*mol*L^-1` with respect to `[NaCl(aq)]`

Note that this dissolution is quite properly regarded as a chemical reaction given that ionization occurs on dissolution, along with the formation of aquated ions....

`NaCl(s) stackrel(H_2O)rarrNa^+ +Cl^-`