1. Calculate the pH of a solution in which the [H*] is: a. 1.5 M Also classify each solution as either acidic, basic or neutral. b. 2.6 x 104 c. 9.3 x 107
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.
![1. Calculate the pH of a solution in which the [H*] is:
b. 2.6 x 104
Also classify each solution as either acidic, basic or neutral.
а. 1.5 М
c. 9.3 x 10-7
2. Calculate the [H*] in a solution which has a pH of:
С. 7.97
а. 4.62
b. 9.41
3. Calculate the [OH"] in a solution which has a pH of:
b. 1.00
а. 3.19
C. 9.87
4. In a certain solution the equilibrium concentration of acetic acid is 0.3 M and acetate
is 0.5 M. What is the pH of the solution? Ka of acetic acid
1.8 x 10-5
%3D
6. How many moles of sodium acetate should be added to 375 ml of 0.3M acetic acid in
order to prepare a buffer with pH
= 4.50? Assume no volume change.
7. A buffer is prepared by adding 45 ml of 0.15 M NaF to 35 ml of 0.1 M HF. What is the
pH of the final solution? Ka of HF = 6.8 x 104.
8. Find the pH of a solution that is 0.50 M in formic acid and 0.40 M in sodium formate.
Find the pH after 0.050 mol of HCI has been added to 1.0 liter of the solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2b72c308-3814-44d5-9b2b-3970a767798f%2Fdacd417a-565d-4034-b6cc-7006c99d1771%2Fllxjvcr_processed.jpeg&w=3840&q=75)
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