Practice Exam—#3 CHEMISTRYCh 6.7

1. A gas containing 0.42 mole of helium has a volume of 3.00 L. What is the new volume when 1.0 mole of nitrogen is added to the container (pressure and temperature remain constant)?  

2. What is the volume occupied by 28.0 g of oxygen, O2 at STP?

3. What is the volume, in liters, of a container that holds 14.6 g N2 at STP?

4. What is the number of moles of O2 in 4.88 L. of O2 gas at STP?

5. What is the number of moles of CO2 in 4.00 L. of CO2 gas at STP?

6. What is the volume (in L) of 6.40g of O2?

7. What is the volume (in mL) occupied by 50.0 g of neon?

CH. 6.8

1. A gas mixture containing oxygen, helium and nitrogen exerts a total pressure of 925 torr. If the partial pressures are oxygen 425 torr and helium 75 torr, what is the partial pressure of the nitrogen in the mixture?

2. One tank of gas contains a gas sample at 2.0 atm. A second tank of gas with a pressure of 7.0 atm is pumped into the first tank. The pressure in the first tank is now…?

3. What is the pressure, in mm Hg, of a sample of gases containing oxygen at 1.500 atm, nitrogen at 432.0 torr, and helium at 824.0 mm Hg?

4. A balloon is filled with helium gas with a pressure of helium gas with a pressure of 1.00 atm and neon gas with a pressure of 0.50 atm For each of the following changes of the initial balloon, select the diagram (A, B or C) that shows the new volume of the balloon:

4. Continued—a. The balloon is put in a cold storage unit; P & n remain constant.b. The balloon floats to a higher altitude where the pressure is less; n & t are

constant.c. All of the neon gas leaks out.

Initial SizeCA B

d. The temperature doubles, and one-half of the gas atoms leak out; P is constant.

E 2.0 moles of O2 gas is added at constant T & P.Ch 7.1

1. Identify the solute in each of the following solutions. a. 2 g of sugar and 100 mL of waterb. 60.0 mL of ethyl alcohol and 30.0 mL of methyl alcoholc. 55.0 mL of water and 1.50 g of NaCl d. Air: 200 mL of O2 and 800 mL of N2

Ch 7.21. Which of the following solutes will dissolve in water? Why?

a) Na2SO4

b) gasoline (nonpolar)c) I2d) HCl

2. What is the electrical charge and the number of equivalents in 1 Mole of each of the following:

a. Na+ b. Ca2+ c. Fe 3+

d. Cl1- e. SO4

2-

3. Name the following Electrolytes:a. 4 strong electrolytes which are ionic compoundsb. 2 strong electrolytes which are basesc. 5 strong electrolytes which are acidsd. 4 weak electrolytese. 4 non-electrolytes which are carbon compounds

4. Indicate the type of electrolyte represented in the following equations:a. HF(g) + H2O(l) H3O+(aq) + F-(aq)b. NH3(g) + H2O(l) NH4

+(aq) + OH-(aq) c. CaCl2(s) Ca2+(aq) + 2Cl−(aq)

Ch 7.3

1. At 40 C, the solubility of KBr is 80 g/100 g of H2O.Identify the following solutions as either 1 saturated or 2 unsaturated. Explain.

a. 60 g KBr added to 100 g of water at 40 C.b. 200 g KBr added to 200 g of water at 40 C.c. 25 g KBr added to 50 g of water at 40 C.

2. A solution with a solubility of 34g/100g containing 80g of KCl in 200 g of H20 at 50 C is cooled to 20 C.

a) how many grams of KCL remain in the solution at 20 C?b) How many grams of KCL crystallized after cooling?

3. Explain the following observations:A. Why could a bottle of carbonated soda possibly explode when left out in the

hot sun?

B. Why do fish die in water that is too warm?

CH 7.4

1. What is the molarity of 325 mL of a solution containing 46.8 g of NaHCO3?

2. A solution is prepared by mixing 15.0 g of Na2CO3 and 235 g of H2O. Calculate the mass percent (% m/m) of the solution.

3. How many grams of NaCl are needed to prepare225 g of a 10.0% (m/m) NaCl solution?

4. How many grams of NaOH are needed to prepare 75.0 g of 14.0% (m/m) NaOH solution?

5. How many milliliters of a 5.75% (v/v) ethanol solution can be prepared from 2.25 mL of ethanol?

6.How many mL of a 4.20% (m/v) will contain 3.15 g of KCl?

7. How many grams of NaOH are needed to prepare 125 mL of a 8.80% (m/v) NaOH solution?

CH 7.5

1. What is the molarity of 0.500 L of NaOH solution if it contains 6.00 g of NaOH?

2. What is the molarity of 325 mL of a solution containing 46.8 g of NaHCO3?

3.What is the molarity of 225 mL of a KNO3 solution containing 34.8 g of KNO3?

4. How many grams of AlCl3 are needed to prepare125 mL of a 0.150 M solution?

5. How many milliliters of 2.00 M HNO3 contain 24.0 g of HNO3?

6. What volume of a 2.00% (m/v) HCl solution can be prepared by diluting 25.0 mL of 14.0% (m/v) HCl solution?

7. What is the percent (% m/v) of a solution prepared by diluting 10.0 mL of 9.00% NaOH to 60.0 mL?

8. What is the molarity (M) of a solution prepared by diluting 0.180 L of 0.600 M HNO3 to 0.540 L?

9. What is the final volume (mL) of 15.0 mL of a 1.80 M KOH diluted to give a 0.300 M solution?

Ch 7.9

1. A semipermeable membrane separates a 10% sucrose solution A from a 5% sucrose solution B. If sucrose is a colloid, fill in the blanks in the statements below.

A. Solution ____ has the greater osmotic pressure.B. Water initially flows from ___ into ___.C. The level of solution ____will be lower.

2. Indicate if each of the following solutions is 1) isotonic, 2) hypotonic, or 3) hypertonic.

A.____ 2% NaCl solution B.____ 1% glucose solution C.____ 0.5% NaCl solution D.____ 5% glucose solution

3. When placed in each of the following, indicate if a red blood cell will 1) not change, 2) hemolyze, or 3) crenate.

A.____ 5% glucose solution B.____ 1% glucose solution C.____ 0.5% NaCl solution D.____ 2% NaCl solution

CH 8.1

1. What is the correct name for each of the following acids.A. HBr B. H2CO3

C. HBrO2

2.Match the formulas with the names.

A. ___HNO2 1) Iodic acidB. ___Ca(OH)2 2) Sulfuric acidC. ___H2SO4 3) Sodium hydroxideD. ___HIO3 4) Nitrous acidE. ___NaOH 5) Calcium hydroxide

3.Identify each as a characteristic of an A) acid or B) base.

____1. has a sour taste____2. produces OH− in aqueous solutions____3. has a chalky taste____4. is an electrolyte____5. produces H+ in aqueous solutions

4. A. Write the conjugate base of each of the following: 1. HBr 2. H2S 3. H2CO3

B. Write the conjugate acid of each of the following: 1. NO2

−

2. NH3

3. OH−

5. Identify the sets that contain acid-base conjugate pairs.

1. HNO2, NO2−

2. H2CO3, CO32−

3. HCl, ClO4−

4. HS−, H2S5. NH3, NH4

+

6. A. The conjugate base of HCO3− is

1. CO32− 2. HCO3

− 3. H2CO3

B. The conjugate acid of HCO3− is

1. CO32− 2. HCO3

−

3. H2CO3

C. The conjugate base of H2O is 1. OH− 2. H2O 3. H3O+

D. The conjugate acid of H2O is 1. OH− 2. H2O 3. H3O+

CH. 8.2

1. Identify each of the following as a strong or weak acid or base. A. HBr strong acidB. HNO2 weak acidC. NaOH strong baseD. H2SO4 strong acidE. Cu(OH)2 weak base

2. Identify the stronger acid in each pair. 1. HNO2 or H2S 2. HCO3

− or HBr 3. H3PO4 or H3O+

CH 8.3

1. What is the [H3O+] of a solution if [OH−] is 5.0 x 10-8 M?

2. If lemon juice has [H3O+] of 2 x 10−3 M, what is the [OH−] of the solution?

3. The [OH−] of an ammonia solution is 4.0 x 10−2 M. What is the [H3O+ ] of the solution?

CH 8.4

1. Identify each solution as1) acidic 2) basic 3) neutral

A. ___ HCl with a pH = 1.5 B. ___ pancreatic fluid [H3O+] = 1 x 10−8 MC. ___ Sprite® soft drink pH = 3.0

D. ___ pH = 7.0E. ___ [OH−] = 3 x 10−10 MF. ___ [H3O+ ] = 5 x 10−12

2. Calculate the pH for a solution with [H3O+] = 1 x 10−4

3. What is the pH of coffee if the [H3O+] is 1 x 10−5 M?

4. The [H3O+] of tomato juice is 2 x 10−4 M. What is the pH of the solution?

5. The [OH−] of a solution is 1.0 x 10−3 M. What is the pH of the solution?

6. What is the [H3O+] of a solution with a pH of 10.0?

7. What is the [OH−] of a solution with a pH of 2.00?

CH 8.5

1. Write the products of the following reactions of acids.

A. Zn(s) + 2HCl(aq)

B. MgCO3(s) + 2HCl(aq)

2. Write the balanced equation for the neutralization of magnesium hydroxide and nitric acid.

Mg(OH)2 + HNO3

3. Select the correct group of coefficients for each of the following neutralization equations.

A. HCl(aq) + Al(OH)3(aq) AlCl3(aq) + H2O(l) 1) 1, 3, 3, 1 2) 3, 1, 1, 1 3) 3, 1, 1 3

B. Ba(OH)2(aq) + H3PO4(aq) Ba3(PO4)2(s) + H2O(l) 1) 3, 2, 2, 2 2) 3, 2, 1, 6 3) 2, 3, 1, 6

4.Write the neutralization reactions for stomach acid HCl and MylantaTM.Mylanta: Al(OH)3 and Mg(OH)2

5. What is the molarity of an HCl solution if 18.5 mL of 0.225 M NaOH are required to neutralize 10.0 mL of HCl?

HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)

STEP 1: Given: 18.5 mL of 0.225 M NaOH; 10.0 mL of HCl Need: Molarity of HCl

6. Calculate the mL of 2.00 M H2SO4 required to neutralize 50.0 mL of 1.00 M KOH.

H2SO4(aq) + 2KOH(aq) K2SO4(aq) + 2H2O(l)

7. A 25.0 mL sample of phosphoric acid is neutralized by 42.6 mL of 1.45 M NaOH. What is the molarity of the phosphoric acid solution?

3NaOH(aq) + H3PO4 (aq) Na3PO4(aq) + 3H2O(l)

CH 8.6

1. Which combination(s) make a buffer solution? A. HCl and KClB. H2CO3 and NaHCO3

C. H3PO4 and NaClD. HC2H3O2 and KC2H3O2

2. Which of the following would act as a buffer system? A. HCl

B. Na2CO3

C. NaOH and NaNO3

D. NaHCO3 and H2CO3

3. What is true of a typical buffer system?A. It contains a weak base only.B. It maintains a pH of 7.0C. It contains a strong acid and its salt.D. None of these is true.

4. Which of these solutions will form a buffer?A. KOH and KClB. NaHCO3 and H2CO3

C. KF and KClD. HCl and NaOH

CH 10.1 ORGANIC COMPOUNDS 1. Identify each characteristic as most typical of compounds that are 1) inorganic or 2) organic.

A. has a high melting point. B. is not soluble in water.C. has a formula CH3─CH2─CH3.D. has a formula MgCl2.E. burns easily in air.F. has covalent bonds.

CH 10.2 ALKANES 1.Alkanes are written with structural formulas that are expanded to show each _;

condensed to show each and its attached .

2. The names of alkanes are determined by the __________________system; end in _-____________; with 1-4 carbons in a chain Name # Carbons Condensed Structural Formula

ane 1 CH 4

ane 2 CH 3― CH 3

ane 3 CH 3― CH 2― CH 3

ane 4 CH 3― CH 2― CH 2― CH 3

3. A. Write the condensed formula for: H H H H H

H C C C C C H H H H H H

B. What is its molecular formula?C. What is its name?

4. Write the condensed structural formula for:A. ethane.B. heptane.

5. Alkanes with 5-10 carbon atoms in a chain use Greek prefixes.

Name # Carbons Structural Formula

ane 5 CH3CH2CH2CH2CH3

ane 6 CH3CH2CH2CH2CH2CH3

ane 7 CH3CH2CH2CH2CH2CH2CH3

ane 8 CH3CH2CH2CH2CH2CH2CH2CH3

ane 9 CH3 CH2 CH2CH2CH2CH2CH2CH2CH3

ane 10 CH3CH2CH2CH2CH2CH2CH2CH2CH2CH3

6. Name the following.

A. CH3─CH2─CH2─CH3

B.

C. CH3─CH2─CH2─CH2─CH2─CH2─CH2─CH3

D.

CH. 10.31. Write the name of:

Cl CH3

CH3─CH2─CH─CH─CH3

2. Give the IUPAC name for each of the following:

A. CH3 CH3

| | CH3─CH─CH2 ─CH─CH3

B. Cl CH3

| |CH3─CH2─CH─CH2─C─CH2─CH3

| Cl

3. Draw the condensed structural formula for 3-bromo-1-chlorobutane.

4. A three-carbon substituent is called?

5. The substituent in the box is ?

6. What is the IUPAC name of this compound?

7. How would you name this compound?

CH 10.41. Write a balanced equation for the complete combustion of propane.

2. What are the products of the combustion of propane?

3. What is the coefficient in front of carbon dioxide in the balanced combustion reaction of pentane?

CH 10.51. Classify each of the following as: alcohol, ether, aldehyde, ketone, carboxylic acid, ester, amine, or amide.

1) CH3─CH2─CH2─OH2) CH3─O─CH2─CH3

3) CH3─CH2─NH2

O O ║ ║

4) CH3─C─OH 5) CH3─C─O─CH3

2. How many covalent bonds will nitrogen make?

3. What functional group is present in this compound?

4. What functional group is present in this compound?

5. What functional groups are present in this compound?

6. What functional groups are present in this compound?

ANSWERS:

CH. 6.71. 10 L ~ When moles go up, the volume goes up. The amount of moles is 1.42 moles!

2. 19.6 L ~ At STP, 1 mole of any gas occupies 22.4 L of space. The correct solution is 28.0 g x (1 mole / 32.0 g) x (22.4 L / 1 mole) = 19.6 L

3. 11.7 L ~At STP, 1 mole of any gas occupies 22.4 L of space. The correct solution is 14.6 g N2 x (1 mole / 28.0 g) x (22.4 L / 1 mole) = 11.7 L

4. 2.00 moles of O2.

5. 0.179 moles of CO2.

6. 4.48 L.

7. 55 4400 mL.

CH. 6.8

1. 425 torr

2. 9.0 atm When you combine gas samples, you add their pressures to get a new total pressure.

3. 2396 mm Hg 1140 mm Hg O2 + 432.0 mm Hg N2 + 824.0 mm Hg He = 2396 mm Hg.

4. a. A b. C c. A d. B e. C

CH 7.1

1. A. 2 g of sugar B. 30.0 mL of methyl alcohol C. 1.5 g of NaCl D. 200 mL of O2

CH 7.21. Most polar and ionic solutes dissolve in water because water is a polar solvent.

a) Na2SO4 yes, ionicb) gasoline no, nonpolarc) I2 no, nonpolard) HCl yes, polar

2. An equivalent (Eq) is the amount of an ion that provides 1 mole of electrical charge (+ or -).

a. Na+ = 1+ 1Eqb. Ca2+ = 2+ 2Eqc. Fe 3+ = 3+ 3Eqd. Cl1- = - 1Eqe. SO4

2- = 2- 2Eq

3. Name the following Electrolytes:a. 4 strong electrolytes which are ionic compoundsNaCl, KBr, MgCl2, NaNO3b. 2 strong electrolytes which are basesNaOH, KOHc. 5 strong electrolytes which are acidsHCl, HBr, HNO3, HClO4, H2SO4d. 4 weak electrolytesHF, H20, NH3, HC2H3O2

e. 4 non-electrolyte carbon compoundsCH3OH, C2H5OH, C12H22O11, CH4N2O

4. Indicate the type of electrolyte represented in the following equations:a. a weak electrolyte dissociates partially : HF(g) + H2O(l) H3O+(aq) +

F-(aq)b. a weak electrolyte dissociates partially : NH3(g) + H2O(l) NH4

+(aq) + OH-(aq)

c. a strong electrolyte dissociates completely : CaCl2(s) Ca2+(aq) + 2Cl−

(aq)

CH 7.3 1. A. 2 Amount of 60g KBr/100 g of water is less than the solubility of 80 g KBr/100 g of water. B. 1 In 100g of water, 100g of KBr exceeds the solubility of 80 g KBr /100 g of water at 40 C. C. 2 This is the same as 50g KBr in 100g of water, which is less than the solubility of 80g KBr/ 100g of water at 40C.

2. a)68g of KCl b)12 g of KCl

3. a)The pressure in a bottle increases as the gas leaves solution when it becomes less soluble at higher temperatures. As pressure increases, the bottle could burst.

b) Because O2 gas is less soluble in warm water, fish cannot obtain the amount of O2 required for their survival.

CH 7.41) 46.8 g NaHCO3 x 1 mole NaHCO3 = 0.557 mole NaHCO3

84.0 g NaHCO3

0.557 mole of NaHCO3 = 1.71 M NaHC 0.325 L

2) STEP 1: mass solute = 15.0 g of Na2CO3 mass solution = 15.0 g + 235 g = 250. gSTEP 2: Use g solute/g solution ratio

STEP 3: mass %(m/m) = g solute x 100 g solutionSTEP 4: Set up problem mass %(m/m) = 15.0 g Na2CO3 x 100 = 6.00%

Na2CO3 250. g solution

3. STEP 1: Given: 225 g solution; 10.0% (m/m) NaCl Need: g of NaCl

STEP 2: g solution g NaClSTEP 3: Write the 10.0% (m/m) as conversion factors.10.0 g NaCl and 100 g solution 100 g solution 10.0 g NaClSTEP 4: Set up using the factor that cancels g solution.

225 g solution x 10.0 g NaCl = 22.5 g NaCl 100 g solution

4. 10.5 g NaOH

5. 39.1mL solution

6. 75.0 mL KCl

7. 11.0 g NaOH

CH 7.5

1. 0.300 M NaOH

2. 46.8 g NaHCO3 x 1 mole NaHCO3 = 0.557 mole NaHCO3

84.0 g NaHCO3

0.557 mole of NaHCO3 = 1.71 M NaHCO3 0.325 L

3. 34.8 g KNO3 x 1 mole KNO3 x 1 = 1.53 M 101.1 g KNO3 0.225 L

4. 2.50 g AlCl3

5. 190. mL of HNO3

6. C1V1 = C2V2

V2 = V1C1 = (25.0 mL)(14.0%) = 175 mLC2 2.00%

7. C2= C1 V 1 = (10.0 mL)(9.00%) = 1.50% (m/v) V2 60.0 mL

8. M1V1 = M2V2

M2 = M1V1 = (0.600 M)(0.180 L) = 0.200 M V2 0.540 L

9. 90.0 mL

CH 7.9

1. A. Solution A has the greater osmotic pressure.B. Water initially flows from B into A.C. The level of solution B will be lower.

2. A. 3 2% NaCl solution B. 2 1% glucose solution C. 2 0.5% NaCl solution D. 1 5% glucose solution

3. A._1_ 5% glucose solution B._2_ 1% glucose solution C._2_ 0.5% NaCl solution D._3_ 2% NaCl solution

CH 8.1

1. A. HBr is hydrobromic acidThe name of an acid with H and a nonmetal uses the prefix hydro and ends

with ic acid.

B. H2CO3 is carbonic acid

An acid with H and a polyatomic ion is named by changing the end of an ate ion to ic acid.

C. HBrO2 is bromous acidThis acid of bromite (BrO2

-) is bromous acid.2. A. 4 HNO2 Nitrous acid

B. 5 Ca(OH)2 Calcium hydroxideC. 2 H2SO4 Sulfuric acidD. 1 HIO3 Iodic acid E. 3 NaOH Sodium hydroxide

3. A 1. has a sour tasteB 2. produces OH− in aqueous solutions B 3. has a chalky tasteA, B 4. is an electrolyteA 5. produces H+ in aqueous solutions

4. A. Remove one H+ to write the conjugate base. 1. HBr – H+ Br−

2. H2S – H+ HS−

3. H2CO3 – H+ HCO3−

B. Add one H+ to write the conjugate acid.

1. NO2 −+ H+ HNO2

2. NH3 + H+ NH4+

3. OH− + H+ H2O

5. 1. HNO2, NO2−

4. HS−, H2S5. NH3, NH4

+

6. A. The conjugate base of HCO3 − is—1. CO3

2−

B. The conjugate acid of HCO3− is—3. H2CO3

C. The conjugate base of H2O is—1. OH− D. The conjugate acid of H2O is—3. H3O+

CH. 8.2

1. A. HBr strong acidB. HNO2 weak acidC. NaOH strong baseD. H2SO4 strong acidE. Cu(OH)2 weak base

2. 1. HNO2 2. HBr 3. H3O+

CH. 8.3

1. STEP 1: Write the Kw for water.Kw = [H3O+ ][OH− ] = 1.0 x 10−14

STEP 2: Rearrange the Kw expression.

[H3O+] = 1.0 x 10 -14 [OH−]

STEP 3: Substitute [OH−]. [H3O+] = 1.0 x 10 -14 = 2.0 x 10-7 M

5.0 x 10- 8

2. 5 x 10−12 M

Rearrange the Kw to solve for [OH− ]Kw = [H3O+ ][OH− ] = 1.0 x 10−14

[OH− ] = 1.0 x 10 -14 = 5 x 10−12 M 2 x 10 - 3

3. 2.5 x 10−13 M

[ H3O+] = 1.0 x 10 −14 = 2.5 x 10−13 M 4.0 x 10−2

CH 8.4

1. A. 1 HCl with a pH = 1.5 B. 2 pancreatic fluid [H3O+] = 1 x 10−8 MC. 1 Sprite® soft drink pH = 3.0D. 3 pH = 7.0E. 1 [OH−] = 3 x 10−10 MF. 2 [H3O+] = 5 x 10−12

2. pH = −log [1 x 10−4 ]pH = - [-4.0]pH = 4.0

Note: The number of decimal places in the pH equals the significant figures in the coefficient of [H3O+].

4.0 1 SF in 1 x 10-4

3. pH = 5.0pH = -log [1 x 10−5] = -(-5.0) = 5.0

4. 3.7pH = - log [ 2 x 10-4] = 3.72 (EE) 4 (+/-) log (+/-)

5. 11.00 Use the Kw to obtain [H3O+] = 1.0 x 10 −11

pH = - log [1.0 x 10 −11] 1.0 (EE) 11 (+/-) log (+/-)

6. What is the [H3O+] of a solution with a pH of 10.0? 1 x 10-10 M 1 x 10-pH

7. What is the [OH−] of a solution with a pH of 2.00? 2) 1.0 x 10−12 M

[H3O+] = 1.0 x 10−2 M 1 x 10-pH

[OH−] = 1.0 x 10 −14 = 1.0 x 10−12 M 1.0 x 10−2

CH 8.5

1.Write the products of the following reactions of acids.

A. Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g)

B. MgCO3(s) + 2HCl(aq) MgCl2(aq) + CO2(g) + H2O(l)

2. Write the balanced equation for the neutralization of magnesium hydroxide and nitric acid.

STEP 1: Write the acid and base. Mg(OH)2 + HNO3

STEP 2: Balance H+ in acid with OH− in base. Mg(OH)2+ 2HNO3

STEP 3: Balance with H2O. Mg(OH)2 + 2HNO3 salt + 2H2O

STEP 4: Write the salt from remaining ions. Mg(OH)2 + 2HNO3 Mg(NO3)2 + 2H2O

3. A. 3) 3, 1, 1 3 3HCl(aq) + Al(OH)3(aq) AlCl3(aq) + 3H2O(l)

B. 2) 3, 2, 1, 6 3Ba(OH)2(aq) + 2H3PO4(aq) Ba3(PO4)2(s) + 6H2O(l)

4. 3HCl(aq) + Al(OH)3(aq) AlCl3(aq) + 3H2O(l)

2HCl(aq) + Mg(OH)2(aq) MgCl2(aq) + 2H2O(l)

5. STEP 1: Given: 18.5 mL of 0.225 M NaOH; 10.0 mL of HCl Need: Molarity of HCl

STEP 2: 18.5 mL L moles NaOH moles HCl M HCl L HCl

STEP 3: 1 L = 1000 mL 0.225 mole NaOH/1 L NaOH 1 mole HCl/1 mole NaOHSTEP 4: Calculate the molarity of HCl.18.5 mL NaOH x 1 L NaOH x 0.225 mole NaOH

1000 mL NaOH 1 L NaOH

x 1 mole HCl = 0.00416 mole HCl 1 mole NaOH

MHCl = 0.00416 mole HCl = 0.416 M HCl

0.0100 L HCl

6. 0.0500 L KOH x 1.00 mole KOH x 1 mole H2SO4 x 1 L KOH 2 mole KOH 1 L H2SO4 x 1000 mL = 12.5 mL 2.00 mole H2SO4 1 L H2SO4

7. 0.0426 L x 1.45 mole NaOH x 1 mole H3PO4 = 0.0206 mole H3PO4

1 L 3 mole NaOH

0.0206 mole H3PO4 = 0.824 mole/L = 0.824 M 0.0250 L

CH 8.6

1. B. H2CO3 + NaHCO3 A weak acid and its salt.D. HC2H3O2

+ KC2H3O2 A weak acid and its salt.

2. NaHCO3 and H2CO3

A buffer is composed of a weak acid and its conjugate base (or a weak base and its conjugate acid).

3.NaHCO3 and H2CO3

A buffer is composed of a weak acid and its conjugate base (or a weak base and its conjugate acid).

4. B—only solution B will form a buffer.

CH 10.11. Identify each characteristic as most typical of compounds that are 1) inorganic or 2) organic. 1 A. has a high melting point.

2 B. is not soluble in water.2 C. has a formula CH3─CH2─CH3.1 D. has a formula MgCl2.2 E. burns easily in air.2 F. has covalent bonds.

CH 10.21. Alkanes are written with structural formulas that areexpanded to show each bond.condensed to show each carbon atom and its attached hydrogen atoms.

2.The names of alkanes are determined by the IUPAC system; end in – ane ; with 1-4 carbons in a chain. Name # Carbons Condensed Structural Formula Methane 1 CH4

Ethane 2 CH3―CH3

Propane 3 CH3―CH2―CH3

Butane 4 CH3―CH2―CH2―CH3

3. A. CH3─CH2─CH2─CH2─CH3

B. C5H12

C. pentane

4. A. ethane CH3─CH3

B. heptane CH3─CH2─CH2─CH2─CH2─CH2─CH3

5. Alkanes with 5-10 carbon atoms in a chain use Greek prefixes.Name # Carbons Structural FormulaPentane 5 CH3CH2CH2CH2CH3

Hexane 6 CH3CH2CH2CH2CH2CH3

Heptane 7 CH3CH2CH2CH2CH2CH2CH3

Octane 8 CH3CH2CH2CH2CH2CH2CH2CH3

Nonane 9 CH3 CH2 CH2CH2CH2CH2CH2CH2CH3

Decane 10 CH3CH2CH2CH2CH2CH2CH2CH2CH2CH3

6. Name the following.A. CH3─CH2─CH2─CH3 butane

B. cyclopropane

C. CH3─CH2─CH2─CH2─CH2─CH2─CH2─CH3 Octane

D. Cyclohexane

CH 10.3

1. Write the name of:STEP 1:Longest chain is pentane.STEP 2:Number chain from end nearest substituent.

Cl CH3 CH3─CH2─CH─CH─CH3

5 4 3 2 1

STEP 3:Locate substituents and name alphabetically. 3-chloro-2-methylpentane2. A. CH3

CH3

| | CH3─CH─CH2 ─CH─CH3 2,4-dimethylpentane

1 2 3 4 5

B. Cl CH3 more substituents on C3 | |

CH3─CH2─CH─CH2─C─CH2─CH3 | 7 6 5 4 3 2 1

Cl 3,5-dichloro-3-methylheptane

3. 3-bromo-1-chlorobutaneSTEP 1: Longest chain has 4 carbon atoms.

C─C─C─C

STEP 2: Number chain and add substituents. Br

C ─ C ─ C ─ C ─ Cl

4 3 2 1STEP 3: Add hydrogen to complete 4 bonds to each C.

Br CH3─CH─CH2─CH2─Cl

4. A three-carbon substituent is called propyl.- Substituents have the ending -yl

5. The substituent in the box is?

A branched three-carbon substituent is an isopropyl group.

6. What is the IUPAC name of this compound?

 3-bromo-2-chloropentane — The bromo substituent is on carbon 3 and the chloro substituent is on carbon two. List the two substituents alphabetically, not numerically.

7.How would you name this compound?

  —ethylcyclohexane

8. What is the relationship between these compounds?

  They are identical compounds—which have identical molecular formulas and the atoms are connected in the same manner. CH 10.4

1. Write a balanced equation for the complete combustion of propane.Unbalanced equation

C3H8 + O2 CO2 + H2OBalance C

C3H8 + O2 3CO2 + H2OBalance H

C3H8 + O2 3CO2 + 4H2OBalance O

C3H8 + 5O2 3CO2 + 4H2O (Balanced)

2. What are the products of the combustion of propane?-Combustion reactions produce water and carbon dioxide.

3. What is the coefficient in front of carbon dioxide in the balanced combustion reaction of pentane?  —5 One molecule of pentane reacts with 8 molecules of oxygen gas to produce 5 molecules of carbon dioxide and 6 molecules of water.

CH 10.5

1. 1) CH3─CH2─CH2─OHalcohol2) CH3─O─CH2─CH3 ether3) CH3─CH2─NH2 amine

O O ║ ║

4) CH3─C─OH 5) CH3─C─O─CH3

carboxylic acid ester

2. How many covalent bonds will nitrogen make?-three

3.What functional group is present in this compound?

This compound is an ether.

4. What functional group is present in this compound?

This compound is an alcohol.

5. What functional groups are present in this compound?

This compound is an ester.

6.What functional groups are present in this compound?

This is an amine and a ketone.