Question

you want to determine the concentration when 93 ml of a 2.03 m kf solution is diluted by adding 3920 ml h₂o. m₁ = 2.03 m v₁ = 93 ml m₂ = ? m v₂ = 4013 ml m₁v₁ = m₂v₂ what is the molarity of the diluted solution? ? m molarity (m) submit

Explanation:

Step1: Recall dilution formula

We use the dilution formula \( M_1V_1 = M_2V_2 \), where \( M_1 \) is initial molarity, \( V_1 \) initial volume, \( M_2 \) final molarity, \( V_2 \) final volume.

Step2: Rearrange for \( M_2 \)

Rearrange the formula to solve for \( M_2 \): \( M_2=\frac{M_1V_1}{V_2} \)

Step3: Substitute values

Substitute \( M_1 = 2.03\space M \), \( V_1 = 93\space mL \), \( V_2 = 4013\space mL \) into the formula: \( M_2=\frac{2.03\times93}{4013} \)

Step4: Calculate numerator

Calculate \( 2.03\times93 = 188.79 \)

Step5: Divide to find \( M_2 \)

Divide \( 188.79\) by \( 4013 \): \( M_2\approx0.047 \)

Answer:

\( 0.047 \)