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Chapter 7: Problem 77

Which of the following statements is falsc? (1) Hydrolysis of the salt of strong acid and weak base is called cationic hydrolysis (2) Hydrolysis of the salt of weak acid and strong base is known as anionic hydrolysis (3) Aqueous solution of aluminium chloride is acidic due to hydrolysis of \(\mathrm{Al}^{3}\) ion (4) Aqueous solution of sodium carbonate is basic due to hydrolysis of \(\mathrm{Na}\) ion

Short Answer

Expert verified
Statement 4 is false because sodium ion does not hydrolyze.

Step by step solution

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01

- Analyze Statement 1

Hydrolysis of the salt of a strong acid and a weak base is known as cationic hydrolysis. Since the cation of the weak base hydrolyzes, this statement is correct.
02

- Analyze Statement 2

Hydrolysis of the salt of a weak acid and a strong base is called anionic hydrolysis. Since the anion of the weak acid hydrolyzes, this statement is correct.
03

- Analyze Statement 3

Aqueous solution of aluminium chloride is acidic due to hydrolysis of \(\text{Al}^{3+}\) ion. The \(\text{Al}^{3+}\) ion reacts with water to form \(\text{Al(OH)}^{2+}\) and \(\text{H}^{+}\) ions, making the solution acidic. This statement is correct.
04

- Analyze Statement 4

Aqueous solution of sodium carbonate is basic due to hydrolysis of \(\text{Na}\) ion. This is incorrect because sodium ion (Na\(\text{Na}^{+}\)) from sodium carbonate does not hydrolyze; instead, the carbonate ion (CO_3^{2-}) hydrolyzes to form hydroxide ion (OH^{-}), making the solution basic.

Key Concepts

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

cationic hydrolysis
In cationic hydrolysis, a salt formed from a strong acid and a weak base reacts with water. The cation, which originates from the weak base, hydrolyzes.
For example, consider ammonium chloride (NH4Cl). When it dissolves in water, it forms NH4+ and Cl- ions. The NH4+ ion undergoes cationic hydrolysis by reacting with water to form NH4OH and H+ ions.
This process makes the solution acidic because of the presence of H+ ions.
  • The general reaction for cationic hydrolysis can be written as:
    \text{BH\(^{+}\) + H\( _{2} \)O ↔ B + H\(_{3} \)O\(^{+}\)}
anionic hydrolysis
Anionic hydrolysis happens when the salt of a weak acid and a strong base dissolves in water. Here, the anion from the weak acid is the one that hydrolyzes.
For instance, take sodium acetate (CH3COONa). When it dissolves in water, it forms CH3COO- and Na+ ions. The CH3COO- ion undergoes anionic hydrolysis by reacting with water to form CH3COOH and OH- ions.
This process makes the solution basic due to the presence of OH- ions.
  • The general reaction for anionic hydrolysis is:
    \text{A- + H\( _{2} \)O ↔ HA + OH\(^{-}\)}
acidic solutions
An acidic solution has an excess of hydrogen ions (H+).
When salts undergo cationic hydrolysis, they often produce acidic solutions.
For example, aluminium chloride (AlCl3) in water forms Al3+ and Cl- ions. The Al3+ ion reacts with water to form Al(OH)2+ and H+ ions, increasing the H+ concentration in the solution.
This hydrolysis reaction can be written as:
\text{Al\( ^{3+} \) + 3H\(_{2}\)O ↔ Al(OH)\(_{3}\) + 3H}\(^{+}\)
  • In general, solutions with high H+ concentration are acidic.
basic solutions
A basic solution has an excess of hydroxide ions (OH-).
When salts undergo anionic hydrolysis, they often produce basic solutions.
For example, sodium carbonate (Na2CO3) in water forms Na+ and CO3^2- ions. The CO3^2- ion reacts with water to form HCO3- and OH- ions, increasing the OH- concentration in the solution.
This hydrolysis reaction can be written as:
\text{CO\(_{3}^{2-}\) + H\(_{2}\)O ↔ HCO\(_{3}^{-}\) + OH}\(^{-}\)
  • In general, solutions with high OH- concentration are basic.

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Most popular questions from this chapter

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 \(10^{-10} \mathrm{M}\left(\mathrm{Cl}^{-}\right)\)

For the reaction \(2 \mathrm{X}(\mathrm{g})+\mathrm{Y}(\mathrm{g}) \rightleftharpoons 2 \mathrm{Z}(\mathrm{g}) ; \Delta H=\) 80 kcal. The highest yicld of \(Z\) at cquilibrium occurs at (1) \(1000 \mathrm{~atm}\) and \(500^{\circ} \mathrm{C}\) (2) \(500 \mathrm{~atm}\) and \(500^{\circ} \mathrm{C}\) (3) \(1000 \mathrm{~atm}\) and \(100^{\circ} \mathrm{C}\) (4) \(500 \mathrm{~atm}\) and \(100^{\circ} \mathrm{C}\)

The \(\mathrm{pH}\) of a \(1 \times 10^{8} \mathrm{M}\) aqueous solution of \(\mathrm{HCl}\) is slightly less than 7 because(1) the ionization of \(\mathrm{HCl}\) is incomplete (2) the ionization of water is negligible (3) the ionization of water at such a low concentration of \(\mathrm{HCl}\) is significant (4) the ionization of both \(\mathrm{HCl}\) and water are negligible

To \(100 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{AgNO}_{3}\) solution, solid \(\mathrm{K}_{2} \mathrm{SO}_{4}\) is added. The concentration of \(\mathrm{K}_{2} \mathrm{SO}_{4}\) that shows the precipitation is \(\left(K_{s p}\right.\) for \(\left.\mathrm{A}_{\mathrm{g}_{2}} \mathrm{SO}_{4}=6.4 \times 10^{-5} \mathrm{M}\right)\) (1) \(0.1 \mathrm{M}\) (2) \(6.4 \times 10^{-3} \mathrm{M}\) (3) \(6.4 \times 10^{-7} \mathrm{M}\) (4) \(6.4 \times 10^{-5} \mathrm{M}\)

\(\Lambda \mathrm{B}_{2}\) dissociates as \(\Lambda \mathrm{B}_{2}(\mathrm{~g}) \rightleftharpoons \Lambda \mathrm{B}(\mathrm{g})+\mathrm{B}(\mathrm{g})\). When the initial pressure of \(\Lambda \mathrm{B}_{2}\) is \(600 \mathrm{~mm} \mathrm{IIg}\), the total cquilibrium pressure is \(800 \mathrm{~mm} \mathrm{~kg}\). Calculate \(\mathrm{K}_{\mathrm{p}}\) for the reaction assuming that the volume of the system remains unchangcd. (1) 50 (2) 100 (3) \(166.8\) (4) 400
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