Calculate the mass of CH3COOH present in 200ml of 0.5 molar solution?
Answers
Answer:
6
Explanation:
0.5=(g.m×1000)/(m.m×vol in ml)
Concept:
Molarity: The molarity of a solution is defined as the number of moles of solute dissolved per unit volume of the solution. It is denoted by M and is given by,
M = n/V
where n = Number of moles of solute
V = Volume of the solution
Number of moles of the solute is given by,
n = m/W
where m = Mass of the solute in grams
W = Molecular mass of the solute
Given:
Molarity, M = 0.5 M
Volume of the solution, V = 200 mL = 0.2 L
Solute = Acetic acid = CH₃COOH
Find:
Mass of CH₃COOH present in 200 mL of 0.5 molar solution.
Solution:
First of all, we will calculate the molecular mass of the solute.
Molecular mass of CH₃COOH = Atomic mass of C + 3×Atomic mass of H + Atomic mass of C + Atomic mass of O + Atomic mass of O + Atomic mass of H
Molecular mass of CH₃COOH, W = 12 + 3(1) + 12 + 16 + 16 + 1
W = 60 g mol⁻¹
Molarity, M = 0.5 [Given]
Let number of moles be n.
Volume, V = 0.2 L
As we know,
M = n/V
0.5 = n/0.2
n = 0.5×0.2
n = 0.1
Now, Number of moles, n = 0.1
Let the mass of CH₃COOH be m.
Number of moles, n = m/W
0.1 = m/60
m = 0.1×60
m = 6 g
∴ Mass of CH₃COOH, m = 6 g
Hence, the mass of CH₃COOH present in 200 mL of 0.5 molar solution is 6 grams.
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