- Home/
- CDS & Defence/
- Article
If the density of methanol is 0.793 kg/L, what is its volume needed for making 2.5L of its 0.25M solution?
By BYJU'S Exam Prep
Updated on: September 25th, 2023
If the density of methanol is 0.793 kg/L, its volume needed for making 2.5L of its 0.25M solution is 25.22 mL. Calculating the volume of methanol:
Step 1: Analysis of the data provided
- It is stated that methanol has a density of 0.793 kgL-1
- Volume of solution = 2.5 L
- Molarity of solution = 0.25 M
Calculations for methanol’s mass include:
CH3OH = 12 + (1 x 3) + 16 + 1 = 32u
Table of content
Step 2: estimating the volume of methanol required for the solution
Using the molarity formula, we can get the mass of methanol required for the solution as follows:
- Molarity = given mass/ molar mass x volume (L)
- 0.25 molL-1 = mass/ (32 g mol-1 x 2.5 L)
- Mass of methanol = 20 g = 0.20 Kg
Step 3: Volume of methanol Calculation Density is defined as the proportion of mass to volume.
As a result, the amount of methanol required can be calculated as follows:
- Volume = mass/density
- Volume = 0.2 Kg/ 0.793 Kg L-1
- Volume = 0.2522 L = 25.22 mL
Therefore, 25.22 mL is the amount of liquid required to make its 0.25 M solution in 2.5 L.
Summary:
If the density of methanol is 0.793 kg/L, what is its volume needed for making 2.5L of its 0.25M solution?
If methanol has a density of 0.793 kg/L, then 25.22 mL of methanol is required to make 2.5L of its 0.25M solution. The volume of methanol is defined as the ratio of mass by density in mL.