If the density of methanol is 0.793 kgL^-1 , what is the volume needed for making 2.5 L of its 0.25 M solution?
If the density of methanol is 0.793 kgL-1 , what is the volume needed for making 2.5 L of its 0.25 M solution?
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Let us calculate moles of methanol present in 2.5 L of 0.25 M solution.
Molarity = Moles of CH3OH /Volume in L
0.25 = Moles of CH3OH/2.5
Moles of CH3OH = 0.25 x 2.5 = 0.625 moles
Mass of CH3OH = 0.625 x 32 = 20 g
(Molecular mass of CH3OH = 32)
Now 0.793 x 103 g of CH3OH is present in 1000 mL
20 g of CH3OH will be present in = 1000/ 0.793 x 103 x 20 = 25.2 mL
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