[Krishen]

Hi all.

First question:

Calculate the molarity, normality, and molality of a sulfuric acid solution containing 27% H2SO4 by mass. (MW 98.0 G/mol). The sulfuric acid solution has a density of 1.198 g/mL. Assume both acidic protons react.

The density is throwing me off on this question.

Second Question: The Ksp for SrF2 at 25 degrees C is 2.8 x 10^-9. What are the [Sr2+] and [F-] in a saturated solution of SrF2? Demonstrate your understanding of the Common Ion effect using this solution.

I'm just not sure how to do this...I thought I may need more information.

Any help on either would be appreciated.

[Borek]

Calculate the molarity, normality, and molality of a sulfuric acid solution containing 27% H2SO4 by mass. (MW 98.0 G/mol). The sulfuric acid solution has a density of 1.198 g/mL. Assume both acidic protons react.

http://www.chembuddy.com/?left=concentration&right=toc

http://www.chembuddy.com/?left=concentration&right=percentage-to-molarity

http://www.chembuddy.com/?left=concentration&right=percentage-to-molality

http://www.chembuddy.com/?left=concentration&right=normality

Second Question: The Ksp for SrF2 at 25 degrees C is 2.8 x 10^-9. What are the [Sr2+] and [F-] in a saturated solution of SrF2? Demonstrate your understanding of the Common Ion effect using this solution.

Start with the reaction equation. Write formula for Kso.