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 Ritesh|Updated : November 4th, 2022

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

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.

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