Chemistry: Ch. 13

A solution is saturated in O2 gas and KNO3 at room temperature. What happens if the solution is warmed to 75 ∘C? Nothing happens (both O2 and KNO3 remain in solution). Solid KNO3 precipitates out of solution. Gaseous O2 bubbles out of solution. Solid KNO3 precipitates out of solution and gaseous O2 bubbles out of solution.

Gaseous O2 bubbles out of solution.

saturated solution

a solution that holds the maximum amount of solute under the solution conditions. If the additional solute is added to a saturated solution, it will not dissolve

What is the name for this kind of solution? a heterogeneous mixture a weak electrolyte a strong electrolyte a nonelectrolyte

a strong electrolyte

recrystallization

a technique used to purify a solid; involves dissolving the solid in a solvent at high temperature, creating a saturated solution, then cooling the solution to cause the crystallization of the solid

unsaturated solution

a solution holding less than the maximum possible amount of solute under the solution conditions

supersaturated solution

a solution holding more than the normal maximum amount of solute

What are the ion concentrations in a 0.12 M solution of AlCl3? 0.12 M Al3+ ions and 0.36 M Cl− ions 0.36 M Al3+ ions and 0.12 M Cl− ions 0.040 M Al3+ ions and 0.040 M Cl− ions 0.12 M Al3+ ions and 0.040 M Cl− ions none of the above

0.12 M Al3+ ions and 0.36 M Cl− ions

A 0.15 M solution of BaCl2 contains: 0.15 M Ba2+ ions and 0.15 M Cl− ions. 0.30 M Ba2+ ions and 0.15 M Cl− ions. 0.30 M Ba2+ ions and 0.30 M Cl− ions. 0.15 M Ba2+ ions and 0.30 M Cl− ions. none of the above

0.15 M Ba2+ ions and 0.30 M Cl− ions.

Which one of the following aqueous solutions would have the higher concentration of K+ (aq) ions? (Assume total solubility in water.) 1.0 M K3PO4 1.0 M KNO3 1.0 M KC2H3O2 1.0 M K2CO3 All of these solutions have the same concentration of K+ (aq).

1.0 M K3PO4

You need to prepare 2.00 L of 0.100 M Na2CO3 solution. The best procedure is to weigh out: 21.2 g Na2CO3 and add 2.00 L of water to it. 10.6 g Na2CO3 and add water until the final solution has a volume of 2.00 L. 10.6 g Na2CO3 and add 2.00 L of water to it. 21.2 g Na2CO3 and add water until the final solution has a volume of 2.00 L.

21.2 g Na2CO3 and add water until the final solution has a volume of 2.00 L.

Refer to Figure 13.4 in the textbook to determine whether each of the given amounts of solid will completely dissolve in the given amount of water at the indicated temperature. Check all that apply. 32.0 g KCl in 70.0 g of water at 82 ∘C 65.0 g NaNO3 in 125 g of water at 15 ∘C 30.0 g KClO3 in 85.0 g of water at 35 ∘C

32.0 g KCl in 70.0 g of water at 82 ∘C 65.0 g NaNO3 in 125 g of water at 15 ∘C

If the solubility of sodium acetate (Molar mass = 82 g/mol) is 76 grams per 100 grams of water, which of the following solutions would be considered supersaturated? 5.5 moles of sodium acetate dissolved in 500 mL of water 1.2 moles of sodium acetate dissolved in 200 mL of water 8.5 moles of sodium acetate dissolved in 1 L of water 1.8 moles of sodium acetate dissolved in 300 mL of water none of the above

5.5 moles of sodium acetate dissolved in 500 mL of water. Definition of supersaturated: a solution holding more than the normal maximum amount of solute

If the solubility of sodium chloride is 36 grams per 100 grams of water, which of the following solutions would be considered unsaturated? 5.8 moles of NaCl dissolved in 1 L of water 3.25 moles of NaCl dissolved in 500 ml of water 1.85 moles of NaCl dissolved in 300 ml of water none of the above

5.8 moles of NaCl dissolved in 1 L of water Definition of unsaturated: a solution holding less than the maximum possible amount of solute under the solution conditions

Which solution below contains the highest total quantity of dissolved sodium ions? 100. mL of 4.0 M NaCl 50.0 mL of 2.0 M Na3PO4 50.0 mL of 8.0 M NaOH 75.0 mL of 3.0 M Na2SO4 none of the above

75.0 mL of 3.0 M Na2SO4

What is a stock solution? A stock solution is a saturated solution from which you prepare an unsaturated solution. A stock solution is a low-concentrated solution prepared using osmosis. A stock solution is a concentrated solution from which you prepare a more diluted solution. A stock solution is a heterogeneous mixture from which you prepare a homogeneous solution.

A stock solution is a concentrated solution from which you prepare a more diluted solution.

Which of the following statements about colligative properties is FALSE? The change in temperature is proportional to the molality. The boiling point of a solution is increased by the addition of salt. The freezing point of a solution is lowered by the addition of salt. The identity of the solute is not a factor. All of the above statements are true.

All of the above statements are true.

Which of the following aqueous solutions has the highest molar concentration of Na+ (aq)? (Assume each compound is fully dissolved in water.) 6.0 M NaCl (sodium chloride) 6.0 M NaC2H3O2 (sodium acetate) 3.0 M Na2SO4 (sodium sulfate) 2.0 M Na3PO4 (sodium phosphate) All of these solutions have the same concentration of Na+ (aq).

All of these solutions have the same concentration of Na+ (aq).

What is an aqueous solution? An aqueous solution is a homogeneous mixture of two or more substances. An aqueous solution exists when a solid, liquid, or a gas is dissolved in water. An aqueous solution is a heterogeneous mixture of two or more substances. An aqueous solution exists when a solid, liquid, or a gas is mixed with water.

An aqueous solution exists when a solid, liquid, or a gas is dissolved in water.

Common Laboratory Solvents

Common Polar Solvents: water (H20) acetone (CH3COCH3) methyl alcohol (CH3OH) Common Nonpolar Solvents: hexane (C6H14) diethyl ether (CH3CH2OCH2CH3) toluene (C7H8)

Which compound forms an electrolyte solution when dissolved in water? KBr Br2 CH3OH C6H12O6 (glucose)

KBr

Which compound below forms an electrolyte solution when dissolved in water? C12H22O11 (sucrose) CH3CH2OH Cl2 KOH none of the above

KOH

Define the concentration unit mass percent. Mass percent defined as the number of moles of solute per liter of solution. Mass percent defined as the mass (in grams) of a given component (solute or solvent) per 100 grams of solution. Mass percent defined as the number of moles of solute dissolved per kilogram of solvent. Mass percent defined as the mass(in kilograms) of a given component (solute or solvent) per volume(in cubic meters) of solution.

Mass percent defined as the mass (in grams) of a given component (solute or solvent) per 100 grams of solution.

Define molality. Molality defined as the mass (in grams) of a given component (solute or solvent) per 100 grams of solution. Molality defined as the mass(in kilograms) of a given component (solute or solvent) per volume(in cubic meters) of solution. Molality defined as the number of moles of solute dissolved per kilogram of solvent. Molality defined as the number of moles of solute per liter of solution.

Molality defined as the number of moles of solute dissolved per kilogram of solvent.

Define the concentration unit molarity. Molarity defined as the number of grams of solute per 100 g of solution. Molarity defined as the number of moles of solute per liter of solution. Molarity defined as the number of moles of solute per kilogram of solution. Molarity defined as the mass (in grams) of a given component (solute or solvent) per 100 grams of solution.

Molarity defined as the number of moles of solute per liter of solution.

Which of these compounds would you expect to be least soluble in water? N2 NaCl CH3OH NH3 not enough information

N2

Which of the following compounds is a strong electrolyte? C7H14O5 H8C4O2 C6H12O6 NaC2O2 all of the above

NaC2O2

Oftentimes solubility of a compound limits the concentration of the solution that can be prepared. Use the solubility data given with each compound shown below to determine which compound would allow the preparation of a 10.0 Molar solution. KCl (solubility = 34.0 g/100 g H2O) NH4Cl (solubility = 41.1 g/100 g H2O) NaNO3 (solubility = 89.0 g/100 g H2O) AgNO3 (solubility = 122 g/100 g H2O) none of the above

NaNO3 (solubility = 89.0 g/100 g H2O)

How is rock candy made? Rock candy is made from sugare placed on the pan. Sugar melts, than a string is placed into the sugar liquid and drawn out. When it is removed from the pan the sugar crystalize on the string. Rock candy is made from a natural mineral Candide that is mined in the north of Canada. Candide is treated with sugar under high temperature and then slowly cooled in nitrogen atmosphere. When it is 55∘C, string is placed into the system to form a candy. Rock candy is made the same way as a cotton candy. A string is placed into the special apparatus where small solid sugar particles are sputter on it. As a string is moved up and down more sugar is planted to form a rock candy. Rock candy is made from a saturated solution of sugar and a string placed into the solution. As the solution cools, it becomes saturated and the sugar crystals come out of solution and crystalize on the string.

Rock candy is made from a saturated solution of sugar and a string placed into the solution. As the solution cools, it becomes saturated and the sugar crystals come out of solution and crystalize on the string.

Common Types of Solutions

Solution phase: gaseous solutions Solute phase: gas Solvent phase: gas Ex.: air (mainly oxygen and nitrogen)

Common Types of Solutions

Solution phase: liquid solutions Solute phase: gas Solvent phase: liquid Ex.: soda water (CO2 and water)

Common Types of Solutions

Solution phase: liquid solutions Solute phase: liquid Solvent phase: liquid Ex.: vodka (ethanol and water)

Common Types of Solutions

Solution phase: liquid solutions Solute phase: solid Solvent phase: liquid Ex.: seawater (salt and water)

Common Types of Solutions

Solution phase: solid solutions Solute phase: solid Solvent phase: solid Ex.: Brass (copper and zinc)

A solution is saturated in both nitrogen gas (N2) and sodium iodide (NaI) at 50°C. When the solution is cooled to 25°C, which of the following is most likely to occur? Some nitrogen gas bubbles out of solution. Some sodium iodide will precipitate out of solution. Both A and B will happen. Nothing will happen. not enough information

Some sodium iodide will precipitate out of solution.

How does the presence of a nonvolatile solute affect the boiling point and melting point of a solution relative to the boiling point and melting point of the pure solvent? The addition of a nonvolatile solute will lower the freezing point and raise the boiling point of a solution relative to that of the pure solvent. The addition of a nonvolatile solute will lower both, the freezing point and the boiling point of a solution relative to that of the pure solvent. The addition of a nonvolatile solute will raise the freezing point and lower the boiling point of a solution relative to that of the pure solvent. The addition of a nonvolatile solute will raise both, the freezing point and the boiling point of a solution relative to that of the pure solvent.

The addition of a nonvolatile solute will lower the freezing point and raise the boiling point of a solution relative to that of the pure solvent.

Describe what happens when additional solute is added to a supersaturated solution. The additional solute will dissolve. The additional solute will cause the excess solute to come out of solution. The additional solute does not dissolve. None of the above.

The additional solute will cause the excess solute to come out of solution.

What will happen if a healthy red blood cell is placed into a container of pure water? The cell will become swollen. The cell will remain unchanged. The cell will totally dissolve in the water. The cell will shrink. none of the above

The cell will become swollen

Why does the dilution equation, M 1 V 1 = M 2 V 2, work? The dilution equation works because the number of moles remains the same. The dilution equation works because the molarity remains the same. The dilution equation works because the mass remains the same. The dilution equation works because the volume remains the same.

The dilution equation works because the number of moles remains the same.

A KCl solution containing 42 g of KCl per 100 g of water is cooled from 60 ∘C to 0 ∘C. What happens during cooling?

The excess KCl will recrystallize.

A KNO3 solution containing 45 g of KNO3 per 100 g of water is cooled from 40 ∘C to 0 ∘C. What happens during cooling?

The excess KNO3 will recrystallize.

Why is it NOT a good idea to drink seawater when people are lost at sea? The seawater has fish urine in it and who wants to drink that? The osmotic pressure builds up in the cells of your intestine until they potentially rupture. The high concentration of salt forces water out of the cells lining your stomach and intestine. The semipermeable membrane protecting your stomach is ruptured during osmosis. none of the above

The high concentration of salt forces water out of the cells lining your stomach and intestine.

Henry's law

The higher the pressure above a liquid, the more soluble the gas is in the liquid

Which of the following relationships is known as Henry's law? The sum of the partial pressures of each component in a gas mixture equals the total pressure. The volume of a gas and its pressure are inversely proportional. The higher the pressure above the liquid, the more soluble the gas is in the liquid. The lower the pressure above the liquid, the more soluble the gas is in the liquid.

The higher the pressure above the liquid, the more soluble the gas is in the liquid.

Solution A has a concentration of 0.10 M sugar and Solution B has a concentration of 0.20 M sugar. If the two solutions are separated by a semipermeable membrane, which of the following occurs during osmosis? Solvent molecules move from B into A. Sugar molecules move from B into A. The molarity of A increases. The molarity of B increases. none of the above

The molarity of A increases

After you have completed the task of diluting a solution, which statement below must be TRUE? The new solution has more volume but has a higher concentration than before. The new solution has less volume but has a higher concentration than before. The new solution has less volume but has a lower concentration than before. The new solution has more volume but has a lower concentration than before. none of the above

The new solution has more volume but has a lower concentration than before.

What is solubility? The solubility is the amount of solute that is necessary to prepare a supersaturated solution. The solubility is the amount of solute that is necessary to prepare an unsaturated solution. The solubility is the amount of solvent that dissolves in a specified amount of solute. The solubility is the amount of solute that dissolves in a specified amount of solvent. The solubility is the amount of solvent that is necessary to prepare an unsaturated solution. The solubility is the amount of solvent that is necessary to prepare a supersaturated solution.

The solubility is the amount of solute that dissolves in a specified amount of solvent.

Some laboratory procedures involving oxygen-sensitive reactants or products call for using preboiled (and then cooled) water. Explain why this is so. The reactivity of gases decreases as temperature increases. When water is boiled, the dissolved oxygen becomes inactive. The solubility of gases decreases as temperature increases. When water is boiled, the dissolved oxygen is completely removed. By increasing temperature the dissolved oxygen reacts more readily with dissolved hydrogen forming water. As result the concentration of oxygen decreases. By increasing temperature the dissolved oxygen oxidizes more readily impurities contained in the water. As result the concentration of oxygen decreasess.

The solubility of gases decreases as temperature increases. When water is boiled, the dissolved oxygen is completely removed.

How does gas solubility depend on temperature? The solubility of gases decreases with decreasing temperature. The solubility of gases does not depend on temperature. The solubility of gases increases with increasing temperature. The solubility of gases decreases with increasing temperature.

The solubility of gases decreases with increasing temperature.

How does gas solubility depend on pressure? The solubility of gases increases with increasing pressure. The solubility of gases does not depend on pressure. The solubility of gases decreases with increasing pressure. The solubility of gases increases with decreasing pressure

The solubility of gases increases with increasing pressure.

Which of the following mixtures are solutions? Check all that apply. a brass buckle air carbon dioxide and water mixture a blueberry muffin

a brass buckle air carbon dioxide and water mixture

molality (m)

a common unit of solution concentration, defined as the number of moles of solute per kilogram of solvent molality (m)= moles solute/ kilograms solvent

molarity

a common unit of solution concentration, defined as the number of moles of solute per liter of solution molarity (M)= moles solute/ liters solution

stock solution

a concentrated form in which solutions are often stored

solution

a homogeneous mixture of two or more substances

semipermeable membrane

a membrane that selectively allows some substances to pass through but not others

What is the name for this kind of solution? a weak electrolyte a nonelectrolyte a strong electrolyte a homogeneous mixture

a nonelectrolyte

strong electrolyte solution

a solution containing a solute that dissociates into ions; therefore, a solution that conducts electricity well

nonelectrolyte solution

a solution containing a solute that dissolves as molecules; therefore, the solution does not conduct electriclity

concentrated solution

a solution containing large amounts of solute

dilute solution

a solution containing small amounts of solute

Suppose a vodka martini contains 30% alcohol with the remaining portion of the drink composed of water. What is the solute in this type of martini? ice olive alcohol water none of the above

alcohol

Which of the following substances is NOT a solution? Which of the following substances is NOT a solution? sea water soda bronze homogenized milk All of the above are solutions.

all of the above are solutions

When preparing sodium hydroxide solution, it is best to use water that does not contain any dissolved carbon dioxide as it reacts with the sodium hydroxide. Removing the carbon dioxide can be accomplished by: vigorously stirring the solution. boiling the water. using water fresh out of the purification system. Nothing can be done to remove dissolved gases. none of the above

boiling the water

Properties that depend only on the number of particles in solution and not on the type of solute particle are called __________ properties. chemical colligative extensive structural

colligative

Which of the following substances is NOT a solution? copper air vodka brass All of the above are solutions.

copper

The solubility of gases in water: decreases with increasing temperature. increases with increasing temperature. is independent of temperature. gases are not soluble in water. none of the above

decreases with increasing temperature.

When you heat water on a stove, bubbles form on the bottom of the pot before the water boils. What are these bubbles? evaporated water gases that are coming out of walls of the pot dissolved gases that are coming out of solution dissolved solids that are coming out of solution

dissolved gases that are coming out of solution

When an ionic compound dissolves in water: the positive end of water dipoles attract the negative ions. the solvent-solute attractive forces overcome the solute-solute attractions. the negative end of water dipoles attract the positive ions. each of the above (A, B, and C) occurs. none of the above (A, B, or C) occurs.

each of the above (A, B, and C) occurs.

Solubility of gases in water: increases with increasing pressure above solution. decreases with increasing pressure above solution. is independent of pressure above solution. Gases are not soluble in water. none of the above

increases with increasing pressure above solution.

The solubility of solids in water: increases with increasing temperature. decreases with increasing temperature. is independent of the temperature. Solids are not soluble in water. none of the above

increases with increasing temperature.

The solubility of a gas in a liquid can always be increased by: increasing the temperature of the solvent. decreasing the pressure of the gas above the solvent. decreasing the polarity of the solvent. increasing the pressure of the gas above the solvent. none of the above

increasing the pressure of the gas above the solvent.

What kinds of solutes form strong electrolyte solutions? molecular compounds ionic compounds

ionic compounds

The solubility of solids in water: increases with increasing pressure above solution. is independent of pressure above solution. decreases with increasing pressure above solution. Solids are not soluble in water. none of the above

is independent of pressure above solution.

mass percent

is the number of grams of solute per 100 g of solution mass percent= mass solute/ mass solute + mass solvent *100%

dilution equation

m1v1=m2v2

Mass percent of the solution is the relationship between __________. mass of solute and mass of solution moles of solute and moles of solvent mass of solute and mass of solvent moles of solute and mass of solvent

mass of solute and mass of solution

Molarity is the relationship between ___________. mass of solute and mass of solvent moles of solute and mass of solvent moles of solute and moles of solvent moles of solute and liters of solution

moles of solute and liters of solution

Which among the following is NOT true about the solubility of a solid in water? Which among the following is NOT true about the solubility of a solid in water? The solubility generally increases as temperature increases. Solid crystallizes when a saturated solution is prepared at a higher temperature and then cooled. A saturated solution prepared at a lower temperature becomes unsaturated when heated to a higher temperature. The solubility is not affected by pressure. none of the above

none of the above

Hexane, a nonpolar solvent, will dissolve which of the following substances? oil sodium chloride vinegar (acetic acid) ammonium acetate none of the above

oil

Which of the following is a colligative property? specific heat capacity melting point density osmotic pressure

osmotic pressure

Which of the following substances is NOT a solution? oxygen beer steel humid air All of the above are solutions.

oxygen

colligative properties

physical properties of solutions that depend on the number of solute particles present but not the type of solute particles

A solution contains 35 g of NaCl per 100 g of water at 25 ∘C. Is the solution unsaturated, saturated, or supersaturated?

saturated

If you prepare a solution by adding sufficient amount of solute so that after heating and cooling the solution there is a visible amount of solid solute left in the bottom of the beaker, the solution would be considered ________. saturated thermally saturated unsaturated supersaturated none of the above

saturated

Which of the following best describes a mixture that has the same composition throughout? solvent heterogeneous solution solute

solution

In comparing a 0.25 molality aqueous NaCl solution to a 0.25 molality aqueous CaCl2 solution: the CaCl2 solution has the higher boiling point and the NaCl solution has the lower freezing point. the NaCl solution has the higher boiling point and the lower freezing point. the NaCl solution has the higher boiling point and the CaCl2 solution has the lower freezing point. the CaCl2 solution has the higher boiling point and the lower freezing point. both solutions have the same boiling point and the same freezing point.

the CaCl2 solution has the higher boiling point and the lower freezing point.

solubility

the amount of the compound, usually in grams, that dissolves in a certain amount of liquid

What are the dissolved particles in a solution containing an ionic solute? the cations only the molecules the cations and anions the anions only

the cations and anions

freezing point depression

the decrease in the freezing point of a solvent caused by the presence of a solute

osmosis

the flow of solvent from a lower concentration solution through a semipermeable membrane to a higher-concentration solution

boiling point elevation

the increase in the boiling point of a solution caused by the presence of the solute delta Tb= m * Kb for water: Kb= 0.512( degree Celcius kg solvent/ mol solute)

An osmosis cell is constructed of a "U" shaped tube with a semipermeable membrane separating the two arms of the tube. Suppose a concentrated solution is placed in the left arm of the U-tube, and a dilute concentration of the same substance is poured into the other arm to the same height. After a period of time has elapsed, you would expect to find that: no molecules of any type cross the membrane. the level of liquid in the left arm is now higher. the level of the liquid in the right arm is now higher. the levels in both arms stay at the same height. none of the above

the level of liquid in the left arm is now higher.

solvent

the majority component of a solution

solute

the minority component of a solution

What are the dissolved particles in a solution containing a molecular solute? the molecules the atoms the ions the cations

the molecules

osmotic pressure

the pressure produced on the surface of a semipermeable membrane by osmosis or the pressure required to stop osmotic pressure

Osmotic pressure: the pressure required to stop the rupture of the semipermeable membrane. the pressure required to stop the flow of solvent from a region of high solute concentration to a region of low solute concentration. the pressure required to reverse the flow of solvent through a semipermeable membrane during osmosis. the pressure required to stop the flow of solvent from a region of low solute concentration through a semipermeable membrane into a region of high solute concentration. none of the above

the pressure required to stop the flow of solvent from a region of low solute concentration through a semipermeable membrane into a region of high solute concentration.

The tragedy at Lake Nyos in Cameroon, West Africa, was caused by: the release of excess water stored in the volcanic lake which flooded the village below. the release of excessive amounts of oxygen gas that had been dissolved in the water at the bottom of the lake. the release of excessive amounts of carbon dioxide that had been dissolved in the water at the bottom of the lake. the release of excessive amounts of nitrogen gas that had been dissolved in the water at the bottom of the lake. none of the above

the release of excessive amounts of carbon dioxide that had been dissolved in the water at the bottom of the lake.

The oxygen in the air we breath is classified as: The oxygen in the air we breath is classified as: the solute in a heterogeneous gas-liquid mixture. the solvent in a homogeneous gas mixture. the solute in a homogeneous gas mixture. the solvent in a simple mixture. none of the above

the solute in a homogeneous gas mixture.

In order for a solute to dissolve in solution: the solute-solvent forces must equal the solute-solute forces. the polarity of the solute and solvent must be opposite. the solute-solute forces must be greater than the solute-solvent forces. the solute-solvent forces must be greater than the solute-solute forces. none of the above

the solute-solvent forces must be greater than the solute-solute forces.

A solution contains 28 g of KNO3 per 100 g of water at 25 ∘C. Is the solution unsaturated, saturated, or supersaturated? (Use Figure13.4 in the textbook.)

unsaturated

The solubility of Pb(NO3)2 is 55 grams per 100 g H2O at 20°C. Which term would properly describe a solution where 44 grams of Pb(NO3)2 is added to 100 grams of water at this temperature? unsaturated supersaturated insoluble saturated none of the above

unsaturated

soda water carbon dioxide is solvent and water is solute water is solvent and carbon dioxide is solute

water is solvent and carbon dioxide is solute

salt water: salt is solvent and water is solute water is solvent and salt is solute

water is solvent and salt is solute

sugar water water is solvent and sugar is solute sugar is solvent and water is solute

water is solvent and sugar is solute