Examination June 1985 Chemistry PART ONE Answer af/56 qUDltions ill this part. (65]

DIRECTIONS (1-56): For each statement or question, select the scord or crpressiml that of IhOOf' gin'lI, best compleres the statement or answers til(' qll('sliorl Record your OIlSWI'r ill the space pravided at the right.

1 Which temperature is the same as -130 Celsius? (I) 260 K (3) 747 K (2) 286 K (4) 773 K J__

2 Which substance can not be decomposed by a chemical change? 1 mercury (11) oxide 3 water 2 potassium chlorate 4 copper "­

3 A gas occupies a volume of30 milliliters at 273 K. If the temperature is increased to 364K while the pressure remains constant, what will be the vel­ume of the gas? (I) 60 ml (2) 40 ml

(3) 30 ml (4) 20 ml 3__

4 At 1 atmosphere, which substance will sublime when heated? (I) CO,(s) (3) CH.(g) (2) H,O(() (4) HCI(aq) '- ­

5 Which particle has a negative charge? 1 alpha particle 3 proton 2 beta particle 4 neutron '- ­

1

EXAMINATiON June1985 Chemistry 2

6 The amount of energy required to remove the most loosely bound electron from an atom in the gaseous phase is called 1 kinetic energy 3 ionization energy 2 potential energy 4 electron affinity 6__

7 What is the total number of electrons in an atom with an atomfe number of 13 and a mass number of 271 (I) 13 (3) 27 (2) 14 (4) 40 '- ­

8 Which atom in the ground state contains only one orbital that is partially occupied? (I) Si (3) Ca (2) Ne (4) Na 8__

9 What is the maximum number of sublevels in the third principal energy level? (1)1 (3)3

9__(2)2 (4)4 ,

10 If X is the symbol of an element, which pair cor­rectly represents isotopes of X? (1) J~ and l~X (3) l~X and 1:1X

(2) l~X and I~X (4) l~X and l1:X 10__.

11 The number of valence electrons in an atom with an electron configuration of ls22s22/,e.3s 23p 4 is (I) 6 (3) 16 (2) 2 (4) 4 11__

EXAMINATION June1985 Chemistry 3 EXAMINATION June 1985 Chemistry 4

12 Whieh oxide?

is the correct formula for nitrogen (IV) 18 The strongest hydrogen bonds art:' formed he ­tween molecules in which hydrogen is covalently

(1) NO (3) NO, bonded to an element with

(2) NO, (4) NO, '''-­1 high electronegativity and large atomic rudiu, 2 high electronegativttv and small atomic radius 3 low electronegattvity and large atomic radius

13 Which is an empirical formula? 4 low electronegativity and small atomic radius 18__

il) C,H, (2) C,H,

(3) AhCl, (4) "'0 13__

19 The pair of elements chemical properties are

with the most similar

(I) Mg and S (3) Mg and Ca

U When the ejluation Cd-l" + 02 __ C02"" nso is (2) Ca and Br (4) Sand Ar 19__

balanced using smallest whole numbers, what is the coeffteient of the 02? W More than two-thirds of the elements of tlu­

(1) 1 (2)2

(3) 3 (4)4 14__

Periodic Table are 1 metalloids 2 metals

3 nonmetals 4 noble gases 20__

15 Why is N'I-IJ classified as a polar molecule? 21 Which element is a member of the halogen

(1) NH.1 is a gas at STP. family?

(2) l\~H bonds are nonpolar. (3) Nitrogen and hydrogen are both nonmetals.

(1) K (2) B

(3) I (4) S 21 __

(4) NHJ molecules have asymmetric-a I charge distributions. 15__ 22 Which of the following dements has the JrllL'{'.\·/

eleetronegativrty?

16 The greatest degree of ionic character would he found in a bond between sulfur and

1 carbon 2 fluorine

3 nitrogen 4 oxygen 2l!

1 oxygen 2 chlorine

3 bromine 4 phosphorus 16__ 23 Which are two properties of most nonmetals'?

1 low ionization energy and good electrical eon­duetivity

17 Helium may be liquefied at low temperature and 2 high ionization energy and poor electrical con­high pressure primarily because of ductivity 1 hydrogen bonding 3 low ionization energy and poor electrical con­2 covalent bonds ductivity 3 van dee Waals forces 4 high ionization energy and good electrical con­4 ionic attraction 17__ ductivity sa

EXAMINATION June1985 Chemistry 5 EXAMINATION June 1985 Chemistry 6 24 Which g;mllp contains ele-me-nts with <l total 01

:30 A z.Oo-gram sample of helium g~'s at STP \\ill tour electrons in the outermost principal energy level? occupy

(1)11.21 (3) 33.6 (II IA (.3) VIA 30__(2) 224 ( (4) 44.0 ( (-Id IVA2) ° "'-- ­

2.') \Vhich element exlulutv a crystalline structure at 31 The effect of a catalyst on a chemical reaction iv to STP! change the 1 Iluonne :3 hromine 1 activation energy

.:2 chlorine ..j, iodine 25__ 2 heat of reaction 3 potential energy of the products 4 potential energy of the reactants 31__

26 What is the percent by muss ofoxygen in FC203 (formula mass = 1601? (J) 16"/r (2) 30. 'Ie

(.3) 56"-1 (41 70.q --­ .32 According to Reference Table G, the greatest

amount of energy would be given lip by the com­plete oxidation of 1 mole or'

27 Which quantity is equivalent to .39 grams of Li F? (lJ 1.0 mole (.3) 0.50 mole

(1) CH.(g) (2) C,H,(g)

(3) CH,OH(f) (4) C,H"O,(,) 32___

(2) 2.0 moles (4) L5 moles 27__ 33 Consider the reaction; ,

lbO(f) + energy ~ lh(g) + T02(g) 28 If 0.50 liter of a 12-molar solution is dllnted to

1.0 'iter, the molarity of the new solution is Which phrase best describes this reaction? , (1) 2.4 (3) 12 1 exothermic, releasing energy (2) 6.0 (4) 24 28__ 2 exothermic, absorbing energy

3 endothermic, releasing energy 4 endothermic, absorbing energy :l:L­

29 Given the reaction: 4NH,(g) + 50,(g) ­ 4NO(g) + 6IhO(g) 34 In a gaseous system, temperature remaining con­

At cunstant pressure, how many liters of 02(~) stant, an increase in pressure will would be required to produce -10. liters ofNO(~)? 1 increase the activation energy (I) 50 (2) 9.0

(3) 32 (4) 50. 29_

2 decrease the activation energy 3 increase the reaction rate 4 decrease the reaction rate 34..-­

EXAMINATION June 1985 Chemistry 7 EXAMINATION June 1965 Chemistry 8

3" Given the equilibrium: AgCI(s) '" Ag·(o<!1 + C] (aq:

The equilibrium constant will chang!' if there is an increase in the

41 Given the reaction: Sn2+(aq', + 2FeJ~ia(t'1 ;....:.. Sn~' (aq) + Lh·':· (aqJ

The total number of 1I101t-'S of electrons lmt bv 1 mole of Sn2

t is 1 concentration of Ag~ iUlI:S

2. concentration of CI- ions :3 pre5;;ure 4 temperature 35__

--1;;

(3) 3 (4) 4

(1)1 (21 :2

What is the oxidation number of sulfur in lhS04?

.1

36 According to Reference Tablej , which of the fol­lowing is the strongest Bn)]lstl?d acid? (I) HNO, (31 CH,COOH (2) i),5 (4) H,PO, 36__

il} 0 III -2

--13 in Ilw re.u-tton

(3) +6 (4) +..j. 4'-­

17 Given the reaction: 1l\IU:2 (<ttl);2 H' (aq) + ~02- {<If';

The ionization constant, J.:", is equal to

4Hel + MnOz -. :MnCh + 2H20 + Cb, the manganese is

1 reduced and the OXidation number ch'Ulge~ from +--1 to +2

(I)

(21 .

IHNO,] [W][NO,·]

[W][NO,-: [HNO,j

. I

(3.

(4)

[NO,-J [n ][HNOz]

[W][HNO,[ [1\0, ]

37__

2 oxidized and the OXidation number changes from +4 to +2

:3 reduced and the oxidation number challge~ from +2 to +4

4 oxidized and the oxidation number changes from +2 to + 4 43__

:38 Pure water at 25°C has a pH of

(I) 1 < iot (31 7 (2)I<lO" (4)14 38__

44 In the reaction 2Na + 2H20 - 2:1\a+ stance oxidized Is

+ 20H ­ + Hz, the sub­

39 Which metal HCI(a,,)? (l1 Au (2) Ag

will

(3) Cu (4) Mg

read spontaneously with

39__ 45 Clven the reaction:

(I) If,

(2) W (3) Na (4) Na' 44_­

40 In the reaction ffcI + H~O ~ 1-1:10" + CI-, conjugate acid-base pair is (1) HC] and H,O· (3) HC! aud C! (2) HCI and H,O (4) H,O and CI·

a

'0__ (3) Cu +2

(4) N+2

3Cu + 8HN03 -- 3Cu(NOaht + 2NO + 4H20 The reducing agent is

(1) Cu" (2) W' 45__

, EXAMINATION June1965 Chemistry 9 EXAMINATION June 1985 Chemistry 10

46 How many moles of electrons are needed to re­duce one mole of Cu'' > to Cu 1+?

Note that questions ,52 through 56lwve only three choices.

,I) I (2) 2

(3) 3 (4) 4 46__

52 As a gtveu volume of gas is compressed, the num­ber of molecules

47 Which compound is an isomer ofCI-bCOOCH:l? 1 decreases 2 Iucreases

(I) cn-ocu, (2) CH,ClhCOOH

(3) CH,COClh (4) Clf,ClhClhOH 47__

3 remains the same 52__

48 Which molecule is represented by .\ in the reac­tion H-~-H + 2Br2 --,10 X?

H H I I

(I) H-C-C-B, I IH H

H H I I

(3) H-C-C-B, I I

H B, -

53 A sample of lhO(() at 20"C is in eq utlibrium with its vapor in a sealed container. When the tem­perature increases to 25"C, the entropy of the system will 1 decrease 2 increase 3 remain the same 53__

(21

H H I I

H-C-C-H I i Br Br

Br Br I I

(4) H-C-C-H I I Br Br

46__

54 Given the reaction at equilibrium: Ba50.(,) "" Ba"(aq) + 50.'-(aq)

As the concentration of the so,» ions is In­creased, at constant temperature, the concentra­tion of Ba2+ ions

49 The structure represent

~ ~

or @ may be used to

I decreases 2 Increases 3 remains .the same 54__

I benzene 2 methane

3 acetylene 4 cyclopropane 49__

55 As the '-1:10+ ion concentration of a solution in­creases. the pH of the solution I decreases

50 Which compound is a saturated hydrocarbon? I ethene 3 ethylene 2 ethane 4 ethyne "'-­

2 increases 3 remains the Same 55__

51 The compound C2H2 belongs to the series ofhy­drocarbons with the general formula

(I) C"H" (3) C".H,"-, (2) GlRH:tR (4) Ct"H2,d

51__

56 As a .l-gram sample of IhO(f) changes to H20(g) at lOO"C, the potential energy of the molecules 1 decreases 2 increases 3 remains the same 56__

12 EXAMINATION June1985 Chemistry 11

PARTlWO

ThLI' part CO/lsisls oj twelve groups. Choose severlaj these 'wehw groups. Be sure to answer all questions ill each g('(lllp chosen. Write 'lie cnsu.ers to these quce­!iOIIS irl the space provided,

GIIOUP I-Matter and Energy

DIRECTIONS (57-61); Record each answer ill the space urocided .

57 A sealed flask contains 1 mole of hydrogen and 3 moles of helium at 20°C. If the total pressure is 400 torr, the partial pressure of the hydrogen is (I) 100 ton (3) 300 ton

57__(2) 200 ton (4) 400 ton

58 A sample ofnitrogen containing 1.5 X 1()23 mole­cules has the same number of molecules as a. SCUll­

pie containing (I) 1.0 mole of H, (3) 0.25 mole of 0,

58__(2) 2.0 mole, of He (4) 0.50 mole of Ne

59 Which term represents the change of a substance from the solid phase to the liquid phase? 1 condensation 3 evaporation

59__2 vaporization 4 fusion

60 Under which conditions does a real gas behave most like an ideal gas? 1 at high temperatures and low pressures 2 at high temperatures and high pressures 3 at low temperatures and low pressures 4 at low temperatures and high pressures 00__

EXAMINATION June 1965 Chemistry

61 At constant temperature, which line best shows the relationship between the volume of an ideal gas and its pressure?

t B D

V>

'"~ c -...J

.!:

E'":>

~I/~ --- I

o Pressure (mm of Hg) ..

(I) A (3) C (2) B (4) D 61__

GROUP 2-Atomic Structure

DIRECTIONS (62-66): Record each cnsuier ill the space provided.

62 Which two particles have approximately the same mass? 1 neutron and electron 3 proton and neutron 2 ueutron and deuteron 4 proton and electron 62__

63 The element with atomic Humber 10 has an elec­tron configuration that is the same as (I) Na (3) CI (2) Na' (4) CI 63__

, EXAMINATION Junel985 Chemistry 13

64 Which electron dot symbol could represent a metalloid?

(I) X' (3) :X:

(2) X: (4) ·X·

65 Which diagram correctly represents an atom of flnorine in an exeited state?

2. 2, ,."

{II (j) (ll (j](j](j) o {21 (j] (j]1jJ)(j]o o "I (j) (j] (j](j](j) o (41 IjJ) (j] (j]1jJ)(j) (j)

86 How many grams of a 32-gram sample O{32P will remain after 71.5 days? (I) I (3) 8 (2) 2 (4) 4.

GROUP 3-Bonding

DIRECTIONS (67-71): Record each answer ;11 the space provided.

67 Which compound contains ionic bonds? (I) NaBr(,) (3) C.H"O.(s) (2) HBr(g) (4) CO,(g)

68 Which molecule contains a nonpolar covalent bond? (I) HCI (3) CO, (2) F, (4) NH,

64__

65__

66__

67__

68__

,.EXA-..INATION June 1985 Chemislry

69 Which type of solid does pnre water form when it freezes? 1 ionic 3 metallic 2 network 4 molecular

70 Whieh symbol represents a molecule at STP? (I) H (3) Kr (2) N (4) Br

71 At 298 K, the vapor pressure of H20 is less than the vapor pressure of CS2 • TIle best explanation for this is that H20 has 1 larger molecnles 2 a larger molecnlar mass 3 stronger ionic bonds 4 stronger mtermoleculer forces

GIIOUP 4-Periodic Table

DIRF.CTIONS (72-76): Record each answer in the space provided. .

72 Which period contains three elements that com­monly exist as diatomic molecules? 1 Period 1 3 Period 3 2 Period 2 4 Period 4

73 Which is an alkaline earth metal? (I) Mg (3) Li (2) Zn (4) Ph

74 The S:l- ion differs from the So atom in that the S2- ion has a 1 smaller radius and fewer electrons 2 smaller radius and more electrons 3 larger radius and fewer electrons 4 larger radius and more electrons

69__

70__

71 __

72__

, 73__

74__

EXAMINATION June 1985 Chemistry

75 An aqueous solution of .\Ch contains colored ions. Element .\ is most likely 1 all alkaline earth 3 a transition metal 2 a halogen 4 an alkali metal

76 A reason why {luor-ine has a higher ionization energy than oxygen is that fluorine has a 1 smaller IHI(·If'~~r e-borge 2 larger nuclear charge 3 smaller number of neutrons 4 larger number of neutrons

GI\OUP 5-Mat.hematics of Chemistry

DIRECTJONS (77-81); Record each Gll~ln'T ill the space nmoided .

77 What is the molecular formula of a compound whose empirical formula is CH4 and molecular mass is 16? (I) CH, (3) C,H, (2) C2H4 (4) CIlHu

78 How many moles of hydrogen atoms are there in one mole of C6H1206 molecules? (I) 24(6.0 x 10") (3) 24 (2) 12(6.0 x 10"') (4) 12

79 The density of a gas is 2.0 grams per liter at STP. Its molecular mass is approximately (1) 67 (3) 22 (2) 45 (4) 8.0

80 A 5-gram sample of water is heated and the tem­perature rfses from ro-c to 15°C. The total amount of heat energy absorbed by the water is (1) 25 cal (3) 15 cal (2) 2Il cal (4) 5 cal

15

75__

76__

77__

"-­

79__

"'- ­

EXAMINATION June1985 Chemistry

81 What is the ratio by mass of carbon to hydrogen in the compound C2H6? (1) 6,2 (3) IA (2) 2,6 (4) 4,1

GROUP 6-Kineti~ and F.fluilibrium

D1ROCTIONS (82-86): Rec/lrd each onsuer in the space prodded.

82 Why does the reaction K(s) + fCb (g) --.. KCI(s)

occur spontaneously? [Refer to Reference Table E.] (1) DS is positive. (3) DC is positive. (2) flS is negative. (4) 6.G is negative.

83 Based on Reference Table J\. a saturated solution of which salt would be most dilute? (I) AgCI (3\ ZnS (2) B,SO, (41 PbCrO,

S4 For a chemical reaction. the free energy change, 6.C, is equal to (1) 611 + T6S (3) T611 + 65 (2) 6H - T6S (4) T6S - 6H

85 Given the reaction at equilibrium: Mg(OH),(s) '" Mg"(aq) - ZOW(aq)

What is the correct expression for the solubility product constant for this reaction? (1) J'" ~ [Mg>+][20W] (2) J',. ~ [Mg") + [20W] (3) J',. ~ (Mg"][OW]' (4) J'" ~ (Mg"j + lOW]'

16

'1__

82~_

83__

84__

,

"'- ­

EXAMINATION June1985 Chemistry 17

86 Based on Reference Table K, in a saturated solu­tion of BaS04 at 1 atmosphere and 291;1 K. the product of {Ba2 f- ] X \5042-] is equal to (I) l.l x 10-" (3) l.l x 10" (2) 1.1 x 10-' (4) i.i x 10" 8"----

GROtiP 7-Acids and B8.'Mlll

DIRECTIONS (87-91): Record each ansu:er in the space pravided .

87 ]0 thf' reaction H20 + H20 _ lh04 + OH-, the water is acting as 1 a proton acceptor, only 2 a proton donor, only 3 both a proton acceptor and donor 4 neither a proton acceptor nor donor 87__

88 Which solution will turn litmus from red to blue? (I) IhS(aq) (3) SO,(aq)

88__(2) I'H,(aq) (4) CO,(aq)

89 Which solution listed below is the best conductor of electricity? (I) 01 M C,H,OH (3) 0.1 M C,H"O,

89__(2) 0.1 M CH,COOH (4) 0.1 M HNO,

90 The rOH-] of a solution is 1 x 10-6 , At 1 atmo­sphere and 298 K, the product of the [H,O+]lOWj is

(I) I x 10-' (3) I x 10-' 00__(2) I x 10-' (4) I X 10-"

91 According to Reference Table], whteh is an am­phiprotic ion? (I) HSO.­ (3) NO,­

91__(2) NH4+ (4) C!­

,.EXAMINATION June1985 Chemistry

csocr 8-Redox and Electrochemistry

DlROCTmN~' (92--96): Rewrd each anauier in the space provided.

92 What is the voltage for a chemical cell that has reached equihbnum? (I) I (3) between 0 and 1 i2} greater than 1 (41 0

Base your answers to questions 93 and 94 on the diagram below which represents a cbemteal cell at 298 K. The equation which accompanies the diagram represents the net cell reaction.

Switch 5

AI"""""""'I

LaM AHNOi)3

VOlf/Mter

LOW Cu(NO.)z

c, ::;~../ 'olidgt

2AI0(S) + 3Cu:l+{aq) -+ 2..\I:l+(aq) + 3Cu D{s)

93 When switch S is closed, the maximum potential (EO) tor the cell will he

(1) 1.32 volts (3) -132 volts (2) 2.00 volt, (4) -2.00 volt,

94 When switch S is dosed, electrons in the ex­ternal circuit will flow from (I) AI to AI'+ (3) Cu '0 AI (2) Alw c« (4l Cu to Cu2+

9'­

93_

"'-­

CYA U.I..I AT.'·..... 'une1985 Chemistry

95 \Vhkh atom-Ion pair will react spontaneously un­der standard condtnons? (I) .\fg + Li' (3) Mg + Ag ' (2) Mg + Ba2 - (4) Mg + S.... 9'__

96 During the electrolysis of fused KBr, which reac­hen occurs at the positive electrode? OJ Br" ions are oxidized. (2) Br ions are redncpd. (3) KT ions are reduced. (4) K~ ions are oxidized. 96__

GflQUP 9-0f~anic Chemistry

DIRECTIONS (97-101): Record each On.t!N7 in the space provided.

97 Which compound is a dthydroxy alcohol? (1) Al(OH), (3) Ca(OH). (2) C,H,(OH), (4) C.H.(OH). 97__

98 Which is the formula of a primary alcohol?

H 0 H HI II I I(11 H-C-C (3) H-C-C--QHI \ I IH OH H H

o H H II I I(2) H~C (4) H-C--C--0H 98_\ I IH H H-C-H

I u

99 The name of the compound having the formula CJH5(OH):J is 1 glycerol 3 propene 2 ethylene glycol 99__4 propanoic acid

20

100__

101 Which of the following compounds has the IOU:t:,~·t

normal boiling point? 1 butane 3 methane 2 ethane 4 propane 101__

GROUP lO-Applicalioru of Chemir:aJ Principles

DIRECTIONS (102-106): Record each answer itl the space procided ,

102 Which oxide will react with carbon (coke) to pro­duce a free metal? (1) MgO (3) N..,O (2) zso (4) U.O 10"----­

103 Which process inereases the yield of gasoline and kerosene from crude oil? 1 oxidation 3 Haber 2 cracking 4 contact 10"­

104 Which represents the positive electrode of a nickel-cadmium battery? (11 Ni(OH), (3) Ni (2) Cd (4) Cd(OH). 104__

~

105 Which metal is usually obtained by electrolytic reduction? 1 iron 3 lead 2 tin 4 potassium 105__

-----

EXAMINATION June1985 Chemislry 21 Ir EXAMINATION June1985 Chemistry 22

106 Which reaction correctly represents the step in III In tht' reaction gAl + ~ IIe --+ r~p -+- .\ -tilt' the contact process that produces the compound

particle represented hy .\ isS03? 1 a neutron 3 an t'lt'dnlll

V20S(I) 25 + 30, I 2S03 2 a heta particle -l an alpha pur-tick- JJJ__

(2)5+0, V20S I SO;)

G~OVP 12-Laooratory Activities

v.o., ) 2503(3) 250, + 0, DIRECiIOr>;S (112-116): Record each ansuicr iu tile space provided.

v,o, ) 3S0 lIZ TIlt' process of filtration is performed in the labo­(4) 350, + 0, '- 3 106__ ratorv to 1 form precipitates

GJ\OUP ll-Nuclear Chemistry 2 remove water from solutions .") separate dissolved particles from the solvent

DIRECTIONS (107-111): Record each ansu'eT in the space prcroided. -4 separate insoluble substances in an aqueous

107 DUring which process would the ratio of mixture 11~

uranium-238 to lead-206 he used? IIJ Which graph shown below could represent the1 diagnosing thyroid disorders

uniform cooling of" substanee, starting with the2 dating geologic formanons gaseous phase and ending with the solid phase? 3 detecting brain tumors

4 treating cancer patients 107__

u , . e,108 The equation ¥H + I H --+ 2 He represents D. ,1\1 alpha decay :) fi.~sion

2 beta decay 4 fusion 108__ '" .... " Cf TIME (MIN) o TIME (MIN.)

109 Which substance m<l.Y he used as both tilt' coolant and moderator in a reactor? 1 boron 3 heavv wain 2 cadmium 4: solid· graphite 109__

P 0:

110 An isotope of which element may he used as a ur ".... fuel in a fission reaction?

( I 1 131

P D. ," ~

I1 hydrogen .") lithium o ....,U~o TIME (MIN.) ,' ....... {MIN.>2 carbon 4 plutonium 110__ 113__( 21 (4 J

EXAMINATION June1985 Chemistry 23

114 A student determined the melting point of a sub­stance to hf' S5.2DC. If the accepted value is 50, IDe, the percent error in her determination is (I) 5.10 (3) 10.2 Answers June 1985 Chemistry (;11 9.24 (4) 12.0 114__

ANSWER KEY

U5 Given the J;,J!owing titration data: PART ONE

"ohmw of base (KOHl := 40.0 ml I. 1 15. <I 29. -t 4:t Molaritv of base 0;:: 0.20 M Volume' of acid (Hel) added '= 20.0 ml

The conc-ntranon of Hel required for the acid to

2. 4 :1. 2: ,. 1 . ,a. z

re. I 17. 3 l8. Z 19. 3

3<). I 3J. I 32. -t 33. -t

44. 4.'}. 46. 1 47. ~

neutralize the base is s. 3 W.l 34. :] -tS. -I­

(1) 1.0 M \2\ 0.20 M

(3) 0.10 M (4) 0.40 M 115__

7. 1 S. , 9. 3

2J. 3 2.2.. I 23. 2

35. -t 36. <I 37. Z

49. J

50. 2 ;'H. ::;

10. 3 :24. 4 38. 3 52. ,1 11. 1 25. 4 39. 4 53. 1

116 Using the rules for significant figures, the sum of 12.. 2 26. 2 40. 3 .')4. I 0.027 gram and 0.002.'] gr:tm should be expressed as

13. oj

14. 3 27. 4 28. 2

41. 2 42. :]

5.'). 56.

1 2

(ll 0.029 gram (2\ 0,0293 gram

(3) 0.03 gram (4) 0.030 gram llB__ PART TWO

57. 1 72. 2 87. J W2. :?: 58. 3 73. I 88. ;: 103. :3 59. oj 74. 4 1;9. -l 104. 1 eo, 1 75. :] 90. 4 lOS. -t 61. 2 76. ;3 91. 1 106. :3 62. 3 77. I as. 1 107. 2 63. Z 78. -t 93. 2 108. -I­64. 4 79. 2 94' 109. .1 65. 2 SO. 1 95. 3 llO. -t ".1 sr. 4 96. I IJ I. 1 67. I 68 .,

82. 4 83. 3

97. 4 ss, 3

Il2. 113.

4 :2

ss. 4 84. 2 99. I 114. 3 70. J 85.3 100. :2­ 115. -t 71.4 86. I 101. 3 116. I

-24