Question

Explain why CO2, SO2 and NH3,CaO cannot be explained by Arrhenius concept

Answer 1

Answer:

The acids like HNO3, HCl, etc. gives one proton on dissociation, called monoprotic acids. The acids like H2SO4, H3PO4, etc. which having more than one hydrogen atoms and gives more than 1 H+ ions on dissociation, called polyprotic acids. It is not necessary that polyprotic acids are stronger than monoprotic acids.

Similarly, Arrhenius bases are compounds that increase the concentration of OH− or hydroxide ion in aqueous solution or having at least one OH− ion in formula. The common examples of Arrhenius base includes NaOH (sodium hydroxide), KOH (potassium hydroxide), Ca(OH)2 (calcium hydroxide), Mg(OH)2 (magnesium hydroxide), NH4OH (ammonium hydroxide)

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Answer 2

Answer:

According to Arrhenius Concept:--

Bases are those substances which dissociate in water and give hydroxyl ions (OH⁻). For example Na OH, KOH, Ca(OH)₂ etc.

NaOH $\longrightarrow$   Na⁺ (aq)  +   OH⁻ (aq)

NH₄OH ⇄  NH₄⁺(aq)   +   OH⁻ (aq)

Ca(OH)₂  ⇄ Ca²⁺ (aq)   +    2OH⁻ (aq)

Acids are those substances which dissociate in water to give hydrogen ions (H⁺). For example: HCl, HNO, CHCOOH etc.

HCl    $\longrightarrow$    H⁺ (aq)   + Cl⁻ (aq)

HNO₃    $\longrightarrow$    H⁺ (aq)   + NO₃ (aq)

So, according to Arrhenius, a acid must contain hydrogen and a base must contain hydroxyl group.

CO₂, SO₂, NH₃ and CaO have basic nature but they do not contain any hydroxyl group. Therefore according to Arrhenius concept, they are not bases.

Therefore, CO₂, SO₂, NH₃ and CaO  cannot be explained by Arrhenius concept of Acids and bases.

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