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calculate the molarity of a solution that contains 20.275g calcium bromide dissolved in 575 mL of solution

Respuesta :

superman1987
1- We have to get the molar mass of calcium bromide, by getting the chemical formula ( CaBr2).
From the chemical formula, we have to get the molecular weight for each of Ca&Br on the periodic table:
Ca = 40.078    & Br = 79.904
* from the chemical formula ( CaBr2) so, the molecular weight of calcium bromide is:
40.078 + 2x(79.904) = 199.89 
2- number of moles = weight / molecular weight
                                  =20.275 / 199.89 = 0.1014 moles
3- where the volume of solution by littre = 575 mL/ 1000 = 0.575 L
So,
4-Molarity = moles of solute / L of solution
                   = 0.1014 / 0.575 = 0.1763 mol/L

Cricetus

The molarity of CaBr₂ will be "0.176 M".

Calcium Bromide (CaBr₂):

Calcium bromide has been primarily used to regulate pressures as a constituent of slightly elevated clear drilling, completing, surface facilities, as well as packaging liquids. It is also used in photography, scaling substances, wood preservatives, as well as flame resistance mixes.

Mass of Calcium Bromide (CaBr₂) = 10.275 g

Molar mass of Calcium Bromide = 199.98 g/mol

Volume of solution = 575 mL or,

                                = 0.575 L

Now,

The number of moles be:

= 20.275 × [tex]\frac{mol}{199.89}[/tex]

= 0.101 mol

hence,

The Molarity of solution be:

= [tex]\frac{0.101}{0.575}[/tex]

= 0.176 M

Thus the response above is appropriate.

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