Problem: A 1.37-M solution of citric acid (H3C6H5O7) in water has a density of 1.10 g/cm3. Calculate the mass percent, molality, mole fraction, and normality of the citric acid. Citric acid has three acidic protons.

FREE Expert Solution

The molar mass of citric acid is 192.124 g/mol.

The molar mass of water is 18.016 g/mol.

In mass percent:

mass percent=mass solutemass solution×100

mass solute=(1.00 L)(1.37 molL)(192.124 g1 mol)=263.21 g

mass solvent=1 L(1 mL10-3 L)(1 cm31 mL)(1.10gcm3)=1,100 g

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Problem Details

A 1.37-M solution of citric acid (H3C6H5O7) in water has a density of 1.10 g/cm3. Calculate the mass percent, molality, mole fraction, and normality of the citric acid. Citric acid has three acidic protons.

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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 Mole Fraction concept. You can view video lessons to learn Mole Fraction. Or if you need more Mole Fraction practice, you can also practice Mole Fraction practice problems.

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

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.