If 18.4 mL of a 1.37 M aqueous KCl solution was placed in a 150-mL volumetric flask and water was added to dilute to the mark, after mixing, how many moles of KCl would be in the flask?

Question

If 18.4 mL of a 1.37 M aqueous KCl solution was placed in a 150-mL volumetric flask and water was added to dilute to the mark, after mixing, how many moles of KCl would be in the flask?

(with correct number of sig figs)

Answer 1

mols = M x L = 1.37 x 0.0184 = ? You can have 3 significant figures in the answer.

Answer 2

To find the number of moles of KCl in the flask, we can use the equation:

moles = concentration (M) x volume (L)

First, we need to convert the initial volume of KCl solution from mL to L:

18.4 mL = 18.4 mL * (1 L / 1000 mL) = 0.0184 L

Now, we can multiply the volume by the concentration to find the number of moles:

moles = 0.0184 L x 1.37 M = 0.025168 mol

However, we need to consider the significant figures. Both the volume and the concentration are given to three significant figures, so the answer should also be expressed to three significant figures. Therefore, the number of moles of KCl in the flask is 0.0252 mol.