Answer :
To determine the new molarity of the solution after dilution, we can use the dilution formula:
[tex]\[ M_1 \times V_1 = M_2 \times V_2 \][/tex]
Where:
- [tex]\( M_1 \)[/tex] is the initial molarity
- [tex]\( V_1 \)[/tex] is the initial volume
- [tex]\( M_2 \)[/tex] is the final molarity
- [tex]\( V_2 \)[/tex] is the final volume
Given:
- [tex]\( M_1 = 3 \, \text{M} \)[/tex]
- [tex]\( V_1 = 50 \, \text{mL} \)[/tex]
- [tex]\( V_2 = 100 \, \text{mL} \)[/tex]
We need to find the final molarity [tex]\( M_2 \)[/tex].
Rearranging the equation to solve for [tex]\( M_2 \)[/tex]:
[tex]\[ M_2 = \frac{M_1 \times V_1}{V_2} \][/tex]
Substituting the given values:
[tex]\[ M_2 = \frac{3 \, \text{M} \times 50 \, \text{mL}}{100 \, \text{mL}} \][/tex]
Calculating the above expression:
[tex]\[ M_2 = \frac{150 \, \text{M} \cdot \text{mL}}{100 \, \text{mL}} \][/tex]
[tex]\[ M_2 = 1.5 \, \text{M} \][/tex]
Therefore, the new molarity of the solution after dilution is [tex]\( 1.5 \, \text{M} \)[/tex], rounded to the tenths place.
So the answer is:
B. 1.5 M
[tex]\[ M_1 \times V_1 = M_2 \times V_2 \][/tex]
Where:
- [tex]\( M_1 \)[/tex] is the initial molarity
- [tex]\( V_1 \)[/tex] is the initial volume
- [tex]\( M_2 \)[/tex] is the final molarity
- [tex]\( V_2 \)[/tex] is the final volume
Given:
- [tex]\( M_1 = 3 \, \text{M} \)[/tex]
- [tex]\( V_1 = 50 \, \text{mL} \)[/tex]
- [tex]\( V_2 = 100 \, \text{mL} \)[/tex]
We need to find the final molarity [tex]\( M_2 \)[/tex].
Rearranging the equation to solve for [tex]\( M_2 \)[/tex]:
[tex]\[ M_2 = \frac{M_1 \times V_1}{V_2} \][/tex]
Substituting the given values:
[tex]\[ M_2 = \frac{3 \, \text{M} \times 50 \, \text{mL}}{100 \, \text{mL}} \][/tex]
Calculating the above expression:
[tex]\[ M_2 = \frac{150 \, \text{M} \cdot \text{mL}}{100 \, \text{mL}} \][/tex]
[tex]\[ M_2 = 1.5 \, \text{M} \][/tex]
Therefore, the new molarity of the solution after dilution is [tex]\( 1.5 \, \text{M} \)[/tex], rounded to the tenths place.
So the answer is:
B. 1.5 M
