1. In each of the equations below, label the acids, bases and their conjugates. HCOOH + H2O ↔ HCOO- + H3O+ HPO42- + H2O ↔ H2PO4- + OH- NH3 + H2O ↔ OH- + NH4+
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. In each of the equations below, label the acids, bases and their conjugates.
| HCOOH | + | H2O | ↔ | HCOO- | + | H3O+ |
| HPO42- | + | H2O | ↔ | H2PO4- | + | OH- |
| NH3 | + | H2O | ↔ | OH- | + | NH4+ |
2.
Decide which of the following statements are True and which are False about equilibrium systems:
A large value of K means the equilibrium position lies far to the left.
For a reaction with K >> 1, the rate of the forward reaction is greater than the rate of the reverse reaction at equilibrium.
For the following reaction: H2(g) + F2(g) ⇌ 2HF(g) the values of K and Kp are the same.
For the following reaction: CaCO3(s) ⇌ CaO(s) + CO2(g) the [CaCO3] appears in the denominator of the equilibrium expression.
The value of K at constant temperature does not depend on the amounts of reactants and products that are mixed together initially.
3.
Given the following equilibrium constants at 427°C:
| O2(g) + 4Na(l) 2Na2O(s) | K1 = 2.50×1049 |
| O2(g) + 2Na(l) 2NaO(g) | K2 = 2.50×109 |
| O2(g) + 2Na(l) Na2O2(s) | K3 = 2.00×1028 |
| O2(g) + Na(l) NaO2(s) | K4 = 3.33×1013 |
What would be the value of the equilibrium constant for each of the following reactions, at 427°C?
| Na2O2(s) + O2(g) 2NaO2(s) |
| Incorrect. | Tries 1/99 | Previous Tries |
| 4NaO2(s) 2Na2O(s) + 3O2(g) |
4. Given:
| Si(s) + 2H2(g) SiH4(g) | K = 7.76×106 |
| C(graphite) + SiH4(g) CH4(g) + Si(s) | K = 1.02×102 |
What is the equilibrium constant for the following reaction?
| C(graphite) + 2H2(g) CH4(g) |
5.
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