CBSE Class 10th Definition in Terms of Furnishing of H+ and OH- ions Details & Preparations Downloads
In the vast world of chemistry, acids and bases play fundamental roles. One way to define and distinguish them is by their ability to furnish ions. Let's delve into the fascinating realm of H⁺ and OH⁻ ions and how they characterize these essential substances.
Unlocking Chemistry Excellence: CBSE NCERT Download for Definition in Terms of Furnishing of H⁺ and OH⁻ Ions
Acids: The Proton Donors: Acids are compounds that readily release H⁺ ions when dissolved in water. This process, known as ionization, is crucial in understanding the acidic nature of substances. Common examples of acids include citric acid found in citrus fruits and hydrochloric acid (HCl).
Explanation: Acids are defined as substances that increase the concentration of H⁺ ions in an aqueous solution. This characteristic gives acids their distinct sour taste and ability to react with metals.
Bases: The Hydroxide Providers: In contrast, bases are substances that furnish OH⁻ ions when dissolved in water. This release of hydroxide ions is integral to understanding the basic properties of these compounds. Sodium hydroxide (NaOH) and ammonia (NH₃) are classic examples of bases.
pH Scale: Measuring Acidity and Alkalinity: To quantify the acidity or alkalinity of a solution, scientists use the pH scale. Acids have a pH less than 7, with lower values indicating stronger acidity. Bases have a pH greater than 7, with higher values indicating stronger alkalinity. Water, with a pH of 7, is considered neutral.
Explanation: The pH scale provides a convenient way to express the concentration of H⁺ ions in a solution, helping us understand the relative strength of acids and bases.
Arrhenius Concept of Acids and Bases
- The Swedish scientist Svante August Arrhenius defined acids as substances that increase the H+ ion concentration of water when dissolved in it.
- These protons go on to form hydronium ions (H3O+) by combining with water molecules.
- Similarly, the Arrhenius definition of a base states that bases are the substances that, when dissolved in water, increase the concentration of OH– ions in it.
- One of the merits of this theory is that it successfully explains the reaction between acids and bases that yield salts and water.
- An important limitation of the Arrhenius definitions of acids and bases is that it fails to explain how substances lacking hydroxide ions form basic solutions when dissolved in water, such as NO2– and F–.
Bronsted Lowry Theory of Acids and Bases
- The Bronsted-Lowry theory defines an acid as a donor of protons.
- A base is defined as a proton acceptor (or H+ ion acceptor) by this theory.
- Bronsted acids undergo dissociation to yield protons and therefore increase the concentration of H+ ions in the solution.
- On the other hand, Bronsted bases accept protons from water (the solvent) to yield hydroxide ions.
- An advantage of the Bronsted-Lowry definition of acids and bases is its ability to explain the acidic or basic nature of ionic species.
- An important limitation of this theory is that it fails to explain how compounds lacking hydrogen exhibit acidic properties, such as BF3 and AlCl3.
Conjugate Acids and Bases
- According to Bronsted-Lowry concept, an acid is a substance that can donate H+ and base is a substance that can accept H+.
- The acid and base which differ by proton , are said to form conjugate acid and base pair.
- A conjugate acid is formed when a proton is added to a base, and a conjugate base is formed when a proton is removed from an acid.
Lewis Concept of Acids and Bases
- The Lewis definition of an acid states that it is a species that has a vacant orbital and therefore, has the ability to accept an electron pair.
- A Lewis base is a species that holds a lone pair of electrons and can, therefore, act as an electron-pair donor.
- This theory does not involve the hydrogen atom in its definition of acids and bases.
- Lewis acids are electrophilic in nature whereas Lewis Bases possess nucleophilic qualities.
- Examples of Lewis acids: Cu2+, BF3, and Fe3+. Examples of Lewis bases: F–, NH3, and C2H4 (ethylene).
- A Lewis acid accepts an electron pair from a Lewis base, forming a coordinate covalent bond in the process. The resulting compound is referred to as a Lewis adduct.
- A notable advantage of this concept is that many compounds can be defined as acids or bases by it. However, it offers little insight into the strength of these acids and bases.
- One of the disadvantages of this theory is that it fails to explain the acid-base reactions that do not involve the formation of a coordinate covalent bond.
Uses of Acids and Bases
The various uses of acids and bases are listed in this subsection.
1. Uses of Acids
- Vinegar, a diluted solution for various household applications. It is primarily used as a food preservative.
- Citric acid is an integral part of lemon juice and orange juice. It can also be used in the preservation of food.
- Sulphuric acid acid is widely used in batteries. The batteries used to start the engines of automobiles commonly contain this acid.
- The industrial production of explosives, dyes, paints, and fertilizers involves the use of sulphuric acid acid and nitric acid.
- Phosphoric acid is a key ingredient in many soft drinks.
2. Uses of Bases
- The manufacturing of soap and paper involves the use of sodium hydroxide. NaOH is also used in the manufacture of rayon.
- Ca(OH)2, also known as slaked lime or, is used to manufacture bleaching powder.
- Dry mixes used in painting or decoration are made with the help of calcium hydroxide.
- Magnesium hydroxide, or milk of magnesia, is commonly used as a laxative. It also reduces any excess acidity in the human stomach and is, therefore, used as an antacid.
- Ammonium hydroxide is a very important reagent used in laboratories.
- Any excess acidity in soils can be neutralized by employing slaked lime.
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SAMPLE PRACTICE QUESTION
Q:1 What fundamental characteristic defines acids in the context of ion furnishing?
Ans: Acids are characterized by their capacity to release hydrogen ions (H⁺) when dissolved in water, a process known as ionization.
Q:2 Provide an example of a widely encountered acid and elucidate how it furnishes H⁺ ions.
Ans: Hydrochloric acid (HCl) serves as a common acid. Upon dissolution in water, it ionizes to liberate H⁺ ions, thereby increasing their concentration in the solution.
Q:3 How are bases defined concerning the furnishing of ions?
Ans: Bases are defined by their ability to release hydroxide ions (OH⁻) when dissolved in water, contributing to their alkaline nature.
Q:4 Offer an illustration of a base and elucidate how it furnishes OH⁻ ions.
Ans: Sodium hydroxide (NaOH) is an example of a base. In an aqueous solution, it dissociates to release OH⁻ ions, elevating the concentration of hydroxide ions in the solution.
Q:5 What role does the pH scale play in our comprehension of acids and bases?
Ans: The pH scale serves as a quantitative measure of the acidity or alkalinity of a solution. Acids register a pH below 7, while bases exhibit a pH above 7.
CBSE CLASS 10 Mathematics Chapters |
Chapter1: Real Numbers |
Chapter2: Polynomials |
Chapter3: Pair of Linear Equations in Two Variables |
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Chapter5: Arithmetic Progressions |
Chapter6: Triangles |
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Chapter11: Areas Related to Circles |
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Chapter2: Acids, Bases and Salts |
>General Properties |
>Examples and Uses |
>Concept of pH Scale |
>Properties and Uses of Sodium Hydroxide |
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Chapter4: Carbon and its Compounds |
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