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 Normality & Equivalent Weight concept. If you need more Normality & Equivalent Weight practice, you can also practice Normality & Equivalent Weight 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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What textbook is this problem found in?

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.