Table of Contents
What is the Ka of ammonium?
| Ka | Acid | |
|---|---|---|
| 6.2 * 10-8 | Hydrogen sulfite ion | HS- |
| 2.9 * 10-8 | Hypochlorous acid | HClO |
| 6.2 * 10-10 | Hydrocyanic acid | HCN |
| 5.8 * 10-10 | Ammonium ion | NH4 + |
How much does ammonia dissociate?
You are told that your ammonia solution has a degree of dissociation of 1.3% at a given temperature T . What that means is that for every 100 molecules of ammonia present in solution, only 1.3 will dissociate.
What is the base ionization constant expression for ammonia?
Strong and Weak Bases and Base Ionization Constant, Kb
| Name of Base | Ionization Equation | Kb |
|---|---|---|
| Ammonia | NH3+H2O⇌NH+4+OH− | 1.8×10−5 |
| Pyridine | C5H5N+H2O⇌C5H5NH++OH− | 1.7×10−9 |
| Acetate ion | CH3COO−+H2O⇌CH3COOH+OH− | 5.6×10−10 |
| Fluoride ion | F−+H2O⇌HF+OH− | 1.4×10−11 |
Is ammonia a weak base?
Ammonia is a weak base, which means it only partially ionizes in water.
How much ammonia can dissolve in water?
The solubility of ammonia gas in water is about 90 g per 100 mL at 0 °C and about 32 g per 100 mL at 25 °C. The room temperature solubility corresponds to a volume of 460 L ammonia gas dissolving in 1 L of water. The term “ammonium hydroxide” raises consternation among many chemists.
What are KA and KB values?
The acid dissociation constant (Ka) is a quantitative measure of the strength of an acid in solution while the base dissociation constant (Kb) is a measure of basicity—the base’s general strength. Acids are classified as either strong or weak, based on their ionization in water.
What is base dissociation constant?
Kb, the base dissociation constant or base ionisation constant, is an equilibrium constant that refers to the dissociation, or ionisation, of a base. For the reaction in which the Arrhenius base, BOH, dissociates to form the ions OH- and B+: BOH OH- + B+ Kb = [OH-][B+]
Why ammonia is a strongest base?
The ammonia reacts as a base because of the active lone pair on the nitrogen. Nitrogen is more electronegative than hydrogen and so attracts the bonding electrons in the ammonia molecule towards itself. That means that in addition to the lone pair, there is a build-up of negative charge around the nitrogen atom.