Question

Your lab partner told you that he measured out 25.0 mL of the unknown acid solution. But he actually went above the line on the graduated cylinder (added more than 25.0 mL). Would your final calculated molarity of the unknown acid be higher, lower or equal to the actual concentration

Answer 1

Answer:

Final calculated molarity of the unknown acid be  lower than the actual concentration.

Explanation:

Volume required unknown acid = V= 25.0 mL

Volume actually measure was more than V that is = V'

V' > V

Molarity of the solution is the moles of compound in 1 Liter solutions.

$Molarity=\frac{\text{Mass of compound}}{\text{Molar mas of compound}\times Volume (L)}$

As we can see from the formula that molarity is inversely proportional to the volume of the solution.

$Molarity\propto \frac{1}{Volume}$

• Molarity of solution decreases with increase in volume
• Molarity of solution Increases with decrease in volume.

We have added more volume than required which will be increase the volume of solution and the molarity of the solution will lower than the actual value.