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ACIDS

Theju Shree K

U11GT21S0351

I B.Sc., (P/C), II SEM

GFGC COLLEGE, TUMKUR

Deepika7676792371@gmail.com                              Phone no: 7676792371

An acid is any substance that gives the H+ ions as a product or an acid is any substance that in water solution tastes sour, changes blue litmus to red litmus and it reacts with some metals to liberate hydrogen.

  • It reacts with bass to form Salts.

E.g. 1) HCL ----> H+ + Cl-

  • PH is less than ‘7’ they are called ‘acidic’. So we called acids.
  • Strong Acid:

The substances which ionizes completely called strong acids.

Eg: HBr, HI, ESOL, HNO3.

  • Weak Acid:

The substances which ionises partially called weak acids. Eg. HCOOH, CH3COOH, C6H5COOH

Some Examples:

Vinegar                                                           ---->                 Acetic acid

Decomposition of Butter                                ---->                 Butyric Acid              

Citrus  Fruits (Lemon, Orange)                      ---->                 Citric Acid

Milk Digestion                                                ---->                 Lactic acid

Apple                                                              ---->                 Malic acid

Uses of Acids:

  • Carbonic acid (HOCO,) is present in the acerated  cool drinks we drink.
  • Sulphuric acid ESOL) is used in Car batteries.
  • Sulphuric acid (H2SO,) is also used to manufacture points, dyes, synthetic fibres.
  • Nitric acids (HNO3) is used in manufacturing of fertilizers.

Applications of Acids:

  1. Lewis Acid - base Theory:

Any substance such as H+ ion, that can accept a pair of non-bonding electrons.

  1. Arrhenius theory:

Acids are the compound that increases the concentration of H+ or proton in aqueous solution.

  1. Lowry Bronsted theory:
  • Acid is a substance which donates an H+ ion or a proton and forms its conjugate base.
  • Aqueous solutions of acids are electrolytes, meaning that they conduct electrical current. Some acids are strong electrolytes because they ionize completely in water, yielding a great many ions. Other acids are weak electrolytes that exist primarily in a non-ionized form when dissolved in water.
  • Acids have a sour taste. Lemons, Vinegar and sour candies all contain acids.
  • Acids change the color of certain acid -base indicates. Two common indicators are litmus and phenolphthalein. Blue litmus turns red in the presence of an acid, while phenolphthalein turns colorless.
  • Acids react with active metals to yield hydrogen gas. Recall that an activity series is a list of metals in descending order ot reactivity. Metals that are above hydrogen in the activity series will replace the hydrogen from an acid in a single - replacement reaction, as show below :

Zn(s) + H2SO4 (aq)> ZnSO4(aq) + H2 (g)

  • Acids react with bases to produce a salt compound and water. When equal moles of an acid and a base are combined, the acid is neutralized by the base. The Products of this reaction are an ionic compound, which is labeled as a salt and water.

Bronsted-Lowry Acid:

Bronsted-Lowry acid is a potential source of protons. For example, HCl is Bronsted-Lowry acid as it has the ability to donate protein. When Bronsted-Lowry acid contributes to the proton, a base is formed, and this base is called the conjugate base. For example, the conjugate base of the HCl molecule is ion chloride.

Bronsted-Lowry Base:

The Bronsted-Lowry base is a proton-absorbing material. For example, NH3 is a Bronsted-Lowry base as it has the ability to receive protons. When the Bronsted-Lowry base adopts a proton, an acid is formed, and this acid is called conjugate acid. For example, the conjugate acid molecule of NH3 is a cation of ammonium

Bronsted-Lowry Acid-Base Reaction:

The Brønsted-Lowry acid-base reaction involves the transfer of protons from the acid to the base. In this process, after donating a proton, the first acid becomes the basis of the conjugate, and after receiving the proton, the first base becomes conjugate acid. Thus, any Bronsted-Lowry acid-base reaction combines two acids with two bases, forming a pair of conjugate acid-base.

Key Points of the Bronsted Lowry Theory:

  • Bronsted-Lowry acid is a type of chemical that can provide proton or hydrogen cation.
  • The Bronsted-Lowry base is a type of chemical that is able to absorb protons. In other words, it is a type with a single pair of electrons available to be synthesised on H +.
  • After Bronsted-Lowry acid donates protein, it forms its own conjugate base. Conjugate acid-base of Bronsted-Lowry forms when it receives a proton. A pair of conjugate acid-base has a molecular formula similar to the original pair of acid-base, except that the acid has one more H + compared to the conjugate base.
  • Solid acids and bases are defined as compounds that add ionise completely to water or an aqueous solution. Acids and weak bases are slightly separated.
  • According to this theory, water is amphoteric and can serve as a base for Bronsted-Lowry acid and base.

When asked to indicate whether a chemical reaction includes solid acids or bases or weak ones, it helps to look at the arrow between reactants and products. The solid acid or base separates completely from its ions, leaving no ions uncoated after the reaction has been eliminated. The arrow usually points from left to right.

On the other hand, weak acids and bases do not completely separate, so the reaction arrow points both left and right. This reflects the dynamic balance that is established when a weak acid or base and its fragmented form both remain in solution.

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