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Densities of Common Materials
NAME SYMBOL DENSITY (g/cm
3
Science Department CHEM 1411-1412 Laboratory 2
Positive Ions (Cations)
Aluminum Al
3+
Ammonium NH 4
Barium Ba
2+
Calcium Ca
2+
Chromium Cr
3+
Cobalt(II) Co
2+
Copper(II), cupric Cu
2+
Copper(I), cuprous Cu
Hydrogen H
Hydronium H 3 O
Iron(III), ferric Fe
3+
Iron(II), ferrous Fe
2+
Lithium Li
Lead(II), plumbous Pb
2+
Magnesium Mg
2+
Mercury(II), mercuric Hg
2+
Mercury(I), mercuous Hg 2
2+
Nickel(II) Ni
2+
Potassium K
Silver Ag
Sodium Na
Strontium Sr
2+
Tin(II), stannous Sn
2+
Zinc Zn
2+
Negative Ions (Anions)
Science Department CHEM 1411-1412 Laboratory 92
Constants
Avogadro’s Number NA 6.022 x 10
23 /mole
Gas constant R 0.08205 L atm mol
-
K
-
8.314 J mol
-
K
-
Speed of light in a vacuum c 2.998 x 10
8 m/s
Planck’s Constant h 6.63 x 10
J•s
e = 2.7183 = 3.
STP: 0 ºC ; 1 atm ; 22.414 L/mol
For water at 25 ºC :
d = 1.00 g/mL P
0
= 23.8 torr
Kb = 0.512 C mol/kg Kf = 1.86 C mol/kg
Kw = 1.00 x 10
CP = 4.184 J/g C CP (ice) = 2.1 J/g C CP (steam) = 2.0 J/g C
Hfus = 333 J/g Hvap = 2260 J/g
Science Department CHEM 1411-1412 Laboratory 93
Equations
d = m/V M = mol/L m = mol/kg
rectangular solid A = l w V = l w h
circle A = r
2
V = r
2
h (cylinder)
sphere A = 4 r
2
V = r
3
F = C + 32 C = (F - 32) K = C + 273
q = m CP T E = q + w E = Efinal - Einitial
c = E = h E = h c/ E = m c
2
En = - J rn = n
2
a 0 H = E
P V = n R T P V =
PTOT = p 1 + p 2 + p 3 + ··· p 1 = 1 PTOT 1 = n 1 / nTOT
Tf = i Kf m Tb = i Kb m
Rate = - = - k [ A ]
x
k = A e
-Ea/RT
[A]t = [A] 0 e
ln [A]t = ln [A] 0 - k t t½ = (ln 2)/ k (
st
order)
K =
pH = -log [H 3 O
] pOH = -log[OH
] pH + pOH = 14
pH = pKa + log ([A
Science Department CHEM 1411-1412 Laboratory 94
Descriptive Solubility Terms
Term Grams solute/100 g solvent Aqueous Solution Example
Very soluble more than 100 Ethanol
Freely soluble 10 - 100 NaCl
Soluble 3 - 10
Sparingly soluble 1 - 3 Ag 2 SO 4
Slightly soluble 0.1 - 1
Very slightly insoluble 0.01 - 0.
Insoluble less than 0.01 AgCl
Solubility Rules for Ionic Compounds in Aqueous Solutions
Soluble
- All common acids are soluble.
(HCl, HNO
3
, H
2
SO
4
, H
3
PO
4
, CH
3
COOH)
- All alkali metal (Li
, Na
, K
, Rb
,
Cs
) and NH 4
salts are soluble.
- All NO 3
1- are soluble; all CH 3
COO
1-
are slightly soluble.
- All Cl
1- , Br
1- , I
1- , and SCN
1- are
soluble, except those of Pb
2+ , Ag
, and Hg 2
2+ .
(PbCl 2
is soluble in hot water.)
- All SO 4
2- are soluble, except those of
Ba
2+ , Sr
2+ , and Pb
2+ .
(CaSO 4
, Ag 2
SO 4
, and HgSO 4
are
slightly soluble)
- All NO 2
1- , ClO 4
1- , ClO 3
1- , MnO 4
1- ,
and Cr 2
O 7
2- are soluble.
Insoluble
(Note that the alkali metal and ammonium salts are always
exceptions - Rule 2 Soluble Salts)
- All OH
1- and O
2- are insoluble.
(Except Ca
2+
, Sr
2+
, and Ba
2+
)
- All F
1- , S
2- , CO 3
2- , PO 4
2- , SO 3
2- , BO 3
3- ,
AsO 4
3- , AsO 3
3- , and SiO 3
2- are insoluble.
- All CrO 4
2- are insoluble.
(Except Mg
2+ , Ca
2+ , Sr
2+ , and Cu
2+ )
- All C 2
O 4
2-
are insoluble.
(Except Fe
3+
)
(MgC 2
O 4
is slightly soluble.)
Science Department CHEM 1411-1412 Laboratory 95
Activity Series and Electrochemical Potentials of Metals
Metal Reduction Reaction E
0
(volts)
Lithium Li
Li (s) - 3.
Potassium K
K (s) - 2.
Barium Ba
Ba (s) - 2.
Calcium Ca
Ca (s) - 2.
Sodium Na
Na (s) - 2.
Magnesium Mg
Mg (s) - 2.
Aluminum Al
Al (s) - 1.
Zinc Zn
Zn (s) - 0.
Iron Fe
Fe (s) - 0.
Cobalt Co
Co (s) - 0.
Nickel Ni
Ni (s) - 0.
Tin Sn
Sn (s) - 0.
Lead Pb
Pb (s) - 0.
Hydrogen 2 H
+ 2 e
H
(g) 0.
Copper Cu
Cu (s) 0.
Silver Ag
Ag (s) 0.
Platinum Pt
Pt (s) 1.
Gold Au
Au (s) 1.
Ease of oxidation increases
