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Chapter 15: Problem 29

What is the strongest acid and the strongest base that can exist in water?

Short Answer

Expert verified
The strongest acid that can exist in water is the hydronium ion (\(H_3O^+\)) and the strongest base that can exist in water is the hydroxide ion (\(OH^-\)).

Step by step solution

01

Understanding Water Autoionization

At any given moment, some molecules of water (H2O) may dissociate to form hydronium and hydroxide ions. This process is known as autoionization of water and is reversible. It can be represented as: \[2H_2O \Leftrightarrow H_3O^+ + OH^-\] This means that water can act as both an acid and a base. Since water is the solvent in this instance and is neutral, the strongest possible acid it can produce is hydronium \((H_3O^+)\), and the strongest base it can produce is hydroxide \((OH^-)\). Both these ions are in equilibrium with water.
02

Determining the Strongest Acid and Base in Water

As noted in the previous step, the strongest acid that can exist in water is the hydroxide ion \(OH^-\), and the strongest base is the hydronium ion \(H_3O^+\). There are other substances which are stronger acids or bases but they cannot exist in water because water will neutralize them. Hydronium and hydroxide ions represent the limit to the acidity and basicity of water. These are the strongest acid and base that can exist in water.

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Most popular questions from this chapter

Like water, liquid ammonia undergoes autoionization: $$ \mathrm{NH}_{3}+\mathrm{NH}_{3} \rightleftharpoons \mathrm{NH}_{4}^{+}+\mathrm{NH}_{2}^{-} $$ (a) Identify the Brønsted acids and Brønsted bases in this reaction. (b) What species correspond to \(\mathrm{H}^{+}\) and \(\mathrm{OH}^{-}\) and what is the condition for a neutral solution?

Consider the two weak acids HX (molar mass = \(180 \mathrm{~g} / \mathrm{mol}\) ) and \(\mathrm{HY}\) (molar mass \(=78.0 \mathrm{~g} / \mathrm{mol}\) ). If a solution of \(16.9 \mathrm{~g} / \mathrm{L}\) of \(\mathrm{HX}\) has the same \(\mathrm{pH}\) as one containing \(9.05 \mathrm{~g} / \mathrm{L}\) of \(\mathrm{HY},\) which is the stronger acid at these concentrations?

Why do we normally not quote \(K_{\mathrm{a}}\) values for strong acids such as \(\mathrm{HCl}\) and \(\mathrm{HNO}_{3}\) ? Why is it necessary to specify temperature when giving \(K_{\mathrm{a}}\) values?

Calculate the \(\mathrm{pH}\) of a \(0.20 \mathrm{M} \mathrm{NaHCO}_{3}\) solution. (Hint: As an approximation, calculate hydrolysis and ionization separately first, followed by partial neutralization.)

Explain the action of smelling salt, which is ammonium carbonate \(\left[\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}\right] .\) (Hint: The thin film of aqueous solution that lines the nasal passage is slightly basic.
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