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Chapter 17: Problem 26

An aqueous solution of sodium carbonate is alkaline because sodium carbonate is a salt of (a) weak acid and weak base (b) weak acid and strong base (c) strong acid and strong base (d) strong acid and weak base

Short Answer

Expert verified
(b) weak acid and strong base

Step by step solution

01

Identify the Components of Sodium Carbonate

Sodium carbonate, also known as Na2CO3, is composed of sodium ions (Na+) and carbonate ions (CO鈧兟测伝). Now we need to understand which acid and base give rise to these ions.
02

Determine the Type of Acid and Base

Carbonate ions (CO鈧兟测伝) come from carbonic acid (H鈧侰O鈧�), which is a weak acid, while sodium ions (Na+) come from NaOH, which is a strong base.
03

Evaluate the Nature of the Salt

Sodium carbonate is the salt formed between a weak acid (carbonic acid) and a strong base (sodium hydroxide). This type of salt leads to an alkaline solution when dissolved in water.

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Key Concepts

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

Alkalinity of Salts
Salts can have different effects on the pH of a solution, typically making it either acidic or alkaline. Sodium carbonate is a perfect example of an alkaline salt. When it dissolves in water, it increases the pH of the solution, making it basic. This is because sodium carbonate is a salt resulting from the reaction between a weak acid and a strong base.
The alkalinity of sodium carbonate comes from the dissociation of the carbonate ions in water. These ions react with water to produce hydroxide ions (OH鈦�), which increases the solution's pH.
  • The dissociation reaction of carbonate ions: \[ \text{CO}_3^{2-} + \text{H}_2\text{O} \rightarrow \text{HCO}_3^{-} + \text{OH}^{-} \]
  • This reaction liberates hydroxide ions, which are primarily responsible for the solution's alkalinity.
  • The process also partially reverses, but the net effect is an increase in hydroxide ions, boosting pH above 7.
Understanding how salts influence alkalinity helps in predicting the behavior of solutions in various chemical reactions and processes.
Weak Acid Strong Base Interaction
Weak acids and strong bases create a particular type of salt that often results in an alkaline solution. When a strong base like sodium hydroxide (NaOH) interacts with a weak acid such as carbonic acid (H鈧侰O鈧�), it produces sodium carbonate (Na鈧侰O鈧�), a salt.
  • The strong base, NaOH, fully dissociates in water to Na鈦� and OH鈦� ions.
  • The weak acid, H鈧侰O鈧�, only partially dissociates, providing very few H鈦� ions in solution.
  • In this interaction, the strong base dominates, and the resultant salt tends to create an alkaline environment when dissolved.
When sodium carbonate dissolves in water, it forms Na鈦�, CO鈧兟测伝, and some OH鈦� ions, which collectively increase the solution's pH above neutral. Therefore, understanding the interaction between weak acids and strong bases is crucial in predicting solution characteristics and their practical applications.
Carbonate Ions
Carbonate ions, represented as CO鈧兟测伝, are central to the chemistry of sodium carbonate. They originate from carbonic acid, H鈧侰O鈧�, which is a weak acid. Because it is weak, it does not completely dissociate in water. This partial dissociation is crucial for understanding the behavior of carbonate ions in solution.
Carbonate ions have several roles and properties in chemical reactions:
  • They exhibit a basic nature upon reacting with water, forming bicarbonate (HCO鈧冣伝) and hydroxide ions (OH鈦�), raising the pH of the solution:
  • Reaction: \[ \text{CO}_3^{2-} + \text{H}_2\text{O} \leftrightarrow \text{HCO}_3^{-} + \text{OH}^{-} \]
  • Carbonate ions also serve as buffer agents, helping to maintain the pH stability in various chemical and biological processes by neutralizing small amounts of added acids or bases.
Understanding carbonate ions facilitates a deeper comprehension of many natural phenomena, such as ocean chemistry and the formation of cave stalactites and stalagmites. So, their role is as essential in lab experiments as they are in natural processes.

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Most popular questions from this chapter

Aluminium is more reactive than iron because its standard reduction potential is higher. Still aluminium is less easily corrdoed than iron because (a) Al reacts with atmospheric carbon dioxide to form a self protective layer of \(\mathrm{Al}_{2} \mathrm{O}_{3}\) (b) it has higher reducing power and forms a self protective layer of \(\mathrm{Al}_{2} \mathrm{O}_{3}\) (c) it has higher reducing power and does not react with oxygen so easily (d) both (a) and (b)

Select the correct statement(s): (a) Be dissolves in alkali forming \(\left[\mathrm{Be}(\mathrm{OH})_{4}\right]^{2-}\) (b) \(\mathrm{BeF}_{2}\) forms complex ion with \(\mathrm{NaF}\) in which \(\mathrm{Be}\) goes with cation (c) \(\mathrm{BeCO}_{3}\) is kept in the atmosphere of \(\mathrm{CO}_{2}\) since, it is least thermally stable (d) \(\mathrm{BeF}_{2}\) forms complex ion with \(\mathrm{NaF}\) in which \(\mathrm{Be}\) goes with anion.

The metallic lusture exhibited by sodium is explained by (a) diffusion of sodium ions (b) oscillation of loose electrons (c) excitation of free electrons (d) existence of body centred cubic lattice.

Match the following (a) Castner Kellner (p) \(\mathrm{MgCl}_{2} .5 \mathrm{MgO} \cdot \mathrm{xH}_{2} \mathrm{O}\) cell (b) Pearl ash (q) \(\mathrm{K}_{2} \mathrm{CO}_{3}\) (c) Solvay's process (r) Manufacture of \(\mathrm{NaHCO}_{3}\)

Out of the following metals, those that cannot be obtained by electrolysis of the aqueous solution of their salts are 1\. \(\mathrm{Ag}\) 2\. \(\mathrm{Mg}\) 3\. Cu 4\. Al (a) 2,4 (b) 2,3 (c) 1,4 (d) all
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