Chem Review

How many grams of water are needed to react with 18.9 grams of Li2OLi2O?Given: Li2O+H2O→2LiOH

11.4

How many grams of sodium metal are needed to make 29.3 grams of sodium chloride? Given the reaction: 2Na + Cl2 → 2NaCl

11.5

How many grams of sodium metal are needed to make 29.3 grams of sodium chloride? Given the reaction: 2Na + Cl2 → 2NaCl

11.5

A solution contains 100.0 g water, 10.0 g NaCl, and 15.0 g methanol. What is the mass percent of methanol in the solution?

12.0%

How many mL of 0.218 M sodium sulfate react with exactly 25.34 mL of 0.113 M BaCl2 given the reaction: BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2NaCl(aq)

13.1

Which nuclear equation accurately represents the beta decay of Xe−133?

133 54Xe→133 55Cs+0 −1e

How many mL of 0.112 M Pb(NO3)2Pb(NO3)2 are needed to completely react with 30.0 mL of 0.105 M KI? Given: Pb(NO3)2(aq)+2KI(aq)→PbI2(s)+2KNO3(aq)

14.1

Calculate the mass percent of a NaCl solution prepared by mixing 21.0 g NaCl with 125.0 mL of pure water.

14.4

What is the pressure of 760 mm Hg when expressed in units of psi?

14.7 psi

A gas mixture containing only helium and neon is 22.1% neon (by volume) and has a total pressure of 748 mmHg. What is the partial pressure of neon?

165 mmHg

Potassium iodide reacts with lead(II) nitrate in the following precipitation reaction: 2KI(aq)+Pb(NO3)2(aq)→2KNO3(aq)+PbI2(s)2KI(aq)+Pb(NO3)2(aq)→2KNO3(aq)+PbI2(s) What minimum volume of 0.200 MM potassium iodide solution is required to completely precipitate all of the lead in 155.0 mL of a 0.122 MM lead(II) nitrate solution?

189 mL

When the equation, ___O2 + ___C 6H 14 →→ ___CO2 + ___H2O is balanced, the coefficient of O2 is:

19

A reaction in which a substance reacts with oxygen, emitting heat and forming oxygen-containing compounds is an example of a(n):

Combustion Reaction

A reaction which forms a solid product is an example of a(n):

Precipitation

How many protons and neutrons are in the nuclide? 207 81Tl

Protons, Neutrons = 81,126

How many protons and neutrons are in the nuclide? 219 86Rn

Protons, Neutrons = 86,133

A chemist wishes to perform the following reaction: N2 + 3 H2 → 2 NH3. If only 14.0 g of N2 is available, what is the minimum amount, in grams, of H2 needed to completely react with this quantity of N2?

3.03 g

What is a buffer?

A buffer is a solution that will resist a change in pH as the weak acid can react with added base and the conjugate base can react with added acid.

A 25.0 mL sample of 0.105 M HCl was titrated with 31.5 mL of NaOH. What is the concentration of the NaOH?

0.0833 M

What mass (in grams) of fructose (C6H12O6) is contained in 125 mL of a 0.500 M fructose solution?

11.3

Calculate the freezing point of a 1.30 mm sucrose (C12H22O11) solution.

-2.42 C

1 atm is equal to:

-760 mmHg -760 torr -14.7 psi -101,325 Pa

Which of the following mixtures are solutions?

-Sterling silver cup -Salt and water mixture

Calculate the molality of a solution prepared by dissolving 13.3 g of KCl in 750.0 mL of water.

0.238

What is the final concentration (M) of a solution prepared by diluting 50.0 mL of a 6.00 M KCl solution to a volume of 1.00 L?

0.300

A 141 −mL sample of a 1.5 M sucrose solution is diluted to 600 mL. What is the molarity of the diluted solution?

0.35 M

What is the final concentration of a solution prepared by diluting 35.0 mL of 12.0 M HCl to a final volume of 1.20 L?

0.350 M

A 330 −mL can of soda pop contains 45 g of sucrose (C12H22O11). What is the molarity of the solution with respect to sucrose?

0.40 M

What is the final concentration (M) of a solution prepared by diluting 50.0 mL of a 6.00 M KCl solution to a volume of 0.750 L?

0.400

Calculate the molarity of a KCl solution made by dissolving 16.6 g of KCl in a total volume of 500. mL.

0.445

What volume (L) of 0.750 M KCl solution contains 25.0 g of KCl?

0.447

What is the molar concentration of potassium ions in a 0.250 MM K2SO4K2SO4 solution?

0.500 M

Given that the freezing point depression constant for water is 1.86°C kg/mol, calculate the change in freezing point for a 0.500 m sugar solution.

0.930 C

What is the molarity of a solution prepared by dissolving 54.3 g of Ca(NO3)2 into 355 mL of water?

0.932 M

Radon-219 decays to radon-218 by releasing:

1 0n

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

How many moles of water are made from complete reaction of 1.4 moles of hydrogen gas? Given the reaction: 2H2 + O2 → 2H2O

1.4

What volume of a 0.36 M Mg(NO3)2 solution contains 88 g of Mg(NO3)2?

1.6 L

How many moles of water are needed to react with 1.7 moles of Li2OLi2O?Given: Li2O+H2O→2LiOH

1.7

If a mixture of gases contained 78% nitrogen at a pressure of 984 torr and 22% carbon dioxide at 345 torr, what is the total pressure of the system?

1.75 atm

A glucose solution is 3.25% glucose by mass and has a density of 1.03 g/mL. What mass of glucose is contained in 58.2 mL of this solution?

1.95

How many grams of KCl are present in 65.0 mL of 2.10 M KCl?

10.2

A gas cylinder contains only the gases radon, nitrogen, and helium. The radon has a pressure of 222 torr while the nitrogen has a pressure of 446 torr. If the total pressure inside the cylinder is 771 torr, what is the pressure that is due to the helium?

103 torr

How many grams of LiF would be present in 575 mL of 0.750 M LiF solution?

11.2

Given the balanced equation CH4 + 2 O2 → CO2 + 2 H2O, which of the following is NOT a correct conversion factor?

2 mole H2O = 18.02g

Hydrogen chloride gas and oxygen gas react to form gaseous water and chlorine gas according to the reaction shown here. 4HCl(g)+O2(g)→2H2O(g)+2Cl2(g) If the first image below represents the amount of HCl available for the reaction, which image represents the amount of oxygen required to react completely with the amount of available HCl?

2 molecules of O2

How many moles of water are needed to react with 2.2 moles of Li2OLi2O? Given: Li2O+H2O→2LiOH

2.2

How many moles of water are needed to react with 2.8 moles of Li2OLi2O?Given: Li2O+H2O→2LiOH

2.8

Provide a symbol for the isotope of bismuth that contains 124 neutrons.

207 83Bi

How many grams of water are needed to react with 36.2 grams of Li2O?Given: Li2O+H2O→2LiOH

21.8

What volume of 12.0 M HCl is required to make 75.0 mL of 3.50 M HCl?

21.9 mL

Which daughter nuclide results from the alpha decay of radon-218?

214 84Po

Uranium-238 undergoes radioactive decay to form an alpha particle and what other daughter nuclide?

234 90Th

How many grams of a 23.4% by mass NaF solution is needed if you want to have 1.33 moles of NaF?

239

Sodium reacts with fluorine to form sodium fluoride. What mass of sodium fluoride forms from the complete reaction of 11.5 gg of fluorine with enough sodium to completely react with it?2Na(s)+F2(g)2Na(s)+F2(g) →→ 2NaF(s)

25.4g NaF

What is the mass percent of a sodium fluoride solution prepared by dissolving 0.64 moles of sodium fluoride into 63.5 grams of water?

29.7%

How many conversion factors (relationships) are given in the following chemical equation? 3 H2(g) + N2(g) → 2 NH3(g)

3 conversion factors

Given that 4 NH3 + 5 O2 → 4 NO + 6 H2O, when 4.50 mol of H2O are formed, the amount of NO formed is:

3.00 mol

For the reaction, calculate how many grams of the product form when 2.0 gg of Cl2Cl2 completely reacts. Assume that there is more than enough of the other reactant. 2Na(s)+Cl2(g)→2NaCl(s)

3.3g

Calculate the molarity of a KCl solution prepared by dissolving 0.898 moles of KCl in 250. mL of water.

3.59

How many moles of sodium metal are needed to make 3.6 moles of sodium chloride? Given the reaction: 2Na + Cl2 → 2NaCl

3.6

How many moles of KOH are contained in 750. mL of 5.00 M KOH solution?

3.75 mol

How many grams of water are made from the reaction of 4.0 grams of hydrogen gas? Given the reaction: 2H2 + O2 → 2H2O

36

Aluminum reacts with chlorine gas to form aluminum chloride. 2Al(s)+3Cl2(g)→2AlCl3(s)2Al(s)+3Cl2(g)→2AlCl3(s) What minimum volume of chlorine gas (at 298 KK and 225 mmHg) is required to completely react with 7.85 g of aluminum?

36.0 L

A 1.2 kg sample of Th-228 has a half-life of 1.9 years. How many grams of Th is left after 9.5 years?

37.5

Diatomic N2 can react with diatomic H2 to form ammonia (NH3). The balanced chemical equation is:N2 + 3 H2 → 2 NH3If 6 moles of H2 totally reacted with more than enough N2, how many moles of ammonia would be expected to form?

4 Moles

Diatomic O2 can react with the element magnesium to form magnesium oxide (MgO). The balanced chemical equation is: O2 + 2 Mg → 2 MgOIf 4 moles of magnesium totally reacted with more than enough O2, how many moles of MgO would be expected to form?

4 Moles

How many moles of water are made from complete reaction of 2.2 moles of oxygen gas with hydrogen gas? Given the reaction: 2H2 + O2 → 2H2O

4.4

A gas sample occupies 3.50 liters of volume at 20.°C. What volume will this gas occupy at 100°C (reported to three significant figures)?

4.46 L

How many moles of H2 can be made from complete reaction of 3.0 moles of Al? Given: 2 Al + 6 HCl → 2 AlCl3 + 3 H2

4.5 moles

Given that 4 NH3 + 5 O2 → 4 NO + 6 H2O, if 3.00 mol NH3 were made to react with excess of oxygen gas, the amount of H2O formed would be:

4.50 mol

What is the mass percent of an ammonium carbonate solution prepared by dissolving 33.2 grams of solid into 39.5 grams of water?

45.7%

What is the final volume (L) of a 10.0 L system that has the pressure doubled?

5.00

What is the final volume of a balloon that was initially 500.0 mL at 25°C and was then heated to 50°C?

542 mL

A gas mixture contains each of the following gases at the indicated partial pressure. N2 - 219 torr O2 - 108 torr He - 248 torr What is the total pressure of the mixture?

575 torr

How many conversion factors (relationships) are given in the following chemical equation? 2 NO(g) + 5 H2(g) → 2 NH3(g) + 2 H2O(g)

6 conversion factors

How many moles of aluminum are needed to make 9 moles of molecular hydrogen? Given the reaction: 2 Al + 6 HCl → 2 AlCl3 + 3H2

6 moles

Divers often inflate heavy duty balloons attached to salvage items on the sea floor. If a balloon is filled to a volume of 3.00 L at a pressure of 2.50 atm, what is the volume of the balloon when it reaches the surface?

7.50 L

How many grams of chlorine gas are needed to make 117 grams of sodium chloride? Given the reaction: 2Na + Cl2 → 2NaCl

71.0

Which solution below contains the highest total quantity of dissolved sodium ions?

75.0 mL of 3.0 M Na2SO4

How many grams of KCl are needed to make 50.0 mL of 2.45 M KCl?

9.13

How many mL of 0.112 M Pb(NO3)2Pb(NO3)2 are needed to completely react with 20.0 mL of 0.105 M KI? Given: Pb(NO3)2(aq)+2KI(aq)→PbI2(s)+2KNO3(aq)

9.38

How many moles of gas were added to a balloon that started with 2.3 moles of gas and a volume of 1.4 L given that the final volume was 7.2 L?

9.5

What volume of 9.00 M nitric acid is needed to make 6.50 L of 1.25 M solution?

903 mL

How many milliliters of 0.755 M H2SO4 solution is needed to react with 55.0 mL of 2.50 M KOH solution? Given: 2 KOH (aq) + H2SO4 (aq) → 2 H2O (l) + K2SO4 (aq)

91.1 mL

Which of the following is the definition of a Brønsted-Lowry base?

A Brønsted-Lowry base is a proton acceptor.

Which of the following is NOT typically a sign of a chemical reaction?

Absorbing light when chemicals are contacted with each other

Which of the following gas law relationships is true?

All of the above are true

Which of the following statements is false?

All of the above are true statements.

Which of the following statements about colligative properties is FALSE?

All of the above statement are true.

Which of following statements are consistent with the Kinetic Molecular Theory?

All of the above statements are consistent with the Kinetic Molecular Theory.

Considering the following precipitation reaction: Pb(NO3)2(aq) + 2KI(aq) →→ PbI2(s) + 2KNO3(aq) Which ion would NOT be present in the complete ionic equation?

All the above ions are in the complete ionic equation.

When must temperature values in gas law calculations be expressed in kelvin units?

Always

What must be supplied for a decomposition reaction to happen?

Any of the above

Pair each cation on the left with an anion on the right that will form an insoluble compound. Use each anion only once.

Ba(2+)SO4(2-) Fe(3+)S(2-) Ag(+)Cl(-) Cu(2+)CO3(2-)

What is the missing particle? 231 90Th _______+ 231 91Pa

Beta Particle

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:

Boiling the water

What is the limiting reactant for the following reaction given we have 3.4 moles of Ca(NO3)2 and 2.4 moles of Li3PO4? Reaction: 3Ca(NO3)2 + 2Li3PO4 → 6LiNO3 + Ca3(PO4)2

Ca(NO3)2

Which of the following laws states that the volume of a gas and its Kelvin temperature are directly proportional?

Charles's Law

Which of the following substances is NOT a solution?

Copper

Determine which of the following compounds are insoluble.

Cu3(PO4)2 Hg2I2 CaSO4 MgS

What type of reaction is the generic equation AB →→ A + B?

Decomposition

The solubility of gases in water:

Decreases with increasing temperature

Given the chemical equation: 2 Ca + O2 → 2 CaO,if 2 moles of CaO are formed in this reaction, then 2 moles of O2 must have reacted.

False

Given the reaction: 2 Na(s) + Cl2(g) → 2 NaCl(s)The conversion factor for chlorine gas to sodium metal is: 2 mol Cl ≡ 2 mol Na

False

H+ is called the hydronium ion.

False

If the number of gas particles is tripled, the volume will be 1/3 of the original given that temperature and pressure do not change.

False

If you had a five liter balloon of argon gas and a five liter balloon of xenon gas, and you removed 10 grams of gas from each balloon, the balloons would both shrink down to the same size.

False

Sugar solutions conduct electricity because the dissolved particles are molecules.

False

The alpha particle is: 4 3He

False

The major component in a solution is called the solute.

False

The molarity of a solution prepared by dissolving 15.0 grams of NaCl in 1000 mL water is 0.15 M.

False

The terms "molarity" and "molality" are considered identical and can always be used interchangeably.

False

The unit of pressure known as the atmosphere (atm) is defined as the average pressure found at the top of Mount Everest.

False

The volume of a gas and the number of particles is inversely proportional.

False

Pressure is the relationship between ___________?

Force and area

A reaction which forms a gaseous product is an example of a(n)________.

Gas Evolution Reaction

A solution is saturated in N2 gas and KCl at room temperature. What happens if the solution is warmed to 75 ∘C?

Gaseous N2 bubbles out of solution.

Which of the following compounds decompose to form water and a gas?

H2CO3

What is the conjugate acid of OH⁻?

H2O

What are the products of the reaction between HBr(aq) and KOH(aq)?

H2O(l) and KBr(aq)

Which of the following is NOT an acid-base conjugate pair?

H2S and OH-

Determine whether or not each mixture is a buffer.

HC2H3O2 and KC2H3O2 HF and NaF

The solubility of solids in water:

Increases with increasing temperature

Considering the following precipitation reaction: Pb(NO3)2(aq) + 2KI(aq) →→ PbI2(s) + 2KNO3(aq) Which ion(s) would NOT be present in the net ionic equation?

K(+), NO3(-)

Determine which of the following compounds are soluble.

K2S NH4Cl Na2CO3 BaS

Which is the limiting reactant in the following reaction given that you start with 42.0 g of CO2 and 99.9 g KOH? Reaction: CO2 + 2KOH → K2CO3 + H2O

KOH

Balancing chemical reactions is consistent with which scientific law?

Law of conversation of mass

Mass percent of the solution is the relationship between __________.

Mass of solute and mass of solution

Define the concentration unit mass percent.

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

Which of these compounds would you expect to be least soluble in water?

N2

Which of the following are spectator ions in the reaction: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

Na(+) and NO3(-)

Identify the spectator ions in the following complete ionic equation: Ba2+(aq)+2I−(aq)+2Na+(aq)+SO42−(aq)→BaSO4(s)+2I−(aq)+2Na+(aq)

Na(+), I(-)

Which of the following compounds is a strong electrolyte?

NaC2O2

At STP, 12.69 g of a noble gas occupies 14.09 L. What is the identity of the noble gas?(R= 0.0821 L atm/ mol K)

Ne

Which among the following is NOT true about the solubility of a solid in water?

None of the above

Which of the following is an example of a fossil fuel?

Octane

Hexane, a nonpolar solvent, will dissolve which of the following substances?

Oil

Which of the following substances is NOT a solution?

Oxygen

Considering the following precipitation reaction: Pb(NO3)2(aq) + 2KI(aq) →→ PbI2(s) + 2KNO3(aq) Which ion(s) would NOT be spectator ions?

Pb(2+), I(-)

A solution contains 35 g of NaCl per 100 g of water at 25 ∘C.

Saturated

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 sodium iodide will precipitate out of solution.

All of the following statements are consistent with the kinetic molecular theory of gases EXCEPT:

Strong attractive forces hold the gas molecules together.

Which of the following happens when solid sodium chloride dissolves in water?

The attractive forces between the sodium and chloride ions are overcome by the attractive forces between the water and the sodium and chloride ions.

What are the dissolved particles in a solution containing an ionic solute?

The cations and anions

What will happen if a healthy red blood cell is placed into a container of pure water?

The cell will become swollen.

Suppose you a have a 100,000-atom sample of a radioactive nuclide that decays with a half-life of 2.0 days. a) How many radioactive atoms are left after 10 days?

a) 3125 atoms

Why is it NOT a good idea to drink seawater when people are lost at sea?

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

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?

The molarity of A increases.

The oxygen in the air we breath is classified as:

The solute in a homogeneous gas mixture.

Which of the following correctly defines the principles of kinetic molecular theory?

There are no attractions between particles.

A beta particle can also be called an electron.

True

A gamma ray is a high energy photon.

True

A saturated solution holds the maximum amount of solute under the solution conditions.

True

A solution is a homogeneous mixture of two or more substances.

True

A solution that is 13.58 percent by mass of sugar contains 13.75 grams of sugar dissolved in 87.5 grams of water.

True

A supersaturated solution is unstable and crystallization usually occurs.

True

Air is an example of a gaseous solution.

True

As you increase temperature, you increase the average energy of the gas particles.

True

Before determining conversion factors, it is necessary to make sure the equation is properly balanced.

True

Gases fill the entire volume of their container.

True

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

True

Salt water is an example of a strong electrolyte solution.

True

The conjugate base to HSO4- is SO42-.

True

The solubility of gases in water decreases with increasing temperature.

True

The solubility of gases in water increases with increasing pressure above the water.

True

When an atom emits an alpha particle, it becomes a different element.

True

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

Boyle's Law is expressed as:

V is proportional to 1/P

Charles's Law is expressed as:

V is proportional to T

Avogadro's Law is expressed as:

V is proportional to n

An aqueous solution is:

Water with another compound dissolved in it.

When a chemical drain opener is added to a clogged sink, bubbles form and the water in the sink gets warmer. Has a chemical reaction occurred?

Yes

For the reaction shown, calculate how many grams of oxygen form when each quantity of reactant completely reacts.2HgO(s)→2Hg(l)+O2(g) a) 2.20g HgO b) 6.17g HgO c) 1.97kg HgO d) 3.83mg HgO

a) 0.163g b) 0.456g c) 146g d) 2.83x10-4g

A 2.5 −L−L sample of a 6.3 MM NaCl solution is diluted to 70 L. a) What is the molarity of the diluted solution?

a) 0.23 M

A snorkeler with a lung capacity of 5.0 LL inhales a lungful of air at the surface, where the pressure is 1.0 atm. The snorkeler then descends to a depth of 45 mm , where the pressure increases to 5.5 atm a) What is the volume of the snorkeler's lungs at this depth? (Assume constant temperature.)

a) 0.91 L

An alkane undergoes combustion when it reacts with oxygen to produce carbon dioxide, water, and energy: alkane+O2→CO2+H2O+energy a) Balance the reaction for the combustion of propane: ?C3H8+?O2→?CO2+?H2O

a) 1, 5, 3, 4

Determine the amount of sucrose in each of the following solutions. a) 38 g of a solution containing 3.5 % sucrose by mass b) 113 mg of a solution containing 10.4 % sucrose by mass c) 3.0 kg of a solution containing 14.9 % sucrose by mass

a) 1.3 g b) 11.8 mg c) 0.45kg

For the reaction shown, calculate how many moles of each product form when the given amount of each reactant completely reacts. Assume that there is more than enough of the other reactant. C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) a) 4.2 mol C3H8 b) 4.2 mol C3H8 c) 0.0567 mol C3H8 d) 0.0567 mol C3H8 e) 4.2 mol O2 f) 4.2 mol O2 g) 0.0567 mol O2 h) 0.0567 mol O2

a) 13 mol CO2 b) 17 mol H2O c) 0.170 mol CO2 d) 0.227 mol H2O e) 2.5 mol CO2 f) 3.4 mol H2O g) 3.40x10-2 mol CO2 h) 4.54x10-2 mol H2O

A soft drink contains 46 g of sugar in 320 g of H2O. a) What is the concentration of sugar in the soft drink in mass percent?

a) 13%

Calculate the concentration of each solution in mass percent. a) 114 g KCl in 628 g H2O b) 30.3 mg KNO3 in 5.66 g H2O c) 8.11 g C2H6O in 74.9 g H2O

a) 15.4% b) 0.532 % c) 9.77 %

For the reaction shown, calculate how many moles of NO2NO2 form when each amount of reactant completely reacts. 2N2O5(g)→4NO2(g)+O2(g) a) 1.2 mol N2O5 b) 5.5 mol N2O5 c) 5.00X103 mol N2O5 d) 1.011x10-3 mol N2O5

a) 2.4 mol b) 11 mol c) 1.00x104 mol d) 2.022x10-3 mol

Write a nuclear equation for the alpha decay of each nuclide. a) U - 234 b) Th - 230 c) Ra - 226 d) Rn - 222

a) 234 92U [ 4 2He+230 90Th b) 230 90Th [ 4 2He+226 88Ra c) 226 88Ra [ 222 86Rn+4 2He d) 222 86Rn [ 218 84Po+4 2He

Consider the following unbalanced equation for the combustion of butane.C4H10(g)+O2(g)→CO2(g)+H2O(g) a) Balance the equation b) Determine how many moles of O2 are required to react completely with 4.7 mol of C4H10C4H10.

a) 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(g)2C4H10(g)+13O2(g)→8CO2(g)+10H2O(g) b) 31 mol

Consider the following unbalanced equation for the neutralization of acetic acid. HC2H3O2(aq)+Ca(OH)2(aq)→H2O(l)+Ca(C2H3O2)2(aq) a) Balance the equation. b) Determine how many moles of Ca (OH) 2 are required to completely neutralize 7.71 mol of HC2H3O2.

a) 2HC2H3O2(aq)+Ca(OH)2(aq)→2H2O(l)+Ca(C2H3O2)2(aq) b) 3.86 mol

Consider the following unbalanced equation for the neutralization of acetic acid. HC2H3O2(aq)+Ca(OH)2(aq)→H2O(l)+Ca(C2H3O2)2(aq) a) Balance the equation. b) Determine how many moles of Ca (OH)(OH) 22 are required to completely neutralize 1.31 mol of HC2H3O2HC2H3O2.

a) 2HC2H3O2(aq)+Ca(OH)2(aq)→2H2O(l)+Ca(C2H3O2)2(aq)2HC2H3O2(aq)+Ca(OH)2(aq)→2H2O(l)+Ca(C2H3O2)2(aq) b) 0.655 mol

A beaker of nitric acid is neutralized with a dilute aqueous solution of calcium hydroxide. a) Enter a balanced molecular equation for this reaction. b) Enter a net ionic equation for this reaction.

a) 2HNO3(aq)+Ca(OH)2(aq)→2H2O(l)+Ca(NO3)2(aq) b) H+(aq)+OH−(aq)→H2O(l)H+(aq)+OH−(aq)→H2O(l)

For the reaction shown, calculate how many moles of NH3NH3 form when each amount of reactant completely reacts. 3N2H4(l)→4NH3(g)+N2(g) a) 5.4 mol N2H4 b) 2.29 mol N2H4 c) 5.9x10-2 mol N2H4 d) 9.73x107 mol N2H4

a) 7.2 mol b) 3.05 mol c) 7.9x10-2 mol d) 1.26x108 mol

Identify the particle represented by each symbol as an alpha particle, a beta particle, a gamma ray, a positron, a neutron, or a proton. a) 0 -1e b) 1 0n c) 0 0(y thing)

a) Beta particle b) Neutron c) Gamma ray

Write the formula for the conjugate acid of each base. a) CH3NH2 b) C5H5N c) Cl- d) F-

a) CH3NH3+ b) C5H6N+ c) HCl d) HF

Write the formula for the conjugate base of each acid. a) HCl b) H2SO3 c) HCHO2 d) HF e) HBr f) H2CO3 g) HClO4 h) HC2H3O2

a) Cl- b) HSO3- c) CHO2- d) F- e) Br- f) HCO3- g) ClO4- h) C2H3O2-

Consider the following unbalanced equation for the reaction of solid lead with silver nitrate. Pb(s)+AgNO3(aq)→Pb(NO3)2(aq)+Ag(s) a) Balance the equation. b) How many moles of silver nitrate are required to completely react with 9.1 mol of lead? c) How many moles of Ag are formed by the complete reaction of 28.8 mol of Pb?

a) Pb(s)+2AgNO3(aq)→Pb(NO3)2(aq)+2Ag(s)Pb(s)+2AgNO3(aq)→Pb(NO3)2(aq)+2Ag(s) b) 18 mol c) 57.6 mol

In a combustion reaction, ethanoic acid (CH3COOHCH3COOH) is burned in the presence of oxygen (O2O2), producing carbon dioxide (CO2CO2) and water (H2OH2O). a) Classify each substance as either a reactant or product in the chemical reaction. b) Starting with the unbalanced equation for the combustion of ethanoic acid, CH3COOH(l)+O2(g)→CO2(g)+?H2O(l)CH3COOH(l)+O2(g)→CO2(g)+?H2O(l) what coefficient should be placed in front of H2OH2O to balance the hydrogen atoms? c) Starting with the partially balanced equation, CH3COOH(l)+O2(g)→?CO2(g)+2H2O(l)CH3COOH(l)+O2(g)→?CO2(g)+2H2O(l) what coefficient should be placed in front of CO2CO2 to balance the carbon atoms? d) Starting with the partially balanced equation, CH3COOH(l)+?O2(g)→2CO2(g)+2H2O(l)CH3COOH(l)+?O2(g)→2CO2(g)+2H2O(l) what coefficient should be placed in front of O2O2 to balance the oxygen atoms?

a) Reactants - Ethanoic acid & Oxygen Products - Carbon Dioxide & Water b) ?=2 c) ?=2 d) ?=2

Identify the solute and solvent in each solution. a) 80-proof vodka (40% ethyl alcohol) b) Oxygenated water c) antifreeze (ethylene glycol and water)

a) Solute - Ethyl Alcohol Solvent - Water b) Solute - Oxygen Solvent - Water c) Solute - Ethylene Glycol Solvent - Water

Identify the solute and solvent in each of solution. a) Salt Water b) Sugar Water c) Soda Water

a) Water is solvent and salt is solute b) Water is solvent and sugar is solute c) Water is solvent and carbon dioxide is solute

Vinegar forms bubbles when it is poured onto the calcium deposits on a faucet, and some of the calcium dissolves. a) Has a chemical reaction occurred?

a) Yes

Calculate the pH of each solution. a) [H3O+] = 3.7×10−8 M b) [H3O+] = 1.0×10−7 M c) [H3O+] = 5.2×10−6 M d) [H3O+] = 4.4×10−4 M

a) pH = 7.43 b) pH = 7.00 c) pH = 5.28 d) pH = 3.36

Determine the pOH of each solution. a) [H3O+] = 6.3×10−10 M b) [H3O+] = 5.6×10−7 M c) [H3O+] = 8.3×10−2 M d) [OH−] = 7.32×10−4 M

a) pOH = 4.80 b) pOH = 7.75 c) pOH = 12.92 d) pOH = 3.135

Identify the particle represented by each symbol as an alpha particle, a beta particle, a gamma ray, a positron, a neutron, or a proton. a) 1 1p b) 4 2He c) 1 +1e

a) proton b) alpha particle c) positron

Classify each base as strong or weak. a) LiOH b) NH4OH c) Ca(OH)2 d) NH3

a) strong b) weak c) strong d) weak

Solubility of gases in water:

increases with increasing pressure above solution.

Osmotic pressure is:

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.

In order for a solute to dissolve in solution:

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