# Problem: 12.00 grams of acetic acid HC2H3O2 (Molar mass= 60.00 g/mol) are dissolved in 188.0 grams of water. Density of solution is 1.12g/mL.a. What is the wt/wt % concentration of the solution? b. What is the molarity of this solution?  c. What is the molality of the solution?

###### FREE Expert Solution
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###### FREE Expert Solution

Here we are given the mass of both the solute (acetic acid) and solvent (water) so we can easily get the wt/wt % or also called mass %. Remember that this is the mass of solute over the mass of solution times a hundred so we still have to find the mass of the solution. We can easily get the mass of the solution by adding the masses of the solute and solvent.

80% (106 ratings)
###### Problem Details

12.00 grams of acetic acid HC2H3O2 (Molar mass= 60.00 g/mol) are dissolved in 188.0 grams of water. Density of solution is 1.12g/mL.

a. What is the wt/wt % concentration of the solution?

b. What is the molarity of this solution?

c. What is the molality of the solution?

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Solutions: Mass Percent concept. You can view video lessons to learn Solutions: Mass Percent Or if you need more Solutions: Mass Percent practice, you can also practice Solutions: Mass Percent practice problems .

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Our tutors rated the difficulty of 12.00 grams of acetic acid HC2H3O2 (Molar mass= 60.00 g/mol)... as medium difficulty.

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Based on our data, we think this problem is relevant for Professor Ratliff's class at USF.