Question

Give four example of acids and base and there differences also​

Answer 1

AND THIS UR ANSWER

PLZ MARK AS BRAINLIEST

Answer 2

$\underline{\textbf{QUESTION :-}}$

Differences ,similarities of acids and bases

$\underline{\textbf{ANSWER :-}}$

Difference in Definition

Acid

An acid is a molecule or substance that has a pH value less than 7.0 when it is present in an aqueous solution. An aqueous solution is any solution where water is a solvent. Acids are termed as compounds that donate H+ (hydrogen ion) to another compound known as base.

Base

A base (alkaline) is a molecule or substance that has a pH value higher than 7.0 when present in an aqueous solution. Bases are the exact chemical opposite of acids. In chemistry. They are substances that, in aqueous solution, release hydroxide (OH−) ions.

Difference in Classification

Acids are classified as:

• Strong acids, such as nitric acid (HNO₃), sulfuric acid (H₂SO₄), and hydrochloric acid (HCl) respectively.

• Strong Lewis acids, such as AlCl₃ (anhydrous aluminium chloride) and BF₃ (boron trifluoride).

• Concentrated weak acids, such as acetic acid (CH₃COOH) and formic acid (CH₂O₂).

• Lewis acids with specific reactivity, for example; solutions of ZnCl₂ (zinc chloride).

• Superacids, which are extremely strong acids.

Bases are classified as:

• Alkalis or Caustics, such as NaOH (sodium hydroxide) and KOH (potassium hydroxide).

• Concentrated weak bases, such as NH₃ (ammonia) in a concentrated solution.

• Alkali metals in metallic form, (i.e. elemental sodium), and hydrides of alkaline and alkali earth metals, i.e. NaH (sodium hydride), which function as a strong hydrate and bases to produce caustics.

• Superbases, which are extremely strong bases, such as metal amides, alkoxides, (i.e. NaNH₂ – sodium amide) and C₄H₉Li (butyllithium), which is an organometallic base.

Difference in Chemical Formula

Acids

The chemical formula for most acids starts with H. For example, Nitric acid (HNO₃), Carbonic acid in soft drink (H₂CO₃), Boric acid (H₃BO₃), Hydrochloric acid (HCl), Oxalic Acid (H₂C₂O₄), Citric Acid or 2-Hydroxy-1,2,3-propanetricarboxylic acid (H₃C₆H₅O₇), and Sulfuric acid (H₂SO₄). However, there are exceptions like Acetic Acid (CH₃COOH).

Bases

The chemical formula for most bases (compounds) has OH at the end. For example, Calcium hydroxide or slaked lime, Ca (OH)₂ (paper, flocculant), Magnesium hydroxide (Mg (OH)₂) or milk of magnesia, Sodium hydroxide (NaOH) or caustic soda (cleaning agent, pH regulator), Ammonium hydroxide (NH₄OH) or ammonia water and KOH (Potassium hydroxide).

Difference in pH

Acids

Acids have a pH less than 7.0.

Bases

Bases have a pH higher than 7.0, and could even go up to 14 if the bases are very strong.

The following are the similarities between the two:

• Most strong acids and bases are both corrosive in nature. They tend to corrode or rust metals.

• Both, acids and bases change the colour of litmus paper. An acid changes the colour of a blue litmus paper to red and a base changes the colour of red litmus paper to blue.

• Strong acids can damage the skin causing severe burns if it gets into contact with the skin. But did you know, even strong bases can do the same?

• A lot of common things that are used in day-to-day basis are acids and bases. For e.g. Citric fruits such as lemon, orange, grapefruit, etc contain citric acid and tamarind, grapes, etc contain tartaric acid, olive oil contains oleic acid and vinegar contains acetic acid. Many soaps, toothpaste, etc have bases in them. Baking soda is also basic in nature.

• Both are classified on the basis of strength, concentration and their respective basicity and acidity. Acids are also classified on the basis of source and the presence of oxygen.

• Acids and bases both react with water and a lot of acids and bases are soluble in nature.

• Both acids and bases are electrolytes which means that they’re good conductors of electricity.

• Acids and bases both produce ions in water solution. Acids release hydrogen ions (H+) whereas Bases release hydroxide ions (OH–).

• The process of mixing acid or a base in water is an exothermic one that releases some amount of heat.

Examples

Acids-

• Sulfuric acid
• Nitric acid

• Hydrochloric acid

• Phosphoric acid

Acids-

• Potassium hydroxide (KOH)
• Sodium hydroxide (NaOH)
• Barium hydroxide (Ba(OH)₂)
• Caesium hydroxide (CsOH)
• Strontium hydroxide (Sr(OH)₂)