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Chapter 4: Problem 46

Phosphorus forms many oxoacids. Indicate the oxidation number of phosphorus in each of the following acids: (a) \(\mathrm{HPO}_{3},\) (b) \(\mathrm{H}_{3} \mathrm{PO}_{2},\) (c) \(\mathrm{H}_{3} \mathrm{PO}_{3}\), (d) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (e) \(\mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7},\) (f) \(\mathrm{H}_{5} \mathrm{P}_{3} \mathrm{O}_{10}\)

Short Answer

Expert verified
The oxidation numbers of phosphorous in the given compounds are: \n (a) HPO3: 5, (b) H3PO2: 1, (c) H3PO3: 3, (d) H3PO4: 5, (e) H4P2O7: 5, (f) H5P3O10: 5.

Step by step solution

01

Determine the oxidation state of Hydrogen and Oxygen

In oxoacids, hydrogen generally has an oxidation state of +1 and oxygen has an oxidation state of -2.
02

Establish the Total Oxidation State of the Compound

For neutral molecules, the sum of the oxidation numbers is zero.
03

Find the Oxidation Number of Phosphorus in HPO3

For HPO3, phosphorus's oxidation number is the unknown. We established that the total oxidation state is 0. The equation to solve would be: +1(P)+ x(H) + (-6)(O) = 0. Solving for x, we get x=5, where x is the oxidation number of phosphorus.
04

Find the Oxidation Number of Phosphorus in H3PO2

For H3PO2, solve the equation: 3(+1) + x + 2(-2) = 0. Solving for x, it is found that x = 1.
05

Find the Oxidation Number of Phosphorus in H3PO3

For H3PO3, solve the equation: 3(+1) + x + 3(-2) = 0. Solving for x, we get x = 3.
06

Find the Oxidation Number of Phosphorus in H3PO4

For H3PO4, solve the equation: 3(+1) + x + 4(-2) = 0. Solving for x, we get x = 5.
07

Find the Oxidation Number of Phosphorus in H4P2O7

For H4P2O7, solve the equation: 4(+1) + 2x + 7(-2) = 0. Solving for x, we get x = 5.
08

Find the Oxidation Number of Phosphorus in H5P3O10

For H5P3O10, solve the equation: 5(+1) + 3x + 10(-2) = 0. Solving for x, we get x = 5.

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Most popular questions from this chapter

A \(60.0-\mathrm{mL} 0.513 \mathrm{M}\) glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) solution is mixed with \(120.0 \mathrm{~mL}\) of \(2.33 \mathrm{M}\) glucose solution. What is the concentration of the final solution? Assume the volumes are additive.

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The molar mass of a certain metal carbonate, \(\mathrm{MCO}_{3}\), can be determined by adding an excess of \(\mathrm{HCl}\) acid to react with all the carbonate and then "back titrating" the remaining acid with a \(\mathrm{NaOH}\) solution. (a) Write an equation for these reactions. (b) In a certain experiment, \(20.00 \mathrm{~mL}\) of \(0.0800 \mathrm{M} \mathrm{HCl}\) were added to a 0.1022 -g sample of \(\mathrm{MCO}_{3}\). The excess HCl required \(5.64 \mathrm{~mL}\) of \(0.1000 \mathrm{M} \mathrm{NaOH}\) for neutralization. Calculate the molar mass of the carbonate and identify \(\mathrm{M}\).
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