write a short note on organic acid, inorganic acid and base with their example
Answers
Answer:
organic acids are those acid which we can obtained from plants and animals.
example : lactic acid, vinegar, formic acid.
in organic acid are those acid which we can obtained from our chemical reaction.
example such as hydrochloric acid sulphuric acid.
Answer:
Explanation:
An organic acid is an organic compound with acidic properties. The most common organic acids are the carboxylic acids, whose acidity is associated with their carboxyl group –COOH. Sulfonic acids, containing the group –SO2OH, are relatively stronger acids. Alcohols, with –OH, can act as acids but they are usually very weak. The relative stability of the conjugate base of the acid determines its acidity. Other groups can also confer acidity, usually weakly: the thiol group –SH, the enol group, and the phenol group. In biological systems, organic compounds containing these groups are generally referred to as organic acids.
A few common examples include:
Lactic acid
Acetic acid
Formic acid
Citric acid
Oxalic acid
Uric acid
Malic Acid
sour.
2. a substance that yields hydrogen ions in solution and from which hydrogen may be displaced by a metal to form a salt. For the various acids, see under the specific name, such as acetic acid. All acids react with bases to form salts and water (neutralization). Other properties of acids include a sour taste and the ability to cause certain dyes to undergo a color change. A common example of this is the ability of acids to change litmus paper from blue to red.
Inorganic acids are distinguished as binary or hydracids, and ternary or oxyacids; the former contain no oxygen; in the latter, the hydrogen is united to an electronegative element by oxygen. The hydracids are distinguished by the prefix hydro-. The names of acids end in -ic, except in the case in which there are two degrees of oxygenation. The acid containing the greater amount of oxygen has the termination -ic, the one having the lesser amount has the termination -ous. Acids with the termination -ic form the salts ending in -ate; those ending in -ous form the salts ending in -ite. The salts of hydracids end in -ide. These rules are demonstrated by the acids and salts: hydrochloric acid (HCl), sodium chloride (NaCl), sulfuric acid (H2SO4), sodium sulfate (Na2SO4), sulfurous acid (H2SO3), sodium sulfite (Na2SO3). Acids are called monobasic, dibasic, tribasic, and tetrabasic, respectively, when they contain one, two, three, or four replaceable hydrogen atoms
In chemistry, bases are substances that, in aqueous solution, release hydroxide (OH−) ions, are slippery to the touch, can taste bitter if an alkali,[1] change the color of indicators (e.g., turn red litmus paper blue), react with acids to form salts, promote certain chemical reactions (base catalysis), accept protons from any proton donor or contain completely or partially displaceable OH− ions. Examples of bases are the hydroxides of the alkali metals and the alkaline earth metals (NaOH, Ca(OH)2, etc.—see alkali hydroxide and alkaline earth hydroxide).
In water, by altering the autoionization equilibrium, bases yield solutions in which the hydrogen ion activity is lower than it is in pure water, i.e., the water has a pH higher than 7.0 at standard conditions. A soluble base is called an alkali if it contains and releases OH− ions quantitatively. However, it is important to realize that basicity is not the same as alkalinity. Metal oxides, hydroxides, and especially alkoxides are basic, and conjugate bases of weak acids are weak bases.
Bases can be thought of as the chemical opposite of acids. However, some strong acids are able to act as bases.[2] Bases and acids are seen as opposites because the effect of an acid is to increase the hydronium (H3O+) concentration in water, whereas bases reduce this concentration. A reaction between an acid and a base is called neutralization. In a neutralization reaction, an aqueous solution of a base reacts with an aqueous solution of an acid to produce a solution of water and salt in which the salt separates into its component ions. If the aqueous solution is saturated with a given salt solute, any additional such salt precipitates out of the solution.