- Calculate either [H3O+] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 1.97 × 10-7 M; [H₂0+] = Solution B: [H3O+] = 9.13 × 10−⁹ M; [OH¯] = Solution C: [H3O+] = 5.77 × 10−4 M; [OH¯] = Which of these solutions are basic at 25 °C? Solution A: [OH-] = 1.97 × 10-¹ M Solution C: [H₂O+] = 5.77 × 10-4 M Solution B: [H3O+] = 9.13 × 10-⁹ M M M M
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.
please help with these 2
![Calculate either [H₂O+] or [OH-] for each of the solutions at 25 °C.
Solution A: [OH-] = 1.97 × 10-7 M; [H₂0†] =
Solution B: [H₂O+] = 9.13 × 10−⁹ M; [OH¯] =
Solution C: [H₂O+] = 5.77 × 10−4 M; [OH¯] =
Which of these solutions are basic at 25 °C?
Solution A: [OH-] = 1.97 × 10-7 M
Solution C: [H3O+] = 5.77 × 10-4 M
Solution B: [H₂O+] = 9.13 × 10-⁹ M
M
M
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff57d3743-5e44-4060-83da-5d90a37d31c6%2F8fe20da1-8d06-4692-a869-16ec3da953cb%2Fmyj7cta_processed.png&w=3840&q=75)
![Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral.
[H+] =
Acidic
= 9.4 × 10-⁹
[H+] = 9.3 × 10-5
pOH = 13.74
[H+] = 1.0 × 10-7
pOH = 1.54
[OH-] = 4.6 × 10-3
Basic
Answer Bank
[OH-] = 1.2 × 10-¹0
pH = 13.90
pOH = 7.00
Neutral
pH = 3.49](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff57d3743-5e44-4060-83da-5d90a37d31c6%2F8fe20da1-8d06-4692-a869-16ec3da953cb%2F4cldd8k_processed.png&w=3840&q=75)
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