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Chapter 16: Problem 59

List four factors that affect the strength of an acid.

Short Answer

Expert verified
Four factors that affect the strength of an acid are: the stability of the conjugate base, the polarity and solubility of the molecule in water, the atomic radius of the central atom, and the electronegativity of the central atom.

Step by step solution

01

Identify the Four Factors

To solve this exercise, the following four factors can be considered: 1. The stability of the conjugate base; 2. The polarity and solubility of the molecule in water; 3. The atomic radius of the central atom; and 4. The electronegativity of the central atom.
02

Explain each Factor

1. The Strength of an acid is influenced by the stability of the conjugate base. A more stable conjugate base leads to a stronger acid.\newline 2. Solubility in water: Substances that can dissolve in water and donate protons tend to be more acidic.\newline 3. The atomic radius of the central atom: Larger central atoms can accommodate negative charge better, thus the strength of an acid increases with the size of the central atom.\newline 4. The electronegativity of the central atom: Higher electronegativity of the central atom assists in stabilizing any extra negative charge, therefore a highly electronegative central atom leads to a strong acid.

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Most popular questions from this chapter

Oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) has the following structure: An oxalic acid solution contains these species in varying concentrations: \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}, \mathrm{HC}_{2} \mathrm{O}_{4}^{-}, \mathrm{C}_{2} \mathrm{O}_{4}^{2-}\), and \(\mathrm{H}^{+}\). (a) Draw Lewis structures of \(\mathrm{HC}_{2} \mathrm{O}_{4}^{-}\) and \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\). (b) Which of the four species listed here can act only as acids, which can act only as bases, and which can act as both acids and bases?

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

\(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a strong acid, but \(\mathrm{HSO}_{4}^{-}\) is a weak acid. Account for the difference in strength of these two related species.

When chlorine reacts with water, the resulting solution is weakly acidic and reacts with \(\mathrm{AgNO}_{3}\) to give a white precipitate. Write balanced equations to represent these reactions. Explain why manufacturers of household bleaches add bases such as \(\mathrm{NaOH}\) to their products to increase their effectiveness.

The \(\mathrm{pH}\) of a solution is 6.7 . From this statement alone, can you conclude that the solution is acidic? If not, what additional information would you need? Can the \(\mathrm{pH}\) of a solution be zero or negative? If so, give examples to illustrate these values.
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