Wednesday

April 1, 2015

April 1, 2015

Posted by **Kevin** on Thursday, January 13, 2011 at 12:15am.

1.Calculate the volume of concentrated H2SO4 needed to make 1.00L of 5.20 molar solution.

2.Calculate the % concentration H2SO4 in the concentrated solution.

3.Calculate the volume of 5.20 molar H2SO4 required to react completely with 100.0 grams of NaHCO3. (Carbon dioxide and water are two of the three products of this reaction-can you figure out the other?)

4.What is the molality of the 5.20 molar H2SO4 solution?

I understand 3 and 4.

1 I don't understand mL x M = mL x M ??

2. Is number 2. (1803.2/1840)x100=98%H2SO4

- ChemistryDrBob222 -
**DrBob222**, Thursday, January 13, 2011 at 5:21pmmL x M = mL x M is the dilution formula.

mL of the concd acid is the unknown.

M of the concd acid is 18.4 M

mL of the diluted solution is 1,000 mL (you want 1.00 L). M of the diluted solution is 5.20M. Solve for the only unknown which is mL of the concd acid you need to use to dilute to 1.00 L to make the 5.20L..

Yes, it is 98% H2SO4.

This post is so far down that any follow up questions should be directed at the top of the page (make a new post that is) so someone will see it sooner.

**Answer this Question**

**Related Questions**

ChemistryDrBob222 - Concentrated sulfuric acid is 18.4 molar and has a density ...

Chemistry - Concentrated sulfuric acid is 18.4 molar and has a density of 1.84 ...

Chemistry - Concentrated sulfuric acid is 18.4 molar and has a density of 1.84 ...

science - Concentrated sulfuric acid (18.4 molar H2SO4) has a density of 1.84 ...

Chemistry - A student makes a solution by dissolving 55.8 grams of potassium ...

Chemistry - A student makes a solution by dissolving 55.8 grams of potassium ...

Chemistry - A student makes a solution by dissolving 55.8 grams of potassium ...

Chemistry - A student makes a solution by dissolving 55.8 grams of potassium ...

chemistry - The density of sulfuric acid, is 15.28 lb/gal. What is the density ...

Chemistry- Drbob-help - I have placed the answer I got please help. A student ...