A 6.00 M H2SO4 solution has d = 1.34 g/mL. What is the mass percent of H2SO4 in this solution?

Choose one answer.
a. 56.1
b. 43.9
c. 37.0
d. 58.8

When we calculated yesterday the answer was not B. 43.9....I got it wrong and don't know why if the math was correct and I followed the steps you showed me.

I think the answer is 43.9% H2SO4. I looked this up in a VERY OLD text book, back in the days when they printed such stuff in texts (you can't find it these days in texts) and they show %H2SO4 = 43.74% for a density of 1.340 g/mL. (They don't show that as 6.00 M but we could calculate it and find it is 5.97 M.)

To find the mass percent of H2SO4 in the solution, we need to use the equation:

mass percent = (mass of H2SO4 / mass of solution) * 100

First, let's calculate the mass of the solution. We have the density and volume of the solution, so we can use the equation:

mass of solution = density * volume

The volume of the solution is not given, so we're missing a key piece of information to proceed. In the absence of the volume, it's not possible to accurately determine the mass percent of H2SO4 in the solution. Therefore, we cannot determine the correct answer among the given options (a. 56.1, b. 43.9, c. 37.0, d. 58.8).

Regarding your previous question, if you followed the correct steps and performed the calculations accurately, the answer should have been correct. If you can provide the details of the question and your calculations, I can help identify any potential errors.