Chapter 9: Solutions

What is the final volume, in milliliters, when $25.0\mathrm{mL}$of each of the following solutions is diluted to provide the given concentration? $(9.5)$

a. $10\%(\mathrm{m}/\mathrm{v})\mathrm{HCl}$solution to give a $2.50\%(\mathrm{m}/\mathrm{v})\mathrm{HCl}$solution.

b. $5.00\mathrm{M}\mathrm{HCl}$solution to give a$1.00\mathrm{M}\mathrm{HCl}$ solution

c. $6.00\mathrm{M}\mathrm{HCl}$solution to give a $0.500\mathrm{M}\mathrm{HCl}$solution

In the following diagram, blue spheres represent the element $A$and yellow spheres represent the element $B$.

a. Write the formulas for each of the reactants and products.

b. Write a balanced chemical equation for the reaction.

c. Indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

Automobile exhaust is a major cause of air pollution. One pollutant is the gas nitrogen oxide, which forms from nitrogen and oxygen caves in the air of the high temperatures in an automobile engine. Once emitted into the air, nitrogen oxide reacts with oxygen to produce nitrogen dioxide, a reddish brown gas with a sharp, pungent odor that makes up smog. One component of gasoline is heptane. ${\mathrm{C}}_7{\mathrm{H}}_{16+}$a liquid which a density of$0.684$g/mL. In one year, a typical automobile uses $550\mathrm{gal}$of gasoline and produces 411 of nitrogen oxide. (7.4. 7.8.8.6)

a. Write balanced chemical equations for the production of nitrogen oxide and nitrogen dioxide.

b. If all the nitrogen oxide emitted by one automobile is converted to nitrogen dioxide in the atmosphere, how many kilograms of nitrogen dioxide are produced in one year by a single automobile?

c. Write a balanced chemical equation for the combustion of heptane.

d. Horn many moles of gaseous ${\mathrm{CO}}_2$are produced from the gasoline used by the typical automobile in one year, assuming the gasoline is all heptane?

e. How many liters of carbon dioxide at $TP$ are produced in one year from the gasoline used by the typical automobile?

Bleach is often added to a wash to remove stains from clothes, The active ingredient in bleach is sodium hypochlorite (NaClO). A bleach solution can be prepared by bubbling chlorine gas into a solution of sodium hydroxide to produce liquid water and an aqueous solution of sodium hypochlorite and sodium chloride. A typical bottle of bleach has a volume of$1.42\mathrm{gal}$, with a density of$1.08\mathrm{g}/\mathrm{mL}$and contains $282\mathrm{g}$of $\mathrm{NaClO},(6.2,6.3,7.4,7.8,8.6,9.4)$

a. Is sodium hypochlorite an ionic or a molecular compound?

b. What is the mass/volume percent $(\mathrm{m}/\mathrm{v})$of sodium hypochlorite in the bleach solution?

c. Write a balanced chemical equation for the preparation of a bleach solution.

d. How many liters of chlorine gas at STP are required to produce one bottle of bleach?

a. If black spheres are carbon atoms, white spheres are hydrogen atoms, and red spheres are oxygen atoms, what is the molecular formula of butyric acid?

b. What is the molar mass of butyric acid?

c. How many grams of butyric acid contain $3.28\times {10}^{23}$atoms of oxygen?

d. How many grams of carbon are in 5.28g of butyric acid?

e. Butyric acid has a density of 0.959 g/ml. How many moles of butyric acid are contained in 1.56 ml of butyric acid?

f. Identify the bonds C-C, C-H, and C-O in a molecule of butyric acid as polar covalent or nonpolar covalent.

Methane is a major component of purified natural gas used for heating and cooking. When $1.0$mole of methane gas bums with oxygen to produce carbon dioxide and water, $883kJ$is produced, Methane gas has a density of $0.715\mathrm{g}/\mathrm{L}$at $STP$. For transport, the natural gas is cooled to $-163°C$to form liquefied natural gas $\left(LNG\right)$with a density of $0.45\mathrm{g}/\mathrm{mL}$. A tank on a ship can hold $7.0$million gallons of $LNG\times (2.1,2,7,3.4,6.7,\$6.9,7.7,7.8,7.9,8.6)$

An LNG carrier transports liquefied natural gas.

a. Draw the Lewis structure for methane, which has the formula${\mathrm{CH}}_4.$

b. What is the mass, in kilograms, of LNG (assume that LNG is all methane) transported in one tank on a ship?

c. What is the volume, in liters, of LNG (methane) from one tank when the LNG is converted to gas at STP?

d. Write a balanced chemical equation for the combustion of methane in a gas burner, including the beat of reaction.

e. How many kilograms of oxygen are needed to react with all of the methane provided by one tank of LNG?

f. How much heat, in kilojoules, is released from burning all of the methane in one tank of LNG?

One tums tablet contains 500mg of calcium carbonate.

a. What is the formula of calcium carbonate?

b. What is the molar mass of calcium carbonate?

c. How many moles of calcium carbonate are in one roll of Tums that contains 12 tablets?

d. If a person takes two Tums tablets, how many grams of calcium is obtained?

e. If the daily recommended quantity of $C{a}^{2+}$to maintain bone strength in older women is 1500mg how many Tums tablets are needed each day to supply the needed calcium?

Tamiflu (oseltamivir), ${\mathrm{C}}_{16}{\mathrm{H}}_{28}{\mathrm{N}}_2{\mathrm{O}}_4$ is an antiviral drug used to treat influenza. The preparation of Tamiflu begins with the extraction of shikimic acid from the seedpods of star anise. From 2.6g of star anise, 0.13g of shikimic acid can be obtained and used to produce one capsule containing 75mg of Tamiflu. The usual adult dosage for treatment of influenza is two capsules of Tamiflu daily for 5 days.

a. If black spheres are carbon atoms, white spheres are hydrogen atoms, and red spheres are oxygen atoms, what is the formula of shikimic acid?

b. What is the molar mass of shikimic acid?

c. How many moles of shikimic acid are contained in 130g of shikimic acid?

d. How many capsules containing 75mg of Tamiflu could be produced from 155g of star anise?

e. What is the molar mass of Tamiflu?

f. How many kilograms of Tamiflu would be needed to treat all the people in a city with a population of 500000 if each person consumes two Tamiflu capsules a day for 5 days?

In wine making, aqueous glucose $\left({\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\right)$from grapes undergoes fermentation to produce liquid ethanol and carbon dioxide gas. A bottle of vintage port wine has a volume of 750 ml and contains 135ml of ethanol. Ethanol has a density of 0.789g/ml. In 1.5 lb of grapes, there is 26g of glucose.

a. Calculate the volume percent (v/v) of ethanol in the port wine.

b. What is the molarity (M) of ethanol in the port wine?

c. Write a balanced chemical equation for the fermentation reaction of glucose.

d. How many grams of glucose are required to produce one bottle of port wine?

e. How many bottles of port wine can be produced from 1 ton of grapes. (1 ton = 2000lb)

Identify the solute and the solvent in each solution composed of the following:

a. $10.0g$of $NaCl$and $100.0g$of$H_{2}O$

b. $50.0mL$of ethanol, $C_2{H}_{6}O$, and $10.0mL$of $H_{2}O$

c.$0.20L$of$O_2$and$0.80L$of$N_2$