Question

In the laboratory, a student adds 55.7 mL of water to 17.6 mL of a 0.718 M hydrobromic acid solution. What is the concentration of the diluted solution

Answer 1

Answer: The concentration of the diluted solution is 0.17M.

Explanation:

The equation for diluted solutions is shown as: $M_{s} V_{s} =M_{d} V_{d}$.

~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!

$0.718M*17.6mL=M_{d} *73.3mL$

(I put $V_{d}$ as 73.3 because you are adding 55.7mL to 17.6mL, meaning that you have to add that to get $V_{d}$. In other words, $17.6mL+55.7mL=73.3mL$)

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.

$17.6mL/1000=0.0176L$     $73.3mL/1000=0.0733L$

Now that we have both volumes in liters, we can plug them in correctly.

$0.178M*0.0176L=M_{d} *0.0733L$

$M_{d} =\frac{0.718M*0.0176L}{0.0733L}$     $M_{d} =0.17M$

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!! :)