/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 55 Commercial aqueous nitric acid h... [FREE SOLUTION] | 91影视

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Chapter 13: Problem 55

Commercial aqueous nitric acid has a density of \(1.42 \mathrm{~g} / \mathrm{mL}\) and is \(16 \mathrm{M}\). Calculate the percent \(\mathrm{HNO}_{3}\) by mass in the solution.

Short Answer

Expert verified
The percent of HNO鈧� by mass in the commercial aqueous nitric acid solution is approximately 71.0%.

Step by step solution

01

Calculate the mass of 1 liter of solution

Given that the density of the solution is 1.42 g/mL, we can easily convert this value to grams per liter (1 L = 1000 mL): Density = 1.42 g/mL 脳 1000 mL/L = 1420 g/L So, the mass of 1 liter of the solution is 1420 g.
02

Calculate the moles of HNO鈧� in 1 liter of solution

The molarity of the solution is given as 16 M. This means that there are 16 moles of HNO鈧� in 1 liter of the solution.
03

Calculate the mass of HNO鈧� in 1 liter of solution

To calculate the mass of HNO鈧� in 1 liter of solution, we need to know its molar mass. The molar mass of HNO鈧� = 1.01 (for H) + 14.01 (for N) + 3 脳 16.00 (for O) = 63.02 g/mol. Now, we can calculate the mass of 16 moles of HNO鈧�: Mass of HNO鈧� = moles 脳 molar mass = 16 mol 脳 63.02 g/mol = 1008.32 g
04

Calculate the mass percent of HNO鈧� in the solution

Finally, we can use the mass of HNO鈧� and the mass of the solution to find the mass percent of HNO鈧� in the solution: Mass percent of HNO鈧� = (mass of HNO鈧� / mass of solution) 脳 100% Mass percent of HNO鈧� = (1008.32 g / 1420 g) 脳 100% 鈮� 71.0% The percent of HNO鈧� by mass in the commercial aqueous nitric acid solution is approximately 71.0%.

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Most popular questions from this chapter

Brass is a substitutional alloy consisting of a solution of copper and zinc. A particular sample of red brass consisting of \(80.0 \% \mathrm{Cu}\) and \(20.0 \% \mathrm{Zn}\) by mass has a density of \(8750 \mathrm{~kg} / \mathrm{m}^{3}\). (a) What is the molality of \(\mathrm{Zn}\) in the solid solution? (b) What is the molarity of \(\mathrm{Zn}\) in the solution?

Most fish need at least \(4 \mathrm{ppm}\) dissolved \(\mathrm{O}_{2}\) in water for survival. (a) What is this concentration in \(\mathrm{mol} / \mathrm{L}\) ? (b) What partial pressure of \(\mathrm{O}_{2}\) above water is needed to obtain \(4 \mathrm{ppm} \mathrm{O}_{2}\) in water at \(10^{\circ} \mathrm{C}\) ? (The Henry's law constant for \(\mathrm{O}_{2}\) at this temperature is \(1.71 \times 10^{-3} \mathrm{~mol} / \mathrm{L}\)-atm.)

(a) A sample of hydrogen gas is generated in a closed container by reacting \(2.050 \mathrm{~g}\) of zinc metal with \(15.0 \mathrm{~mL}\) of \(1.00 \mathrm{M}\) sulfuric acid. Write the balanced equation for the reaction, and calculate the number of moles of hydrogen formed, assuming that the reaction is complete. (b) The volume over the solution in the container is \(122 \mathrm{~mL}\). Calculate the partial pressure of the hydrogen gas in this volume at \(25^{\circ} \mathrm{C}\), ignoring any solubility of the gas in the solution. (c) The Henry's law constant for hydrogen in water at \(25^{\circ} \mathrm{C}\) is \(7.8 \times 10^{-4} \mathrm{~mol} / \mathrm{L}\)-atm. Estimate the number of moles of hydrogen gas that remain dissolved in the solution. What fraction of the gas molecules in the system is dissolved in the solution? Was it reasonable to ignore any dissolved hydrogen in part (b)? [13.111] The following table presents the solubilities of several gases in water at \(25^{\circ} \mathrm{C}\) under a total pressure of gas and water vapor of \(1 \mathrm{~atm}\). (a) What volume of \(\mathrm{CH}_{4}(\mathrm{~g})\) under standard conditions of temperature and pressure is contained in \(4.0 \mathrm{~L}\) of a saturated solution at \(25^{\circ} \mathrm{C}\) ? (b) Explain the variation in solubility among the hydrocarbons listed (the first three compounds), based on their molecular structures and intermolecular forces. (c) Compare the solubilities of \(\mathrm{O}_{2}, \mathrm{~N}_{2}\), and \(\mathrm{NO}\), and account for the variations based on molecular structures and intermolecular forces. (d) Account for the much larger values observed for \(\mathrm{H}_{2} \mathrm{~S}\) and \(\mathrm{SO}_{2}\) as compared with the other gases listed. (e) Find several pairs of substances with the same or nearly the same molecular masses (for example, \(\mathrm{C}_{2} \mathrm{H}_{4}\) and \(\mathrm{N}_{2}\) ), and use intermolecular interactions to explain the differences in their solubilities.

A textbook on chemical thermodynamics states, "The heat of solution represents the difference between the lattice energy of the crystalline solid and the solvation energy of the gaseous ions." (a) Draw a simple energy diagram to illustrate this statement. (b) \(\mathrm{A}\) salt such as \(\mathrm{NaBr}\) is insoluble in most polar nonaqueous solvents such as acetonitrile \(\left(\mathrm{CH}_{3} \mathrm{CN}\right)\) or nitromethane \(\left(\mathrm{CH}_{3} \mathrm{NO}_{2}\right)\), but salts of large cations, such as tetramethylammonium bromide \(\left[\left(\mathrm{CH}_{3}\right)_{4} \mathrm{NBr}\right]\), are generally more soluble. Use the thermochemical cycle you drew in part (a) and the factors that determine the lattice energy (Section 8.2) to explain this fact.

Caffeine \(\left(\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{O}_{2}\right)\) is a stimulant found in coffee and tea. If a solution of caffeine in the solvent chloroform \(\left(\mathrm{CHCl}_{3}\right)\) has a concentration of \(0.0500 \mathrm{~m}\), calculate (a) the percentage of caffeine by mass, (b) the mole fraction of caffeine in the solution.
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