We’re being asked to calculate for the normality of the H_{3}PO_{4} solution and determine the equivalent mass of the acid.

**Normality (N)** represents the number of equivalents per liter of solution.

$\overline{){\mathbf{N}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{\mathbf{equivalents}\mathbf{}\mathbf{of}\mathbf{}\mathbf{solution}}{\mathbf{L}\mathbf{}\mathbf{solution}}}$

$\overline{){\mathbf{equivalents}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{n}}{\mathbf{\times}}{\mathbf{moles}}}$

Calculate the normality of each of the following solutions.

c. 5.3 x 10^{-2} *M* H_{3}PO_{4}

What is the equivalent mass for each of the acids or bases listed above?

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Our tutors have indicated that to solve this problem you will need to apply the Weak Acids concept. If you need more Weak Acids practice, you can also practice Weak Acids practice problems.

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Our tutors rated the difficulty of*Calculate the normality of each of the following solutions.c...*as medium difficulty.

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