Calculate the pH change that results when 11 mL of 5.1 M NaOH is added to 796 mL of each the following solutions. (See the Acid-Base Table.) (a) pure water (b) 0.10 M NH4Cl (c) 0.10 M NH3 (d) a solution that is 0.10 M in each NH4+ and NH3
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.
Calculate the pH change that results when 11 mL of 5.1 M NaOH is added to 796 mL of each the following solutions. (See the Acid-Base Table.)
(b) 0.10 M NH4Cl
(c) 0.10 M NH3
(d) a solution that is 0.10 M in each NH4+ and NH3
![Acid Name
perchloric acid
hydrohalic acid
sulfuric acid
nitric acid
hydronium ion
iodic acid
oxalic acid
sulfurous acid
hydrogen sulfate ion
phosphoric acid
hydrofluoric acid
nitrous acid
lactic acid
formic acid
hydrogen oxalate ion
hydrazoic acid
acetic acid
carbonic acid
hydrogen sulfite ion
hydrosulfuric acid
dihydrogen
phosphate ion
hypochlorous acid
ammonium ion
hydrocyanic acid
hydrogen
carbonate ion
Conjugate Acid
HC1O4
HX (X = I, Br, Cl)
H₂SO4
HNO3
ammonia
hydroxide ion
H₂O¹+
HIO3
H₂C2O4
H₂SO3
HSO
H3PO4
HF
HNO2
HC3H5O3
HCHO2
HC₂0¹1-
HN3
HC2H3O2
H₂CO3
HSO¹-
H₂S
H₂PO¹1-
HCIO
NH1+
HCN
HCO3-
hydrogen phosphate ion HPO2-
HS¹-
hydrogen sulfide ion
water
H₂O
NH3
OH¹-
Ka
>> 1
>> 1
>> 1
>> 1
1.0
0.17
5.9 × 10-2
1.5 × 10-2
1.2 x 10-2
7.5 x 10-3
7.2 x 10-4
4.0 x 10-
-4
6.4 x 10-5
1.8 x 10-4
6.4 x 10-5
1.9 × 10-5
1.8 x 10-5
4.3 x 10-7
1.0 x 10-7
1.0 x 10-7
6.2 x 10-8
3.5 x 10-8
5.6 × 10-10
4.0 × 10-10
4.7 x 10-11
4.8 x 10-13
1.3 x 10-13
1.0 × 10-14
<< 10-14
<< 10-14
pKa
<0
<0
<0
<0
0.00
0.77
1.23
1.82
1.92
2.12
3.14
3.40
3.85
3.74
4.19
4.72
4.74
6.37
7.00
7.00
7.21
Conjugate Base
CIO¹-
X¹-
HSO4-
NO¹-
H₂O
103-
HC₂0¹1-
HSO3-
SO²-
H₂PO¹1-
Fl-
NO¹
C3H5O3-
CHO
C₂0²-
N²-
C₂H30¹2-
HCO3-
SO²-
HS¹-
HPO²-
CIO ¹-
NH3
CN¹-
7.46
9.25
9.40
10.33 CO
12.32 PO³-
12.89
S²-
14.00 OH¹-
NH₂-
0²-
Base Name
perchlorate ion
halide ion
hydrogen sulfate ion
nitrate ion
water
iodate ion
hydrogen oxalate ion
hydrogen sulfite
ion
sulfate ion
dihydrogen
phosphate ion
fluoride ion
nitrite ion
lactate ion
formate ion
oxalate ion
azide ion
acetate ion
hydrogen
carbonate ion
sulfite ion
hydrogen sulfide ion
hydrogen
phosphate ion
hypochlorite ion
ammonia
cyanide ion
carbonate ion
phosphate ion
sulfide ion
hydroxide ion
amide ion
oxide ion](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4c3310c5-cf1b-4860-895e-b0d1f5af2b55%2F21571996-8d7c-4655-a782-fca7ad8dfc7b%2Figrijq_processed.png&w=3840&q=75)
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