Question
Asked Oct 6, 2019
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A 4.00 gram sample of hydrate of nickel(II) bromide loses 0.793 grams of water when heated. Determine the mass percent water in the hydrate and the formula of the hydrate

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Expert Answer

Step 1

Mass of hydrated nickel bromide = 4 g

When it heated it lose water of 0.793 g from nickel bromide.

Mass of nickel bromide without water molecules

(4-0.793)g
=3.207g
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(4-0.793)g =3.207g

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Step 2

The mass percentage is calculated as the mass of a component divided by the total mass of the mixture and then multiply by 100.

The mass percentage of water is 19.82.

 

 

mass of water
mass percentage of water
-x100
mass of given compound(NiBr,.XH2O
0.793
4
-x100
19.82
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mass of water mass percentage of water -x100 mass of given compound(NiBr,.XH2O 0.793 4 -x100 19.82

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Step 3

Mass of anhydrous nickel bromide is 3.207g.

So no. of the mole of anhydrous nickel bromide

By using equation (1), no...

mass (g
(1)
no. of moles(n) =
molecular massg mol
3.207g
218.53 g mol-
n 0.0146 moles
n =
0.793 g
n =
18 gmol-
n 0.0440moles
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mass (g (1) no. of moles(n) = molecular massg mol 3.207g 218.53 g mol- n 0.0146 moles n = 0.793 g n = 18 gmol- n 0.0440moles

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