Question

What is the molarity of 30.0 mL of hydrochloric acid solution after 15.0 mL of a 3.00 M solution has been diluted?

___ M (Answer Format X.X)

Answer 1

1.00 M

Step-by-step explanation:

Molarity is defined as the number of moles of solute per liter of solution. When a solution is diluted, the number of moles of solute remains constant, but the volume of the solution increases. Therefore, the molarity of the solution decreases.

In this case, the initial number of moles of solute in the 15.0 mL of 3.00 M hydrochloric acid solution is (15.0 mL) * (3.00 mol/L) * (1 L/1000 mL) = 0.045 mol.

After dilution, the volume of the solution increases to 30.0 mL + 15.0 mL = 45.0 mL. The molarity of the diluted solution is (0.045 mol) / (45.0 mL) * (1000 mL/L) = 1.00 M.

So, the molarity of 30.0 mL of hydrochloric acid solution after 15.0 mL of a 3.00 M solution has been diluted is 1.00 M.

Answer 2

To find the molarity of the new solution, we need to use the equation:

M1V1 = M2V2

Where:

M1 = initial molarity = 3.00 M

V1 = initial volume = 15.0 mL

M2 = final molarity (what we're solving for)

V2 = final volume = 30.0 mL

Rearranging the equation to solve for M2:

M2 = (M1V1)/V2

M2 = (3.00 M * 15.0 mL)/30.0 mL

M2 = 1.50 M

Therefore, the molarity of the new solution is 1.50 M.