Is nh4cl an acid or a base?
A salt formed from reaction of a weak base and a strong acid should give an acidic solution. For example, NH4Cl is formed from the reaction of NH3, a weak base, and HCl, a strong acid. The chloride ion will not hydrolyze. Fluoride is the conjugate base of HF and produces hydroxide ions in solution.
NH4+ has a pKa of 9.25 while NH3 has a pKb of 4.75. Thus, NH4+ is weakly acidic while NH3 is quite a strong base in comparison. But, NH4+ isn't the weakest acid and NH3 isn't the strongest base in absolute terms (which mean 100% protonation or depronotation in solution, if we use Lowry-Bronsted theory).
- Acetic acid (CH3COOH) is a carboxylic acid (RCOOH), and the majority of the carboxylic acids are weak acids, including acetic acid. This means that these acids dissociate partially into RCOO- anions and H+ cations in a given aqueous solution.
- A: H2PO4- is called dihydrogen phosphate ion. It is the conjugate base of Phosphoric Acid H3PO4 and the conjugate acid of monohydrogen phosphate ion HPO42-.
- precedence over the other ions. For example, (NH4)2S is soluble and a strong electrolyte. Strong Electrolytes: Essentially all ionic compounds and the strong acids. (Example: BaCO3) Weak Electrolytes: Molecular compounds that partially dissociate, which are primarily weak acids and bases.
In contrast to the acid definition, a Bronsted-Lowry base is a substance that accepts protons. An example of a proton acceptor is ammonia (NH3). The ammonia is happy to accept a proton from the hydrogen of water (H2O) to become NH4. NH3 + H2O = NH4+ + OH-.
- A compound that is amphoteric has both acid and base properties. Ammonium Carbonate certainly has both, NH4(1+) (ammonium) is acidic and CO3(2+) is a base. So, as a unit, it is amphoteric. But, when you put it in solution, (NH4)2CO3 comes apart and, by itself, NH4+ is not amphoteric and CO3(2-) is not, either.
- Since NaOH is a strong base, its conjugate acid is a weak acid. The anionic part is carbonate ion, which is the conjugate base of H2CO3 ( carbonic acid) which is a very very weak acid. Hence CO3 2- or the carbonate ion is a strong base.
- acid, H2CO3, and the weak base is bicarbonate, HCO3-. Because the hydrogen ion attaches and is not free in solution, the pH will not change dramatically. The weak acid that forms will not dissociate into hydrogen ions to any great extent.
Both ammonia is a weak base and ammonium ion is a weak acid. Many, even most, acid/base conjugate pairs are like that. A weaker acid has a stronger conjugate base, not necessarily a totally strong one.
- Both ammonia is a weak base and ammonium ion is a weak acid. Many, even most, acid/base conjugate pairs are like that.
- At room temperature, ammonia is a colorless, highly irritating gas with a pungent, suffocating odor. In pure form, it is known as anhydrous ammonia and is hygroscopic (readily absorbs moisture). Ammonia has alkaline properties and is corrosive.
- Ammonia (NH3), colourless, pungent gas composed of nitrogen and hydrogen. It is the simplest stable compound of these elements and serves as a starting material for the production of many commercially important nitrogen compounds.
Updated: 3rd December 2019