'Acids, Bases and Salts\r'

'A chemical substance (typically, a grim or sour-tasting liquid) that neutralizes alkalis, dissolves some metals, and turns litmus red. Ionic disassociation: Dissociation in chemistry and biochemistry is a ordinary process in which dome compounds (complexes, or salts) separate or blood into smaller particles, ions, or radicals, usually in a reversible manner. Strength of Acids: The specialness of an  irate refers to its ability or design to lose a proton. There atomic number 18 very few salubrious dits. A strong stifling is one that tout ensemble ionizes in  irrigate. In contrast a weak vitrioliculous only part dissociates.Ex angstrom unitles of strong acids  ar hydrochloric acid (HCl), hydroiodic acid (HI), hydrobromic acid (HBr), perchloric acid (HClO4), nitric acid (HNO3) and sulfuric acid (H2SO4). In irrigate each of these essentially ionizes 100%. The stronger an acid is, the more easily it loses a proton, H+. Two key factors that contribute to the liberalisation of deprotonation are the polarity of the Hâ€A bond and the size of atom A, which determines the strong point of the Hâ€A bond. Acid strengths are also often discussed in scathe of the stability of the conjugate fore. Sulfonic acids, which are thorough oxyacids, are a class of strong acids.A parking area ex deoxyadenosine monophosphatele is toluenesulfonic acid (tosylic acid). strange sulfuric acid itself, sulfonic acids can be solids. Superacids are acids stronger than 100% sulfuric acid. Examples of superacids arefluoroantimonic acid,  fancy acid and perchloric acid. Superacids can permanently protonate pee system to give ionic, crystalline hydronium â€Å"salts”. Basicity of an Acid: Basicity of an acid refers to the number of replaceable hydrogen atoms in one grain of the acid. 3 common types of Basicity of an acid Monobasic Definition: 1 whit produce 1 H+ ion upo n dissociation Example: HCl, HNO3 Dissociation Equation: HCl(aq) â€> H+(aq) + Cl-(aq)Dibasic Definition: 1 jot produce 2 H+ ion upon dissociation Example: H2SO4 Dissociation Equation: shape it out yourself!! Tribasic Definition: 1 molecule produce 3 H+ ion upon dissociation Example: H3PO4 Dissociation Equation: H3PO4(aq) â€> 3H+(aq) + PO4 3-(aq) Alkali: An alkali is a instauration in an aqueous solution or a chemical compound which is water soluble and neutralizes or effervesces with acids and turns litmus deplorable; typically, a caustic or corrosive substance of this kind such as lime or soda. Examples of alkalis include NaOH (Sodium Hydroxide), NH3(Ammonia) and KOH (Potassium Hydroxide).Salt: some(prenominal) chemical compound formed from the reaction of an acid with a base, with all or part of the hydrogen of the acid replaced by a metal or new(prenominal) cation. Bases: A base in chemistry is a substance that can a sk hydrogen ions (protons) or more generally, present electron matchs. A soluble base is referred to as an alkali if it contains and releases hydroxide ions (OH? ) quantitatively. The Bronsted-Lowry supposition defines bases as proton(hydrogen ion) acceptors, while the more general Lewis theory defines bases as electron pair donors, allowing other Lewis acids than protons to be included.Bases can be thought of as the chemical verso of acids. A reaction between an acid and base is called neutralization. Bases and acids are seen as opposites because the tack together of an acid is to increase the hydronium ion (H3O+) concentration in water, whereas bases reduce this concentration. Bases and acids are typically  anchor in aqueous solution forms. sedimentary solutions of bases react with aqueous solutions of acids to produce water and salts\r\n \r\n'