Difference of acid and base detail 2 3 pages science in
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✨Acids ✨
- acids are those chemical substances which have sour taste.
- acids change the colour of blue litmus to red.
- the acids present in plant materials and animals are called organic acids.eg : formic acid , oxalic acid etc.
- the acid prepared from the minerals of the earth are called mineral acids.
⏩properties of acids
- acids acids have a sour taste
- acids turn blue litmus to red
- acid solution conduct electricity
- acid react with metal to form hydrogen gas.
- acid react with bases to form salt and water
✨Bases ✨
- bases are those chemical substances which have a bitter taste.
- a best is a chemical substance which can neutralize an acid.
⏩properties of bases
- bases and bitter taste.
- bases feel soapy to touch.
- bases turn red litmus to blue.
- bases conduct electricity in solution.
- bases react with some metal to form hydrogen gas.
- bases react with acid to form salt and water.
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water solution ionizes and becomes hydrogen ions and chloride ions. If that is the case, a base, or alkali, is a material that can donate a hydroxide ion (OH-). Sodium hydroxide in water solution becomes sodium ions and hydroxide ions. By the definition of both Thomas Lowry (England) and J.N. Br¯nsted (Denmark) working independently in 1923, an acid is a material that donates a proton and a base is a material that can accept a proton. Was Arrhenius erroneous? $| 8-) No. The Arrhenius definition serves well for a limited use. We are going to use the Arrhenius definitions most of the time. The Lowry- Br¯nsted definition is broader, including some ideas that might not initially seem to be acid and base types of interaction. Every ion dissociation that involves a hydrogen or hydroxide ion could be considered an acid- base reaction. Just as with the Arrhenius definition, all the familiar materials we call acids are also acids in the Lowry - Br¯nsted model. The G.N. Lewis (1923) idea of acids and bases is broader than the Lowry - Br¯nsted model. The Lewis definitions are: Acids are electron pair acceptors and bases are electron pair donors.
We can consider the same idea in the Lowry - Br¯nsted fashion. Each ionizable pair has a proton donor and a proton acceptor. Acids are paired with bases. One can accept a proton and the other can donate a proton. Each acid has a proton available (an ionizable hydrogen) and another part, called the conjugate base. (That word, 'conjugate' just means that it "goes with" the other part.) When the acid ionizes, the hydrogen ion is the acid and the rest of the original acid is the conjugate base. Nitric acid, HNO 3, dissociates (splits) into a hydrogen ion and a nitrate ion. The hydrogen almost immediately joins to a water molecule to make a hydronium ion. The nitrate ion is the conjugate base of the hydrogen ion. In the second part of the reaction, water is a base (because it can accept a proton) and the hydronium ion is its conjugate acid.
HNO3 + H2O ===> (NO3)- + (H3O)+
ACID BASE CONJUGATE
BASE CONJUGATE
ACID
Chemists or chemistry texts often use the hydrogen ion, H+ to show a hydrogen ion released into water solution. In a way, there is no such thing as a hydrogen ion or proton without anything else. The majority of hydrogen atoms are only a single proton and a single electron. If you remove the electron to make it an ion, the only thing that is left is a proton. Protons just don't exist naked like that in water solution. Remember that water is a very polar material. There is a strong partial negative charge on the side of the oxygen atom and a strong partial positive charge on the hydrogen side. Any loose hydrogen ion, having a positive charge, would quickly find itself near the oxygen of a water molecule. At close range from the charge attraction, the hydrogen ion would find a pair (its choice of two pairs) of unshared electrons around the oxygen that would be capable of filling the its outer shell. Each hydrogen ion unites with a water molecule to produce a hydronium ion, (H3O)+, the real species that acts as acid. The hydroxide ion in solution does not combine with a water molecule in any similar fashion. As we write reactions of acids and bases, it is usually most convenient to ignore the hydronium ion in favor of writing just a hydrogen ion, H+.
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