If the density of methanol is 0.793 kg L–1, what is its volume needed for making 2.5 L of its 0.25 M solution?
Let the volume of 0.25 M of ethanol needed = x Molar mass of methanol (CH3OH) = (1 × 12) + (4 × 1) + (1 × 16) = 32 g mol–1 = 0.032 kg mol–1
Molarity of methanol solution
= 24.78 mol L–1 (Since density is mass per unit volume)
Applying, M1V1 = M2V2
(Given solution) (Solution to be prepared)
(24.78 mol L–1) x = (2.5 L) (0.25 mol L–1)
x = 0.0252 L
x = 25.22 mL
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Not clearly explain step by step
no i dont like it
In the first step u wrote ethanol ð
Thanks
Thanks a lot
Great solution
Can u please explain how you get the molarity