Respuesta :
We can use the equation for dilutions that relates concentration and volume:
[tex]M_1V_1=M_2V_2[/tex]
where M is the molarity, V is the volume, and 1 and 2 refer to the initial and final states of the solution, respectively. Here, we are given the molarity of the initial solution and the volumes of the initial and final (diluted) solutions. To find the final concentration (i.e., the molarity of the diluted solution), we would be solving for Mā:
[tex]M_2=\frac{M_1V_1}{V_2} = \frac{(0.55 \text{ M})(145 \text{ mL})}{250 \text{ mL}} \\ M_2 = 0.319 \approx 0.32 \text{ M}.[/tex]
The molarity is given to two significant figures as both our Mā and Vā are given to two significant figures.
Note: Although our volumes are in mL instead of L, we do not need to convert them to L for the purposes of our calculation since we would be multiplying our Vā and Vā by a common factor that would cancel out in division. All that matters is the ratio between the two volumes, which is the same whether the volumes are in mL or in L.
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We follow the exact same procedure in the second question as we did in the first problem: solve for Mā given Mā = 9.02 M, Vā = 35.0 mL, and Vā = 45.0 mL:
[tex]M_2=\frac{M_1V_1}{V_2} = \frac{(9.02 \text{ M})(35.0 \text{ mL})}{45.0 \text{ mL}} \\ M_2 = 7.02 \text{ M}.[/tex]