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Chapter 10: Problem 40

What happens when a strong base such as \(\mathrm{KOH}\) is dissolved in water?

Short Answer

Expert verified
KOH dissociates in water, producing K+ and OH- ions, making the solution alkaline.

Step by step solution

01

Identify the Base

Recognize that the compound in question is potassium hydroxide, \( ext{KOH}\), which is a strong base.
02

Dissociation in Water

Understand that when \( ext{KOH}\) is dissolved in water, it dissociates completely into its constituent ions. The dissociation reaction is represented as: \[ ext{KOH} (s) \rightarrow ext{K}^+ (aq) + ext{OH}^- (aq)\]
03

Effect on pH

Due to the release of hydroxide ions (\( ext{OH}^-\)) into the solution, the pH of the solution increases, making it alkaline. A strong base like \( ext{KOH}\) raises the pH towards the higher end of the pH scale (greater than 7).

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Key Concepts

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

Potassium Hydroxide
Potassium hydroxide, commonly referred to as KOH, is known for its high solubility in water. This compound is classified as a strong base, which means it can completely dissociate in water to yield potassium ions (\(\mathrm{K}^+\)) and hydroxide ions (\(\mathrm{OH}^-\)). It's an industrially important substance, widely used in the manufacturing of soaps, fertilizers, and various chemicals. Due to its caustic nature, it must be handled with care as it can cause burns upon contact.
Dissociation in Water
When potassium hydroxide dissolves in water, it undergoes a process known as dissociation. The solid KOH separates into its constituent ions of potassium (\(\mathrm{K}^+\)) and hydroxide (\(\mathrm{OH}^-\)) in an aqueous solution. This complete dissociation is what characterizes KOH as a strong base:\[ \mathrm{KOH}(s) \rightarrow \mathrm{K}^+(aq) + \mathrm{OH}^-(aq) \]This reaction is crucial because it leads to the increase in hydroxide ion concentration in water, influencing the pH of the solution.
pH Scale
The pH scale is a numerical representation of the acidity or basicity of a solution. It ranges from 0 to 14, with 7 being neutral, representing pure water. A pH less than 7 indicates an acidic solution, while a pH greater than 7 indicates a basic or alkaline solution. When KOH dissociates in water, it increases the concentration of hydroxide ions, thus raising the pH of the solution. A high pH value, typically close to 14, is indicative of a strong base such as potassium hydroxide.
Chemical Reactions
In general, chemical reactions involving strong bases like potassium hydroxide are significant in various fields such as cleaning, chemistry, and industry. When KOH is used in reactions, it typically serves either to neutralize acids or to act as a reactant itself to produce different compounds. For example:
  • In soap making, KOH reacts with fats to produce potassium soaps, which are soft and beneficial for various cleaning applications.
  • In chemical synthesis, it can act as a catalyst or reactant to speed up or induce reactions.
Being a strong base, KOH facilitates these reactions by altering the pH and providing the necessary hydroxide ions to drive these chemical processes forward.

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Most popular questions from this chapter

Label the Br酶nsted-Lowry acids and bases in the following equations, and tell which substances are conjugate acid-base pairs. $$ \begin{array}{l} \text { (a) } \mathrm{CO}_{3}^{2-}(a q)+\mathrm{HCl}(a q) \longrightarrow \mathrm{HCO}_{3}^{-}(a q)+\mathrm{Cl}^{-}(a q) \\ \text { (b) } \mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{NH}_{3}(a q) \longrightarrow \\ & \mathrm{H}_{2} \mathrm{PO}_{4}^{-}(a q)+\mathrm{NH}_{4}^{+}(a q) \\ \text { (c) } \mathrm{NH}_{4}^{+}(a q)+\mathrm{CN}^{-}(a q) \rightleftarrows \mathrm{NH}_{3}(a q)+\mathrm{HCN}(a q) \\ \text { (d) } \mathrm{HBr}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Br}^{-}(a q) \end{array} $$ (e) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}(a q)+\mathrm{N}_{2} \mathrm{H}_{4}(a q) \rightleftarrows\) $$ \mathrm{HPO}_{4}^{2-}(a q)+\mathrm{N}_{2} \mathrm{H}_{5}^{+}(a q) $$

A \(0.10 M\) solution of the deadly poison hydrogen cyanide, HCN, has a pH of 5.2. Calculate the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) of the solution. Is HCN a strong or a weak acid?

What is the approximate \(\mathrm{pH}\) of a \(0.02 \mathrm{M}\) solution of a strong monoprotic acid? Of a \(0.02 M\) solution of a strong base, such as \(\mathrm{KOH}\) ?

If \(35.0 \mathrm{~mL}\) of a \(0.100 \mathrm{~N}\) acid solution is needed to reach the end point in titration of \(21.5 \mathrm{~mL}\) of a base solution, what is the normality of the base solution?

Write balanced equations for proton-transfer reactions between the listed pairs. Indicate the conjugate pairs, and determine the favored direction for each equilibrium. (a) \(\mathrm{HCl}\) and \(\mathrm{PO}_{4}^{3-}\) (b) \(\mathrm{HCN}\) and \(\mathrm{SO}_{4}^{2-}\) (c) \(\mathrm{HClO}_{4}\) and \(\mathrm{NO}_{2}^{-}\) (d) \(\mathrm{CH}_{3} \mathrm{O}^{-}\) and \(\mathrm{HF}\)
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