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?Balance the following equations: (a) \(\mathrm{Ca}_{3} \mathrm{P}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ca}(\mathrm{OH}

Chemistry: The Central Science | 14th Edition | ISBN: 9780134414232 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus ISBN: 9780134414232 1274

Solution for problem 3.14 Chapter 3

Chemistry: The Central Science | 14th Edition

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Chemistry: The Central Science | 14th Edition | ISBN: 9780134414232 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus

Chemistry: The Central Science | 14th Edition

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Problem 3.14

Balance the following equations:

(a) \(\mathrm{Ca}_{3} \mathrm{P}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{PH}_{3}(g)\)

(b) \(\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\)

(c) \(\mathrm{AgNO}_{3}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \longrightarrow \mathrm{Ag}_{2} \mathrm{CO}_{3}(s)+\mathrm{NaNO}_{3}(a q)\)

(d) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{N}_{2}(g)\)

Text Transcription:

Ca3P2(s) + H2O(l) \longrightarrow Ca(OH)2(aq) + PH3(g)

Al(OH)3(s) + H2SO4(aq) \longrightarrow Al2(SO4)3(aq) + H2O(l)

AgNO3(aq) + Na2CO3(aq) \longrightarrow Ag2CO3(s) + NaNO3(aq)

C2H5NH2(g) + O2(g) \longrightarrow CO2(g) + H2O(g) + N2(g)

Step-by-Step Solution:

Step 1 of 5) General Properties of Aqueous Solutions A solution is a homogeneous mixture of two or more substances. (Section 1.2) The substance present in the greatest quantity is usually called the solvent, and the other substances are called solutes; they are said to be dissolved in the solvent. When a small amount of sodium chloride (NaCl) is dissolved in a large quantity of water, for example, water is the solvent and sodium chloride is the solute.Electrolytes and Nonelectrolytes At a young age we learn not to bring electrical devices into the bathtub so as not to electrocute ourselves. That is a useful lesson because most of the water we encounter in daily life is electrically conducting. Pure water, however, is a very poor conductor of electricity. The conductivity of bathwater originates from the substances dissolved in the water, not from the water itself. Not all substances that dissolve in water make the resulting solution conducting. Figure 4.2 shows a simple experiment to test the electrical conductivity of three solutions: pure water, a solution of table sugar (sucrose) in water, and a solution of table salt (NaCl) in water. A light bulb is connected to a battery-powered electrical circuit that contains two electrodes submerged in a beaker of each solution. In order for the light bulb to turn on, there must be an electrical current (that is, a flow of electrically charged particles) between the two electrodes immersed in the solution. Because the light bulb does not turn on in pure water, we conclude that there are not enough charged particles in pure water to

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Chapter 3, Problem 3.14 is Solved
Textbook: Chemistry: The Central Science
Edition: 14
Author: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
ISBN: 9780134414232

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?Balance the following equations: (a) \(\mathrm{Ca}_{3} \mathrm{P}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ca}(\mathrm{OH}