5. Identify each Bronsted acid and base in the following equations. Note that the reactions are assumed to be reversible. a. HC,Oi(aq) + H2O(l) = HO*(aq) + C,O,(aq) b. PO4³(aq) + H₂O(1) HPO42 (aq) + OH(aq) c. F (aq) + H₂O(1) HF (aq) + OH(aq)
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.
![5. Identify each Bronsted acid and base in the following equations. Note that the reactions are
assumed to be reversible.
a. HC₂O4 (aq) + H₂O(1) H3O*(aq) + C₂04² (aq)
b. PO4³ (aq) + H₂O(1) HPO42 (aq) + OH(aq)
c. F (aq) + H₂O(1) HF (aq) + OH(aq)
6. Calculate the molar concentration of OH in water solutions with the following H3O* molar
concentrations.
a. 1.0x10-6
b. 4.8x104
C. 1.4
7. Calculate the molar concentration of H3O* in water solutions with the following OH molar
concentrations.
a.
1.0x10-5
b. 8.3x10⁹
c. 0.072
8. Determine the pH of water solutions with the following characteristics. Classify each solution as
acidic, basic, or neutral.
a. [H+] = 6.2x10-5
b.
[H+] = 8.4x108
c. [H] = 2.2x10-10
d. [OH] = 4.9x10²
e. [OH-] = 6.2x107
9. Convert the following pH values into both [H+] and [OH-] values:
a. pH = 3.95
b. pH = 4.00
c. pH = 11.86](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6d8383fc-abfb-4f3a-b394-eb91005b1f56%2Fa9b6a6e6-c057-44d6-b8ff-b4bb2e261782%2Fppd8j1h_processed.png&w=3840&q=75)
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