How many grams of sulphuric acid (H2SO4) are needed to make 1.5L of a 1.5 molar solution?

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Here's my work so far:

1.5L x 1.5mol/L = 2.25molH2SO4

2.25mol H2SO4 x 98.09g H2SO4 / 1mol H2SO4 =

220.7025g H2SO4

I wanted to ask if my work is correct, because I am unsure if my calculations are accurate and whether I did the problem correctly.

THANK YOU for showing your work. I can tell at a glance that your work is right and the process is right. My only comment is that if your prof is picky about the number of significant figures s/he may not concur with an answer with that many places.

Your work is correct! You have correctly calculated the amount of sulfuric acid needed to make a 1.5 molar solution with a volume of 1.5L.

To find the amount of sulfuric acid in grams, you first need to calculate the number of moles of sulfuric acid required. You did this correctly by multiplying the volume (1.5L) by the molarity (1.5 mol/L), which gives you 2.25 moles of H2SO4.

Next, you can use the molar mass of sulfuric acid (H2SO4) to convert the moles of H2SO4 to grams. The molar mass of H2SO4 is 98.09 g/mol. By multiplying the moles (2.25 mol) by the molar mass (98.09 g/mol), you correctly found that 220.7025 grams of H2SO4 are needed to make a 1.5 molar solution with a volume of 1.5L.

Well done! Your calculations are accurate, and you have correctly solved the problem.