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joja [24]
3 years ago
8

A solution is prepared by dissolving 0.7234 g oxalic acid (H2C2O4) in enough water to make 100.0 mL of solution. A 10.00-mL aliq

uot (portion) of this solution is then diluted to a final volume of 250.0 mL. What is the final molarity of the diluted oxalic acid solution?
Chemistry
1 answer:
marishachu [46]3 years ago
8 0

Answer: The final molarity of the diluted oxalic acid solution is 0.0032 M

Explanation:

Molarity: It is defined as the number of moles of solute present per liter of the solution.

Formula used :

Molarity=\frac{n\times 1000}{V_s}

where,

n= moles of solute

Moles=\frac{\text{Given mass}}{\text{Molar mass}}=\frac{0.7234g}{90g/mol}=0.008moles

V_s = volume of solution in ml

Molarity=\frac{0.008\times 1000}{100.0}=0.08

To calculate the final molarity of the diluted oxalic acid solution

M_1V_1=M_2V_2

where,

M_1\text{ and }V_1 are the molarity and volume of concentrated oxalic acid solution.

M_2\text{ and }V_2 are the molarity and volume of diluted oxalic acid solution.

We are given:

M_1=0.08\\V_1=10.00mL\\M_2=?\\V_2=250.0mL

Putting values in above equation, we get:

0.08\times 10.00=M_2\times 250.0\\\\M_2=0.0032M

Thus the final molarity of the diluted oxalic acid solution is 0.0032 M

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