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Chapter 8: Problem 218

Match the following Column-I (a) Sodium acetate solution (b) Ferric chloride solution (c) Pure water (d) Ammonium acetate solution Column-II (p) \(\mathrm{pH}<7\) (q) \(\mathrm{pH}>7\) (r) salt hydrolysis (s) \(\mathrm{pH}=7\) (t) \(\mathrm{pH}>14\)

Short Answer

Expert verified
(a) q, r; (b) p, r; (c) s; (d) s.

Step by step solution

01

Match Sodium acetate solution

Sodium acetate solution results from dissolving a salt formed from a strong base (sodium hydroxide) and a weak acid (acetic acid). Therefore, the solution will be basic. So, it has a \( \text{pH} > 7 \) due to hydrolysis, making the correct matches \( \text{q} \) and \( \text{r} \).
02

Match Ferric chloride solution

Ferric chloride is a salt that comes from a reaction between a strong acid (HCl) and a weak base (ferric hydroxide). In water, it hydrolyzes to produce an acidic solution. Hence, it has \( \text{pH} < 7 \), so match it with \( \text{p} \) and \( \text{r} \).
03

Match Pure water

Pure water is neutral because it is not an acidic or basic solution. The \( \text{pH} \) of pure water is exactly 7. Therefore, match it with \( \text{s} \).
04

Match Ammonium acetate solution

Ammonium acetate comes from a weak acid (acetic acid) and a weak base (ammonia), and both ion hydrolyze in such a way that the solution remains approximately neutral. Therefore, match it with \( \text{s} \) because its \( \text{pH} \) is close to 7.

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Key Concepts

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

Acid-Base Properties
Understanding acid-base properties is fundamental to predicting the behavior of solutions. The pH scale is commonly used to express the acidity or basicity of a solution. The pH scale ranges from 0 to 14:
  • A pH less than 7 indicates an acidic solution, where more hydrogen ions (\(\text{H}^+\)) are present. For example, solutions like ferric chloride with a strong-acid-weak-base combination are typically acidic.
  • A pH greater than 7 implies a basic or alkaline solution, where hydroxide ions (\(\text{OH}^-\)) prevail. An example is sodium acetate, which forms from a weak acid and a strong base.
  • A pH of 7 is considered neutral, which means the number of hydrogen ions equals the number of hydroxide ions. Pure water perfectly exemplifies this neutral condition.
The behavior of a given salt in solution often depends on the strength of the original acid and base that form it. Recognizing whether the parent components are strong or weak helps determine if the solution will be acidic, neutral, or basic.
Salt Hydrolysis
Salt hydrolysis refers to the reaction of a salt with water leading to the formation of an acidic or basic solution. The ionization process involves the interaction between the ions of the salt and water. This process is especially apparent when a salt originates from a strong acid and a weak base, or vice versa.For example:
  • When ferric chloride (formed from a strong acid, HCl, and a weak base, ferric hydroxide) dissolves in water, it hydrolyzes to create an acidic solution. This occurs because the chloride ions (\(\text{Cl}^-\)) do not participate in further reactions, leaving the ferric ions to attract the hydroxide ions from water, increasing the concentration of hydrogen ions, and thus lowering the pH.
  • In contrast, sodium acetate (coming from a strong base, sodium hydroxide, and a weak acid, acetic acid) leads to a basic solution upon hydrolysis. This is because the acetate ions engage in reactions with water to form acetic acid and hydroxide ions, which raise the solution's pH.
These processes illustrate how the nature of the ions in the salt can either increase or decrease the pH of the resulting solution.
Strong and Weak Acids/Bases
The classification of acids and bases as strong or weak is based on their ionization in water. This principle is critical to understanding chemical behavior and pH in solutions.
  • Strong Acids and Bases: These are fully ionized in water, meaning they dissociate completely into ions. Hydrochloric acid (HCl) and sodium hydroxide (NaOH) are typical examples. The solutions of strong acids have very low pH values, while those of strong bases have very high pH values.
  • Weak Acids and Bases: These only partially dissociate in solution. Acetic acid and ammonia are examples where only a small fraction of the molecules ionize. Solutions of weak acids and bases have pH values that are closer to neutral, influenced by the degree of ionization.
In the context of our exercise:
  • The formation of sodium acetate solution involves a strong base (NaOH) and a weak acid (acetic acid), resulting in a basic solution.
  • Conversely, ferric chloride is the product of a strong acid (HCl) and a weak base (ferric hydroxide), leading to an acidic solution. This understanding aids in predicting solution behaviors and their corresponding pH levels.
These dynamics underscore the importance of the dissociation behavior of acids and bases in determining the characteristics of their resultant solutions.

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Most popular questions from this chapter

The \(\mathrm{pH}\) values of \(1 \mathrm{M}\) solutions of \(\mathrm{CH}_{3} \mathrm{COOH}\) (I), \(\mathrm{CH}_{3}, \mathrm{COONa}(\mathrm{II}), \mathrm{CH}_{3} \mathrm{COONH}_{4}(\mathrm{III})\), and \(\mathrm{KOH}\) (IV) will be in the order (a) IV \(>\mathrm{III}>\mathrm{II}>\mathrm{I}\) (b) IV \(>\mathrm{II}>\mathrm{III}>\mathrm{I}\) (c) \(\mathrm{I}>\mathrm{III}>\mathrm{II}>\mathrm{IV}\) (d) \(\mathrm{II}>\mathrm{I}>\mathrm{III}>\mathrm{IV}\)

At \(25^{\circ} \mathrm{C}\) the \(\mathrm{pH}\) value of a solution is 6 , the solution is (a) neutral (b) acidic (c) alkaline (d) basic

\(\mathrm{M}(\mathrm{OH}) \mathrm{x}\) has \(\mathrm{Ksp}=4 \times 10^{-12}\) and solubility \(10^{-4} \mathrm{M}, \mathrm{x}\) is (a) 1 (b) 2 (c) 3 (d) 4

The pKa of acetyl salicylic acid (aspirin) is \(3.5\). The \(\mathrm{pH}\) of gastric juice in human stomach is about \(2-3\) and \(\mathrm{pH}\) in the small intestine is about 8 . Aspirin will be (a) ionized in the small intestine and almost unionized in the stomach (b) unionized in the small intestine and in the stomach (c) completely ionized in the small intestine and in the stomach (d) ionized in the stomach and almost unionized in the small intestine.

Which of the following is correct? (a) the \(\mathrm{pH}\) of one litre solution containing \(0.49 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is \(2.0\) (b) the conjugate base of \(\mathrm{H}_{2} \mathrm{~S}\) is \(\mathrm{S}^{2-}\) (c) \(\mathrm{BF}_{3}\) is lewis base (d) phenolphthalein is colourless in basic medium.
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