2. For each of the following salts, determine the pH of a 2.50M solution of the salt. You will need the Ka and Kb tables to complete this problem. a. NaBro b. CH3NH3CI c. NaCIO2 d. C6H5OK
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![2. For each of the following salts, determine the pH
of a 2.50M solution of the salt. You will need the Ka
and Kb tables to complete this problem.
a. NaBro b. CH3NH3CI c. NaClO2 d. C6H5OK
e. CSNO3 f. C6H5NH3B
Martin S. Silberberg. Chemiatry: The Molecular Nature of Matter and Change, 2nd Edition. Copyright The McGraw-Hill Companies, Inc. All righto resorvod.
Kb Values for Molecular Bases
Table 18.6 KbValues for Some Molecular (Amine) Bases at 25°C
Name (Formula)
Lewis Structure*
HHH H H
Diethylamine [(CH,CH,),NH]
H-C
-C-C-H
8.6x104
H H
H H H
Dimethylamine [(CH,),NH]
H-C-N-C-H
5.9x10
H.
H H
H-C-C-H
Triethylamine [(CH,CH,),N]
5.2x104
H-C
H H
H-c-c-H
Methylamine (CH, NH,)
H-C-N-H
4.4x104
Ethanolamine (HOCH,CH,NH,)
H-ö-c-C-N-H
3.2x10-5
Ammonia (NH,)
H-N-H
1.76x105
Pyridine (C,H5N)
1.7x10-9
Aniline (C,H,NH2)
-N-H
4.0x10-10
* Blue type indicates the basic nitrogen and its lone pair.
Martin S. Sberberg. Chamietry: The Molacular Nature of Matter and Change, 2 Edbon. Copyrighte The MeGraw-HI Companies, Ire. Al righte recervad.
Ka Values
for Some
Monoprotic
Acids
Table 18.2 Ka Values for Some Monoprotic Acids at 25°C
Name (Formula)
lodic acid (HIO3)
Lewis Structure*
Ka
H-ö-i-ö
1.6x10-1
Chlorous acid (HCIO,)
Nitrous acid (HNO,)
Hydrofluoric acid (HF)
H-ö-N-Ö
H-:
1.12x10-2
7.1x104
6.8x10
Formic acid (HCOOH)
H-C-ö-H
1.8x10
Benzoic acid (C, H,COOH) O--ö-n
6.3x10-5
Acetic acid (CH,COOH)
H-c-C-0-H
1.8x105
H
HH 1O
Propanoic acid
(CH,CH,COOH)
H-c-c-c-ö-H 1.3x10¬5
H H
Hypochlorous acid (HCIO) H-ö-i:
Hypobromous acid (HBRO) H-ö-re
Hydrocyanic acid (HCN)
2.9x108
2.3x109
6.2x10-10
H-C=N
Phenol (C,H;OH)
1.0x10-10
2.3x10-11
Hypoiodous acid (HIO)
H-0-
"Red type indicates the ionizable proton; structures have zero formal charge.
H2SO4 Ka1 = Sstrong Ka2 = 1.2 x 10-2
H2C2O4 Ka1 = 6.0 x 102
Ka2 = 6.1 x 10-5
H2SO3
Ka1 = 1.6 x 102
Ka2 = 6.4 x 10-8
H3PO4
Ka1 = 7.5 x 10-3
Ka2 = 6.2 x 10-8 Ka3 = 4.2 x 10-13
H3C6HSO, Ka1=7.4 x 10-4 Ka2= 1.7 x 105
Ka3 = 4.0 x10-7
Citric acid
H2C6H6O6 Ka1= 8.0 x 10-5 Ka2 = 1.6 x 10-12
Ascorbic acid
ACID STRENGTH
BASE STRENGTH](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F57638993-6d33-4396-984b-2e3f32f46fd1%2F6fd88845-a28f-4401-826c-50380a850683%2Fdpkp1p7_processed.jpeg&w=3840&q=75)
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