Lab Equipment Overview. beakers Erlenmeyer flask Graduated cylinders Test tube.
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As part of a demonstration, the teacher uses a hot plate to heat three liquids in beakers to boiling. Liquid A is water, Liquid B is ethanol, and Liquid C is an aqueous copper(II) sulfate solution. The students observe the boiling liquids and note that, in each beaker, bubbles form on the bottom and side surfaces of the beaker and then rise to the liquid’s surface.
Liquid A Liquid CLiquid B
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QualityCore® Reference SheetChemistry
Atomic Structure
E = hν
c = λν
Gases
d =
T (K) = °C + 273
P total = PA + PB + PC + …
PV = nRT
n =
d =
P1V1 = P2V2
=
=
=
Percent Yield and Percent Error
% Yield = × 100
% Error = × 100⏐accepted value − experimental value⏐_________________________________accepted value
actual yield_______________theoretical yield
P2V2_____T2
P1V1_____T1
P2___T2
P1___T1
V2___T2
V1___T1
PM____RT
m__M
m__V
E = energyh = Planck’s constant = 6.63 × 10−34 J•sν = frequencyc = speed of light = 3.0 × 108 m/sλ = wavelengthNA = Avogadro’s number = 6.02 × 1023 mol−1
d = density (solids, liquids, and gases)m = massV = volumeT = temperatureP = pressuren = number of molesR = gas constant = 0.0821 L•atm/mol•KM = molar massSTP = 1.00 atm and 0.00°C1 atm = 760 mm Hg = 760 torr = 101.3 kPa1 mol of ideal gas = 22.4 L at STP
continued
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Liquids and Solutions
Percent (mass/mass) = × 100
M =
m =
XA =
M1V1 = M2V2
ΔT f = K f × m
ΔTb = Kb × m
Calorimetry and Thermodynamics
q = mCΔT
ΔH°rxn = ΔH°f (products) − ΔH°f (reactants)
ΔS°rxn = S°(products) − S°(reactants)
Acids, Bases, and Equilibrium
pH = − log [H+]
pOH = − log [OH−]
pH + pOH = 14
Kw = [H+][OH−]
Keq = where a A + b B c C + d D
Ksp = [A+]a[B−]b where AaBb(s ) a A+(aq ) + b B−(aq )
[C]c[D]d_________[A]a[B]b
molesA_________molestotal
moles of solute_____________kg of solvent
moles of solute_____________L of solution
mass of solute (g)__________________mass of solution (g)
M = molaritym = molalityXA = mole fraction of component AV = volumeΔT = temperature changeK f = molal freezing point depression constantK f (H2O) = 1.86°C/mKb = molal boiling point elevation constantKb (H2O) = 0.512°C/m
q = heatm = massC = specific heat capacityC (H2O) = 4.184 J/g•°CΔT = temperature changeΔH° = standard enthalpy changeΔS° = standard entropy change
[H+] = H+ molarity[OH−] = OH− molarityKw = ion-product constant for waterKw = 1.0 × 10−14 at 25°CKeq = equilibrium constantKsp = solubility product constant
© 2010 by ACT, Inc. All rights reserved.14193 *019248080* Rev 2
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1H
1.0083Li
6.94111Na
22.9919K
39.1037Rb
85.4755Cs
132.987Fr
(223)
4Be
9.01212Mg
24.3120Ca
40.0838Sr
87.6256Ba
137.388Ra
226.0
21Sc
44.9639Y
88.9157La*
138.989
Ac†
(227)
22Ti
47.8840Zr
91.2272Hf
178.5104Rf
(261)
23V
50.9441Nb
92.9173Ta
180.9105Db
(262)
24Cr
52.0042Mo
95.9474W
183.9106Sg
(263)
25Mn
54.9443Tc
(98)75Re
186.2107Bh
(264)
26Fe
55.8544Ru
101.176Os
190.2108Hs
(265)
27Co
58.9345Rh
102.977Ir
192.2109Mt
(268)
28Ni
58.6946Pd
106.478Pt
195.1110Ds
(281)
29Cu
63.5547Ag
107.979Au
197.0
30Zn
65.3848Cd
112.480Hg
200.6
5B
10.8113Al
26.9831Ga
69.7249In
114.881Tl
204.4
6C
12.0114Si
28.0932Ge
72.5950Sn
118.782Pb
207.2
7N
14.0115P
30.9733As
74.9251Sb
121.883Bi
209.0
8O
16.0016S
32.0734Se
78.9652Te
127.684Po
(209)
9F
19.0017Cl
35.4535Br
79.9053I
126.985At
(210)
2He
4.00310Ne
20.1818Ar
39.9536Kr
83.8054Xe
131.386Rn
(222)
58Ce
140.190Th
232.0
59Pr
140.991Pa
(231)
60Nd
144.292U
238.0
61Pm
(145)93Np
(237)
62Sm
150.494Pu
(244)
63Eu
152.095Am
(243)
64Gd
157.396Cm
(247)
65Tb
158.997Bk
(247)
66Dy
162.598Cf
(251)
67Ho
164.999Es
(252)
68Er
167.3100Fm
(257)
69Tm
168.9101Md
(258)
70Yb
173.0102No
(259)
71Lu
175.0103Lr
(260)
*
†
Periodic Table of the Elements
*019249080* Rev 1
© 2010 by ACT, Inc. All rights reserved.14192
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Answer Key
1) B2) B3) C4) A5) B6) D7) A8) C9) B
10) D11) A12) C13) C14) C15) C16) C17) D18) B19) A20) C21) C22) D23) B24) C25) B26) C27) C28) B29) D30) A31) A32) B33) D34) A35) C36) D37) C
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38) A39) D40) C41) B42) D43) B44) C45) C46) D47) A48) C49) A50) D51) C52) B53) D54) D55) A56) D57) D58) C59) A60) A61) A62) D63) B64) D65) B66) C67) C68) A69) B70) B71) B72) D73) B74) C
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75) C76) D77) C78) A79) D80) A81) B82) A83) B84) A85) C86) D87) B88) C89) A90) D91) B92) A93) A94) B95) D96) D97) A98) B99) C
100) B101) B102) D103) B104) B105) C106) C107) D108) D109) C110) D111) B
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112) A113) C114) A115) A116) D117) A118) A119) B120) C121) C122) A123) D124) C125) D126) A127) C128) D129) B130) A131) A132) A133) B134) D135) A136) C137) A138) A139) B140) B141) A142) A143) A144) C145) C146) B147) C148) A
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149) D150) A151) C152) D153) B154) C155) B156) A157) B158) B159) B160) A161) B162) A163) A164) C165) C166) A167) A168) D169) B170) B171) D172) D173) D174) D175) C176) C177) A178) D179) A180) A181) D182) D183) C184) B185) B
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186) D187) D188) C189) B190) B191) B192) B193) A194) A195) D196) A197) D198) A199) B200) D201) C202) C203) A204) A205) B206) B207) B208) D209) C210) C211) D212) D213) A214) C215) B216) D217) B218) B219) D220) B221) D222) D
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223) B224) B225) C226) C227) D228) C229) C230) A231) B232) B233) A234) D235) D236) C237) A238) D239) A240) C