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Chapter 21: Problem 10

Write the formula for the following compounds. (a) sodium azide (b) sulfurous acid (c) hydrazine (d) sodium dihydrogen phosphate

Short Answer

Expert verified
Answer: The chemical formulas for the given compounds are: (a) NaN3, (b) H2SO3, (c) N2H4, and (d) Na2H2PO4.

Step by step solution

01

(a) Sodium azide

First, we need to identify the components in sodium azide. Sodium is a metal (Na) and has a +1 charge. Azide is a polyatomic ion (N3) and has a -1 charge. Since the charges are equal and opposite, we can simply combine the two ions to create the neutral compound, NaN3.
02

(b) Sulfurous acid

Sulfurous acid is an oxyacid, which means that it contains hydrogen, sulfur, and oxygen. The "sulfurous" part of the name indicates that it contains a sulfite ion (SO3) with a -2 charge. The "acid" part of the name indicates that it contains hydrogen ions (H+). To make the compound neutral, we need two hydrogen ions for each sulfite ion. Therefore, the chemical formula for sulfurous acid is H2SO3.
03

(c) Hydrazine

Hydrazine is a simple inorganic compound containing nitrogen and hydrogen. The prefix "hydra" means that it contains hydrogen, and "azine" refers to the presence of nitrogen. Hydrazine has the chemical formula N2H4, which means it contains two nitrogen atoms and four hydrogen atoms.
04

(d) Sodium dihydrogen phosphate

The compound sodium dihydrogen phosphate contains three different ions: sodium (Na+), hydrogen (H+), and phosphate (PO4). The "dihydrogen" in the name indicates that there are two hydrogen ions, and the "phosphate" part of the name denotes the presence of the phosphate ion, which has a -3 charge. The sodium ion has a +1 charge. To make the compound neutral, we need two sodium ions for each dihydrogen phosphate ion. Therefore, the chemical formula for sodium dihydrogen phosphate is Na2H2PO4.

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Most popular questions from this chapter

Write a balanced net ionic equation for the reaction of nitric acid with (a) a solution of \(\mathrm{Ca}(\mathrm{OH})_{2}\). (b) \(\mathrm{Ag}(s)\); assume the nitrate ion is reduced to \(\mathrm{NO}_{2}(g)\) (c) \(\mathrm{Cd}(s)\); assume the nitrate ion is reduced to \(\mathrm{N}_{2}(g)\).

Give the Lewis structure of (a) the strongest oxoacid of bromine. (b) a hydrogen compound of nitrogen in which there is an \(-\mathrm{N}-\mathrm{N}-\) bond. (c) an acid added to cola drinks.

Consider the reduction of nitrate ion in acidic solution to nitrogen oxide \(\left(E_{\mathrm{red}}^{\circ}=0.964 \mathrm{~V}\right)\) by sulfur dioxide that is oxidized to sulfate ion \(\left(E_{\text {red }}^{o}=0.155 \mathrm{~V}\right)\). Calculate the voltage of a cell involving this reaction in which all the gases have pressures of \(1.00 \mathrm{~atm}\), all the ionic species (except \(\left.\mathrm{H}^{+}\right)\) are at \(0.100 M\), and the \(\mathrm{pH}\) is \(4.30 .\)

A \(1.500-\mathrm{g}\) sample containing sodium nitrate was heated to form \(\mathrm{NaNO}_{2}\) and \(\mathrm{O}_{2}\). The oxygen evolved was collected over water at \(23^{\circ} \mathrm{C}\) and \(752 \mathrm{~mm} \mathrm{Hg}\); its volume was \(125.0 \mathrm{~mL}\). Calculate the percentage of \(\mathrm{NaNO}_{3}\) in the sample. The vapor pressure of water at \(23^{\circ} \mathrm{C}\) is \(21.07 \mathrm{~mm} \mathrm{Hg}\).

If an electrolytic cell producing fluorine uses a current of \(7.00 \times 10^{3} \mathrm{~A}\) (at \(10.0 \mathrm{~V})\), how many grams of fluorine gas can be produced in two days (assuming that the cell operates continuously at \(95 \%\) efficiency)?
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