Respuesta :
Answer: The volume of solution A required is 0.15 L
Explanation:
To calculate the molarity of solution, we use the equation:
[tex]\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}[/tex] .......(1)
- For Solution B:
Molarity of solution B = 0.60 M
Volume of solution B = 50.0 mL = 0.050 L (Conversion factor: 1 L = 1000 mL)
Putting values in equation 1, we get:
[tex]0.60M=\frac{\text{Moles of solution B}}{0.050L}\\\\\text{Moles of solution B}=(0.60mol/L\times 0.050L)=0.003mol[/tex]
Now, calculating the volume of solution A required for the same number of moles as solution B.
Moles of solution A = 0.003 moles
Molarity of solution A = 0.020 M
Putting values in equation 1, we get:
[tex]0.020M=\frac{0.003mol}{\text{Volume of solution A}}\\\\\text{Volume of solution A}=\frac{0.003}{0.02}=0.15L[/tex]
Hence, the volume of solution A required is 0.15 L
0.15 liters of solution A are needed to contain the same number of moles as the 50.0 mL of solution B.
What is a solution?
A solution is a mixture of solute to the solvent.
Solution A is 5.0L at 0.020M
Solution B is 50.0 mL at 0.60M.
Volume of solution B is 50.0 mL = 0.050 L
Step 1: Calculate the molarity of the solution
[tex]\begin{aligned} M &= \dfrac{n}{V}\\0.60\;M &=\dfrac{moles\;of \;sol\;B}{0.050\;L} \end{aligned}\\\\Moles\;of \;sol\;B = 0.60\;mol\times 0.050\;L = 0.003 \;mol[/tex]
Step 2: Calculating the volume of solution A required for the same number of moles as solution B.
Moles of solution A = 0.003 moles
Molarity of solution A = 0.020 M
From 1 equation
[tex]0.020M &=\dfrac{0.003\;mol}{Volume\;of\;soluiton\;A} \\\\\\Volume\;of\;soluiton\;A =\dfrac{0.003\;mol}{0.02}= 0.15\;l[/tex]
Thus, the volume of solution A, needed, is 0.15 L.
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