Q&A Hero

Q: What volume (mL) of a 15% (m/v) NaOH solution contains 120 g NaOH? A) 18 mL B) 0.13 mL C) 13 mL D) 120 mL E) 8.0 102 mL

Q: A patient needs to receive 85 grams of glucose every 12 hours. What volume of a 5.0%(m/v) glucose solution needs to be administered to the patient each 12 hours? A) 1700 mL B) 60 mL C) 6000 mL D) 17 mL E) 204 mL

Q: How many grams of glucose are needed to prepare 400. mL of a 2.0%(m/v) glucose solution? A) 800. g B) 0.0050 g C) 8.0 g D) 2.0 g E) 200. g

Q: What is the concentration, in m/v percent, of a solution prepared from 50. g NaCl and 2.5 L of water? A) 5.0% B) 2.0% C) 0.020% D) 0.050% E) 20.%

Q: Rubbing alcohol is 70.% isopropyl alcohol by volume. How many mL of isopropyl alcohol are in a 1 pint (473 mL) container? A) 70. mL B) 0.15 mL C) 680 mL D) 470 mL E) 330 mL

Q: What is the concentration, in mass percent, of a solution prepared from 50.0 g NaCl and 150.0 g of water? A) 0.250% B) 33.3% C) 40.0% D) 25.0% E) 3.00%

Q: The mass/volume percent concentration refers to A) grams of solute in 1 L of solvent. B) grams of solute in 1 L of solution. C) grams of solute in 100 mL of solvent. D) grams of solute in 100 mL of solution. E) grams of solvent in 100 mL of solution.

Q: The mass percent concentration refers to A) grams of solute in 1 kg of solvent. B) grams of solute in 1 kg of solution. C) grams of solute in 100 g of solvent. D) grams of solute in 100 g of solution. E) grams of solvent in 100 g of solution.

Q: According to Henry's law, the solubility of a gas in a liquid A) decreases as the gas pressure above the liquid increases. B) increases as the gas pressure above the liquid increases. C) remains the same as the temperature increases. D) depends on the liquid polarity. E) depends on the liquid density.

Q: When solutions of NaCl and AgNO3 are mixed, A) a precipitate of AgCl forms. B) a precipitate of NaNO3 forms. C) no precipitate forms. D) precipitate of NaNO3 and AgCl form. E) a precipitate of AgCl2 forms.

Q: When solutions of KCl and Pb(NO3)2 are mixed, a precipitate forms. Which of the following is the balanced equation for the double replacement reaction that occurs?A) KCl(aq) + Pb(NO3) 2(aq) -> KNO3(aq) + PbCl2(s)B) KNO3(aq) + PbCl2(s) -> KCl(aq) + Pb(NO3) 2(aq)C) K+(aq) + NO3-(aq) -> KNO3(aq)D) 2KCl (aq) + Pb(NO3)2(aq) -> 2KNO3(aq) + PbCl2 (s)E) KCl(aq) + Pb(NO3)2(aq) -> KNO3(aq) + PbCl(s)

Q: Which one of the following compounds will be insoluble in water? A) AgNO3 B) CaCl2 C) NH4Cl D) CaCO3 E) Pb(C2H3O2)2

Q: Which one of the following compounds will be soluble in water? A) AgBr B) Cu(OH)2 C) NH4Cl D) CaCO3 E) PbS

Q: Which one of the following compounds will be soluble in water? A) AgCl B) Cu(OH)2 C) LiCl D) CaSO4 E) PbCO3

Q: Which one of the following compounds will NOT be soluble in water? A) LiOH B) K2S C) BaSO4 D) NaNO3 E) MgCl2

Q: Which one of the following compounds will NOT be soluble in water? A) NaOH B) PbS C) K2SO4 D) LiNO3 E) MgCl2

Q: An increase in the temperature of a solution usually A) increases the boiling point. B) increases the solubility of a gas in the solution. C) increases the solubility of a solid solute in the solution. D) decreases the solubility of a solid solute in the solution. E) decreases the solubility of a liquid solute in the solution.

Q: The solubility of KI is 50 g in 100 g of H2O at 20 C. If 110 grams of KI are added to 200 grams of H2O A) all of the KI will dissolve. B) the solution will freeze. C) the solution will start boiling. D) a saturated solution will form. E) the solution will be unsaturated.

Q: When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is A) dilute. B) polar. C) nonpolar. D) saturated. E) unsaturated.

Q: How many equivalents are present in 0.40 moles of SO42-? A) 0.10 Eq B) 0.20 Eq C) 0.40 Eq D) 0.80 Eq E) 1.2 Eq

Q: An intravenous replacement solution contains 4.0 mEq/L of Ca2+ ions. How many grams of Ca2+ are in 3.0 L of the solution? A) 0.24 g B) 0.80 g C) 0.40 g D) 240 g E) 4.0 g

Q: How many equivalents are present in 5.0 moles of Al3+? A) 15 Eq B) 1.3 Eq C) 5.0 Eq D) 0.67 Eq E) 3.0 Eq

Q: How many equivalents are present in 5.0 g of Al3+? A) 15 Eq B) 0.56 Eq C) 0.19 Eq D) 0.37 Eq E) 3 Eq

Q: An equivalent is A) the amount of ion that has a 1+ charge. B) the amount of ion that has a 1- charge. C) the amount of ion that carries 1 mole of electrical charge. D) 1 mole of any ion. E) 1 mole of an ionic compound.

Q: In water, a substance that partially ionizes in solution is called a A) weak electrolyte. B) nonelectrolyte. C) semiconductor. D) nonconductor. E) strong electrolyte.

Q: In water, a substance that ionizes completely in solution is called a A) weak electrolyte. B) nonelectrolyte. C) semiconductor. D) nonconductor. E) strong electrolyte.

Q: Water is a polar solvent and hexane (C6H14) is a nonpolar solvent. Which of the following correctly describes the solubility of the solute? A) mineral oil, soluble in water B) CaCl2, soluble in hexane C) NaHCO3, soluble in water D) CCl4, soluble in water E) octane, soluble in water

Q: When KCl dissolves in water A) the Cl- ions are attracted to dissolved K+ ions. B) the Cl- ions are attracted to the partially negative oxygen atoms of the water molecule. C) the K+ ions are attracted to Cl- ions on the KCl crystal. D) the K+ ions are attracted to the partially negative oxygen atoms of the water molecule. E) the K+ ions are attracted to the partially positive hydrogen atoms of the water molecule.

Q: Oil does not dissolve in water because A) oil is polar. B) oil is nonpolar. C) water is nonpolar. D) water is saturated. E) oil is hydrated.

Q: A solution is prepared by dissolving 2 g of KCl in 100 g of H2O. In this solution, H2O is the A) solute. B) solvent. C) solution. D) solid. E) ionic compound.

Q: Which of the following molecules can form hydrogen bonds? A) CH4 B) NaH C) NH3 D) BH3 E) HI

Q: In a solution, the solvent A) is a liquid. B) can be a liquid or gas. C) can be a solid, liquid, or gas. D) is never a solid. E) is the substance present in the smallest concentration.

Q: Hydrogen bonds are a major factor in the structure of A) DNA. B) hydrogen chloride. C) dry ice. D) air. E) table salt.

Q: A hydrogen bond is A) an attraction between a hydrogen atom attached to N, O, or F and an N, O, or F atom on another molecule. B) a covalent bond between H and O. C) an ionic bond between H and another atom. D) a bond that is stronger than a covalent bond. E) the polar O-H bond in water.

Q: The O-H bond in water is polar because A) it is an ionic bond. B) oxygen is much more electronegative than hydrogen. C) oxygen occupies more space than hydrogen. D) hydrogen is much more electronegative than oxygen. E) it is a hydrogen bond.

Q: Indicate whether each of the following compounds dissolves in water to give ions, molecules, or both. A) both B) ions C) molecules 1> NaCl, a strong electrolyte 2> HI, a strong electrolyte 3> CH3CH2OH, a nonelectrolyte 4> KNO3, a strong electrolyte 5> glucose, a nonelectrolyte 6> H2CO3, a weak electrolyte

Q: Compare the osmotic pressure of these solutions to the osmotic pressure of red blood cells. A) hypertonic B) isotonic C) hypotonic 1>water 2> 0.5% NaCl 3> 7% glucose 4> 5% glucose 5> 0.9% NaCl

Q: Match the type of mixture with the appropriate characteristics. A) suspension B) colloid C) solution 1> a mixture of sodium chloride in water 2> a mixture whose particles settle on standing 3> a homogeneous mixture in which suspended particles cannot pass through a semipermeable 4> a mixture whose particles cannot be separated by filters or semipermeable membranes 5> a mixture whose particles can be separated by filters

Q: Match the correct formula with the gas law name given. A) = B) PT= P1 + P2 + P3 ... C) = D) PV = nRT E) mass/volume F) = G) P1V1 = P2V2 H) = 1> Boyle's Law 2> Combined Gas Law 3> Charles's Law 4> Ideal Gas Law 5> Avogadro's Law 6> Gay-Lussac's Law 7> Dalton's Law

Q: Indicate the effect on the pressure of the following change. A) decreases B) increases C) no change 1> There is a decrease in volume (n, T constant). 2> Some molecules of gas are removed (V, T constant). 3> The temperature is doubled (V, n constant). 4> The volume and the Kelvin temperature are reduced by one-half (n constant). 5> A leak occurs and gas escapes (V, T constant).

Q: In deoxygenated blood, the partial pressure of carbon dioxide is greater than the partial pressure of oxygen left.

Q: During inspiration, we actually make use of 100% of the oxygen in the air we breathe.

Q: Carbon dioxide and water vapor together account for about 5% of the air we breathe.

Q: Ideal Gas Law calculations require the pressure to be in units of atm.

Q: The volume of 1 mole of an ideal gas at STP is 22.4 L.

Q: STP stands for 0 C and 760 mmHg.

Q: STP stands for 25 C and 760 mmHg.

Q: In the combined gas law, temperatures are given in C.

Q: The pressure exerted by a gas on its container is inversely related to its Kelvin temperature.

Q: Gas law calculations normally require the use of the Kelvin temperature scale.

Q: According to Boyle's, when volume increases, pressure decreases.

Q: The air we breathe is about 21% oxygen.

Q: 1 mmHg is the same as 760 atm.

Q: The kinetic energy of a gas sample is directly proportional to the Kelvin temperature of the gas.

Q: The Ideal Gas Law is usually written as ________.

Q: The use of high-pressure chambers to control disease processes is known as ________.

Q: At STP, the molar volume of a gas is ________.

Q: Avogadro's Law is usually written as ________.

Q: Gay-Lussac's Law is usually written as ________.

Q: Boyle's Law is usually written as ________.

Q: Oxygen makes up about ________ percent of the atmosphere.

Q: Nitrogen makes up about ________ percent of the atmosphere.

Q: The pressure unit 1 mmHg is the same pressure unit as the pressure unit ________.

Q: One atmosphere is the same as ________ mmHg.

Q: A barometer is usually filled with ________.

Q: The relationship V1/n1 = V2/n2 is called ________. A) Boyle's Law B) Charles's Law C) Gay-Lussac's Law D) The Combined Gas Law E) Avogadro's Law

Q: The relationship P1/T1 = P2/T2 is called ________. A) Boyle's Law B) Charles's Law C) Gay-Lussac's Law D) The Combined Gas Law E) Avogadro's Law

Q: The relationship P1V1 = P2V2 is called ________. A) Boyle's Law B) Charles's Law C) Gay-Lussac's Law D) The Combined Gas Law E) Avogadro's Law

Q: The pressure exerted by the particles of vapor above a liquid is called the ________. A) vapor pressure B) barometric pressure C) standard pressure D) molar pressure E) atmospheric pressure

Q: A barometer is a device for measuring ________. A) atmospheric pressure B) blood pressure C) gas pressure in a container D) gas pressure in the lung E) vapor pressure

Q: In the kinetic molecular theory of gas behavior, the distance between gas molecules is assumed to be ________ the diameter of the gas molecules. A) 22.4 times B) small relative to C) dependent on D) approximately the same as E) large relative to

Q: A gas sample contains 4.0 g of CH4 and 2.0 g of He. What is the volume of the sample at STP? A) 130 L B) 11 L C) 17 L D) 30. L E) 5.6 L

Q: If atmospheric pressure on a certain day is 749 mmHg, what is the partial pressure of nitrogen, given that nitrogen is about 78% of the atmosphere? A) 170 mmHg B) 580 mmHg C) 600 mmHg D) 750 mmHg E) 760 mmHg

Q: Which of the following correctly describes the partial pressures of gases in the body? A) high O2, low CO2, oxygenated blood B) high O2, low CO2, deoxygenated blood C) high O2, high CO2, oxygenated blood D) high O2, high CO2, tissue E) low O2, low CO2, deoxygenated blood

Q: A tank contains a mixture of helium, neon, and argon gases. If the total pressure in the tank is 490. mmHg and the partial pressures of helium and argon are 215 mmHg and 102 mmHg, respectively, what is the partial pressure of neon? A) 0.228 mmHg B) 603 mmHg C) 377 mmHg D) 807 mmHg E) 173 mmHg

Q: A tank contains helium gas at 490 mmHg, nitrogen gas at 0.75 atm, and neon at 520 torr. What is the total pressure in atm? A) 2.1 atm B) 0.55 atm C) 1.0 103 atm D) 1.5 atm E) 1600 atm

Q: A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of cyclopropane in the mixture is 330 mmHg and the partial pressure of the oxygen is 1.0 atm, what is the total pressure of the mixture in torr? A) 330 torr B) 430 torr C) 760 torr D) 1.4 torr E) 1100 torr

Q: The total pressure in a mixture of gases is equal to the partial pressure(s) of A) the gas with the greatest number of moles. B) the gas with the smallest number of moles. C) the gas with the highest molecular weight. D) the gas that occupies the largest volume. E) all the gases added together.

Q: Which of the following is NOT a potential use for a hyperbaric chamber? A) treatment for burns and infections B) counteracting carbon monoxide poisoning C) increasing the rate at which a broken bone heals D) treating a diver with the bends E) treating some cancers

Q: Zn(s) + 2 HCl(aq) -> H2(g) + ZnCl2(aq)When 25.0 g of Zn reacts, how many L of H2 gas are formed at 25 C and a pressure of 854 mmHg?A) 8.56 LB) 0.120 LC) 8.32 LD) 22.4 LE) 0.382 L