One of the examples of such reaction is when Lithium reacts with NH3 to form Lithium Amide. There are only a few (7) strong acids, so many people choose to memorize them. As others have pointed out, you have a nomenclature problem and a chemistry problem. Grocery stores sell vinegar, which is a 1 M solution of acetic acid: CH 3 CO 2 H. Although both substances are acids, you wouldn't use muriatic acid in salad dressing, and vinegar is ineffective in cleaning bricks or concrete. Both are “ammonia” and very weak acids ([math]pK_a=30[/math]). The only weak acid formed by the reaction between hydrogen and a halogen is hydrofluoric acid (HF). There is no difference between [math]NH_3[/math] and [math]H_3N[/math]. Because it is not listed in Table 11.2 "Strong Acids and Bases", we can assume that it is a weak … There are only a few strong acids in water, they are: HBr, HCl, HI, HNO3, HClO4 and H2SO4 (for the first H only) All other acids are weak acids. Classify these compounds by whether they behave as strong acids, weak acids, strong bases, or weak bases in aqueous solution. The strong acids are hydrochloric acid, nitric acid, sulfuric acid, hydrobromic acid, hydroiodic acid, perchloric acid, and chloric acid. It may be 1% ionized or 99% ionized, but it is still classified as a weak acid. Therefore, the numerical value of K a is a reflection of the strength of the acid. HCl is a strong acid, not a weak acid, so the combination of these two solutes would not make a buffer solution. All the other acids are weak. Strong electrolyte (strong base) Carbonic acid. As explained earlier, NH3 is a weak base and reacts with acids to form salts. Although NH3 is a weak base, it also acts as a weak acid under certain conditions and reacts with bases. Many hardware stores sell "muriatic acid" a 6 M solution of hydrochloric acid HCl(aq) to clean bricks and concrete. Ammonia is actually considered to be a weak base due to it's inability to completely ionise in solution (consequently, it has a relatively low pH>7). HBr H2S Weak acid Strong base LiOH RbOH Na3PO4 Weak base HN3 (CH3)3N NH4CI Chemists use the term "strong" or "weak" with regard to acids and bases to tell how much the substance dissociates in water. Strong and Weak Acids and Bases . Weak acids with relatively higher K a values are stronger than acids with relatively lower K a values. As it turns out, there are very few strong acids, which are given in Table \(\PageIndex{1}\). Strong electrolyte (strong acid) C12H22O11 (sugar) Non-electrolyte (molecular compound and not an acid … It usually reacts as sodium-azide, if there is HN3 present, there is probbably another acid added, which protonates O in epoxide, making it possible for N3- … Strong acid ???. Weak electrolyte (weak acid) CH3COO. Strong electrolyte (soluble) NO3-Strong electrolyte (soluble) Hydroiodic acid. CH 3 NH 2 is methylamine, which is like NH 3 with one of its H atoms substituted with a CH 3 group. Ummm it is a weak acid, but N3- is a good nucleophile. Any acid that dissociates 100% into ions is called a strong acid. It can lose H+ ion and form Amides (NH2-). The acid ionization represents the fraction of the original acid that has been ionized in solution. Weak electrolyte (weak acid) Acetic acid. If an acid is not listed here, it is a weak acid. If it does not dissociate 100%, it is a weak acid.