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Chapter 7: Problem 54

Consider the following reactions (i) \(\mathrm{CO}_{3}^{2-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{HCO}_{3}^{-}+\mathrm{OH}^{-}\) (ii) \(\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}\) (iii) \(\mathrm{NH}_{3}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{NH}_{4} \mathrm{OH}\) (iv) \(\mathrm{HCl}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{Cl}^{-}\) Which pair of reactions proves that water is amphoteric? (1) \(i\) and ii (2) ii and iii (3) iii and iv (4) i and iii

Short Answer

Expert verified
Option (3) iii and iv show water's amphoteric nature.

Step by step solution

01

Understand Amphoteric Substances

Amphoteric substances can act as both acids and bases. Water (H2O) is one such substance.
02

Analyze Reaction (i)

In reaction (i) \(\mathrm{CO}_{3}^{2-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{HCO}_{3}^{-}+\mathrm{OH}^{-}\), water donates a proton (acts as an acid according to Bronsted-Lowry theory).
03

Analyze Reaction (ii)

In reaction (ii) \(\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}\), water combines with CO2 to form carbonic acid (acts as a base).
04

Analyze Reaction (iii)

In reaction (iii) \(\mathrm{NH}_{3}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{NH}_{4} \mathrm{OH}\), water donates a proton to ammonia, forming ammonium hydroxide (acts as an acid).
05

Analyze Reaction (iv)

In reaction (iv) \(\mathrm{HCl}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{Cl}^{-}\), water acts as a base by accepting a proton from hydrochloric acid.
06

Identify the Pair of Reactions

From the above steps, water acts as both an acid and a base in reactions (i) and (iv). This demonstrates water's amphoteric nature clearly.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

acid-base reactions
Acid-base reactions are fundamental in chemistry. They occur when an acid donates a proton \( \text{H}^+ \) to a base. To understand these reactions better, consider common substances. For instance, when hydrochloric acid \( \text{HCl} \) reacts with water \( \text{H}_2\text{O} \), it forms hydronium ions \( \text{H}_3\text{O}^+ \) and chloride ions \( \text{Cl}^- \). This is a classic example of an acid-base reaction.
Bronsted-Lowry theory
The Bronsted-Lowry theory provides a framework for acid-base reactions. According to this theory, an acid is a proton donor and a base is a proton acceptor. This model helps us understand the behavior of substances in different reactions. For example, in the reaction \( \text{NH}_3 + \text{H}_2\text{O} \rightleftharpoons \text{NH}_4^+ + \text{OH}^- \), ammonia \( \text{NH}_3 \) acts as a base by accepting a proton from water. Water, in this case, acts as an acid by donating a proton.
amphoteric substances
Amphoteric substances can act as both acids and bases. Water is a prime example. Depending on the reaction, water can donate or accept a proton. In one reaction, water \( \text{H}_2\text{O} \) donates a proton to the carbonate ion \( \text{CO}_3^{2-} \), acting as an acid. In another reaction, water accepts a proton from hydrochloric acid \(\text{HCl} \), acting as a base. This dual behavior is what makes water amphoteric. Identifying these reactions helps in understanding the versatile nature of such substances.
water chemistry
Water chemistry is fascinating due to the unique properties of water. It is essential for life and exhibits a variety of chemical behaviors. Water can participate in acid-base reactions, as seen in the reactions with \( \text{CO}_2 \) and \( \text{NH}_3 \). Its amphoteric nature allows it to act as both an acid and a base. This makes water a versatile solvent, capable of dissolving many substances. Understanding water chemistry involves exploring its molecular structure, hydrogen bonding, and its role in facilitating chemical reactions.

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Most popular questions from this chapter

Which of the following statements is false? (l) According to Lewis theory electrophiles are Lewis acids while nucleophiles are Lewis bases. (2) In Friedel-Crafts reaction, the catalysts used are Lewis acids. (3) In complex compounds, metal ions are Lewis bases while ligands are Lewis acids. (4) Electron-deficient molecules are Lewis acids.

\(\Lambda\) saturated solution of \(\mathrm{II}_{2} \mathrm{~S}\) in \(0.1 \mathrm{M} \mathrm{IICl}\) at \(25^{\circ} \mathrm{C}\) contains a \(\mathrm{S}^{2-}\) ion concentration of \(10^{-23} \mathrm{~mol} \mathrm{~L}^{-1}\). The solubility products of some sulphidcs are: \(\mathrm{CuS}=10^{-44}\), \(\mathrm{FeS}=10^{-14} ; \mathrm{MnS}=10^{-15}\) and \(\mathrm{CdS}=10^{-25} .\) If \(0.01 \mathrm{M}\) solutions of these salts in \(1 \mathrm{M}\) IICl are saturated with \(\mathrm{H}_{2} \mathrm{~S}\), which of these will be precipitated? (1) All (2) All except MnS (3) All except MnS and FeS (4) Only CuS

The \(\mathrm{pH}\) of the solution containing \(10 \mathrm{~mL}\) of \(0.1 \mathrm{~N}\) \(\mathrm{NaOH}\) and \(10 \mathrm{ml}\) of \(0.05 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) would be (1) zero (2) 1 (3) \(>7\) (4) 7

When equal volumes of the following solutions are mixed, precipitation of \(\mathrm{AgCl}\left(K_{\mathrm{pp}}=1.8 \times 10^{10}\right)\) will occur only with (1) \(10^{-4} \mathrm{M}\left(\mathrm{Ag}^{-}\right)\) and \(10^{-4} \mathrm{M}\left(\mathrm{Cl}^{-}\right)\) (2) \(10^{-5} \mathrm{M}\left(\Lambda \mathrm{g}^{-}\right)\) and \(10^{-5} \mathrm{M}\left(\mathrm{Cl}^{-}\right)\) (3) \(10^{-6} \mathrm{M}\left(\Lambda \mathrm{g}^{-}\right)\) and \(10^{-6} \mathrm{M}\left(\mathrm{Cl}^{-}\right)\) (4) \(10^{-10} \mathrm{M}\left(\Lambda \mathrm{g}^{-}\right)\) and \(10^{-10} \mathrm{M}\left(\mathrm{Cl}^{-}\right)\)

Which onc of the following is not a postulate of Ostwald's theory of indicators? (1) The colour of an indicator in solution is duc to the ions furnished by it (2) The colour of an indicator is duc to the ions furnished by acidic substancc (3) \Lambdall indicators are weak acids or bases (4) \Lambdacidic indicators show decp colour in acidic solutions and vice versa
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