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.
![Q1:Chose the correct answer from the following
1- the [H] concentration for the solution that result from addition of 40.0 ml of 0.10 M KOH to 50
ml of 0.3 M of HCI.
a) 0.0667 M. b) 1.00 x 10
-7
c) 0.12 M
d) 1.50 x 10-13 M
2-What is the pH of 500 mL of solution containing 0.0124 grams of Ca(OH)₂?
c) 2.96
d) 3.17
a) 11.04 b) 9.68
e) 10.83
M
3- What was the pH of the solution that result from addition of 30 ml of 0.1 M hydrochloric acid to
25.0 ml of 0.5 M solution of weak base (Kb=9.74×106 ).?
a. 5.10
c. 8.49
4- A 0.10 M solution of a weak acid, HX, is 0.059% ionized. Evaluate K, for the acid.
a) 3.8 x 10
b) 6.5 x 10-7
c) 7.0 x 10-6
d) 4.2 x 10-6
e) 3.5 x 10-8
b. 4.92
a-
e) none of the above
d. 9.08
5- How many grams of sodium acetate will adde to sufficient amount of 0.1 M solution of acetic acid
to makin 100 ml of buffer solution with pH= 4.1
(Mw of sodium acetate is 82 g/mole and
Ka acetic acid is 1.75×10)
2.27 g
b- 0.34 g
c- 0.180 g
d- 4.76 g
6- If 15.00 ml of 0.1M NaOH solution is needed to reach the end point of 10 ml HNO3. Then the
concentration of HNO3 in ppm is: [M.wt. of HNO,= 63 g/mol]
c) 7.30 × 10³ ppm
d) 18.77 × 10³ ppm
b) 14.70 x10³ ppm
a) 9.45×10³
ppm
a) 3.64
7. Which of the following is true about a 0.10 M solution of a weak acid, HX?
a) [X] = 0.10 M
b) pH = 1
c) [HX] > [H]
d) [H] = 0.10 M
8-. What is the pH of 0.060 M NH4CI? (NH3 Kb = 3.98 x10-¹0)
b) 5.12
a) 5.06
c) 5.18
d) 5.24
c) 4.58
e. 8.72
e) 5.35
9- Calculate the pH that results when the following solutions are mixed.( Ka of formic acid is 3 x10¹)
(1) 35 mL of 0.20 M formic acid
(2) 55 mL of 0.10 M sodium formate
(3) 110 mL of water
b) 3.11
d) 3.39
10-What is the pH of a buffer solution where [HA] = [A-]?
a. pH = 1
b. pH = pOH
c. pH = Ka
e) both b and d
e) 4.20
d. pH = 7.0
e. pH = pk a](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F46ef3182-b77b-4d5e-aa39-bd37ce4fcd02%2Fbe2272a3-91ad-4407-8c19-c7022180de7f%2Ffp3codq_processed.jpeg&w=3840&q=75)
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