you want to determine the concentration when 93 ml of a 2.03 m kf solution is diluted by adding 3920 ml h2o…

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

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

Answer

Explanation:

Step1: Identify the dilution formula

The formula for dilution is $M_1V_1 = M_2V_2$, where $M_1$ and $V_1$ are the initial molarity and volume, and $M_2$ and $V_2$ are the final molarity and volume.

Step2: Rearrange the formula to solve for $M_2$

We can rewrite the formula as $M_2=\frac{M_1V_1}{V_2}$.

Step3: Substitute the given values

Given $M_1 = 2.03\ M$, $V_1=93\ mL$, and $V_2 = 4013\ mL$. Substituting these values into the formula, we get $M_2=\frac{2.03\ M\times93\ mL}{4013\ mL}$.

Step4: Calculate the result

$M_2=\frac{2.03\times93}{4013}\ M=\frac{188.79}{4013}\ M\approx0.047\ M$.

Answer:

$0.047$