Answer: The concentration of the diluted solution is 0.17M.
Explanation:
The equation for diluted solutions is shown as: [tex]M_{s} V_{s} =M_{d} V_{d}[/tex].
~M= Molarity (labeled as M)
~V=Volume (in L)
~s= stock solution (what you started with)
~d= diluted solution (what you finish with)
Now that we have that down, let's plug in our data!
[tex]0.718M*17.6mL=M_{d} *73.3mL[/tex]
(I put [tex]V_{d}[/tex] as 73.3 because you are adding 55.7mL to 17.6mL, meaning that you have to add that to get [tex]V_{d}[/tex]. In other words, [tex]17.6mL+55.7mL=73.3mL[/tex])
There is a little problem here though. The volume is not in liters. But no worries, we can just convert it by dividing it by 1000.
[tex]17.6mL/1000=0.0176L[/tex] [tex]73.3mL/1000=0.0733L[/tex]
Now that we have both volumes in liters, we can plug them in correctly.
[tex]0.178M*0.0176L=M_{d} *0.0733L[/tex]
[tex]M_{d} =\frac{0.718M*0.0176L}{0.0733L}[/tex] [tex]M_{d} =0.17M[/tex]
With all of this shown, we now know that the concentration of the diluted solution is 0.17M.
I hope this helps! Pls mark brainliest!! :)
