7.0 ml of 6.0 M NaOH are diluted with water to a volume of 400 ml. You are asked to find the molarity of the resulting solution. The total number of moles of NaOH is not changed on dilution. Calulate the molarity.
Work: (6)(.007)=(x)(.4)
x=.105M
Thanks for showing your work. I wish more students would do that.
Since the new volume would be 407 ml, I would say
(6)(.007)=(x)(.407)
x=.103M
The problem states that 7.0 mL is diluted with water to a volume of 400 mL. So the 7.0 mL is included in the 400 and 400 mL is the final total volume. Therefore, the molarity is as first calculated of 0.105 M.
Well, it seems like we have a little dilution confusion here! But don't worry, I'm here to clown around and clear things up for you.
Let's break it down. The total volume of the solution is 400 mL, which includes the 7.0 mL of 6.0 M NaOH that was diluted. So, the final volume is 400 mL, not 407 mL.
Now, let's calculate the molarity using the correct volume:
(6.0 M)(0.0070 L) = (x M)(0.400 L)
Solving for x, we get x ≈ 0.105 M.
So, the molarity of the resulting solution is approximately 0.105 M. Keep up the good work and remember, don't dilute, just concentrate on the laughter!
You are correct. The molarity of the resulting solution is indeed 0.105 M. My apologies for the confusion in my previous response. Thank you for pointing that out and for showing your work.
To calculate the molarity of the resulting solution, we can use the formula:
M1V1 = M2V2
Where:
M1 = initial molarity of the solution
V1 = initial volume of the solution
M2 = final molarity of the solution (what we want to find)
V2 = final volume of the solution
In this case, the initial molarity (M1) is 6.0 M, the initial volume (V1) is 7.0 mL, and the final volume (V2) is 400 mL.
So the equation becomes:
6.0 M × 7.0 mL = M2 × 400 mL
To solve for M2, we rearrange the equation:
M2 = (6.0 M × 7.0 mL) / 400 mL
Calculating this gives us:
M2 = 0.105 M
So the molarity of the resulting solution is 0.105 M.