The correct order of increasing [OH^-] in the following aqueous solution is (a) 0.01 M-NaHCO3<0.

step 1 In this problem, the correct order for the correct order of S3O plus is as follow. So just look

The correct order of increasing [OH^-] in the following...

The correct order of increasing $\left[\mathrm{OH}^{-}\right]$ in the following aqueous solution is (a) $0.01 \mathrm{M}-\mathrm{NaHCO}_{3}<0.01 \mathrm{M}-\mathrm{NaCN}$ $<0.01 \mathrm{M}-\mathrm{KCl}$ (b) $0.01 \mathrm{M}-\mathrm{KCl}<0.01 \mathrm{M}-\mathrm{NaCN}$ $<0.01 \mathrm{M}-\mathrm{NaHCO}_{3}$ (c) $0.01 \mathrm{M}-\mathrm{KCl}<0.01 \mathrm{M}-\mathrm{NaHCO}_{3}$ $<0.01 \mathrm{M}-\mathrm{NaCN}$ (d) $0.01 \mathrm{M}-\mathrm{NaCN}<0.01 \mathrm{M}-\mathrm{KCl}$ $<0.01 \mathrm{M}-\mathrm{NaHCO}_{3}$

The correct order of increasing $\left[\mathrm{OH}^{-}\right]$ in the following aqueous solution is
(a) $0.01 \mathrm{M}-\mathrm{NaHCO}_{3}<0.01 \mathrm{M}-\mathrm{NaCN}$
$<0.01 \mathrm{M}-\mathrm{KCl}$
(b) $0.01 \mathrm{M}-\mathrm{KCl}<0.01 \mathrm{M}-\mathrm{NaCN}$
$<0.01 \mathrm{M}-\mathrm{NaHCO}_{3}$
(c) $0.01 \mathrm{M}-\mathrm{KCl}<0.01 \mathrm{M}-\mathrm{NaHCO}_{3}$
$<0.01 \mathrm{M}-\mathrm{NaCN}$
(d) $0.01 \mathrm{M}-\mathrm{NaCN}<0.01 \mathrm{M}-\mathrm{KCl}$
$<0.01 \mathrm{M}-\mathrm{NaHCO}_{3}$

Key Concepts

Salt Hydrolysis

Salt hydrolysis refers to the reaction of an ion from a dissolved salt with water, which can produce either hydronium (H3O+) or hydroxide (OH–) ions. The extent of this reaction depends on whether the ion is a conjugate base of a weak acid or a conjugate acid of a weak base. This process is essential in determining the pH of a salt solution.

Conjugate Acid?Base Pairs

In aqueous solutions, the ions produced by salts act as the conjugate bases or acids of their respective neutral molecules. When a salt is derived from a weak acid, its anion is often a relatively strong base, capable of accepting a proton from water to generate hydroxide ions, thereby increasing the solution’s pH. Conversely, cations from weak bases can donate a proton to water, resulting in acidic properties.

Equilibrium Constant and Basicity (Kb)

The basic strength of an ion in solution is quantified by its equilibrium constant (Kb) for the hydrolysis reaction. The magnitude of Kb determines the concentration of hydroxide ions produced. A larger Kb indicates a higher degree of ion hydrolysis and thus a more basic solution, while a smaller Kb suggests weaker basic properties.

Neutral Salts and Their Effect on pH

Neutral salts, typically formed from strong acids and strong bases, do not significantly interact with water to change the pH. They dissociate completely in solution without undergoing hydrolysis, meaning that the concentration of hydroxide or hydronium ions remains effectively unchanged from that in pure water.

Amphiprotic Behavior

Some ions, particularly those derived from polyprotic acids, can exhibit amphiprotic behavior, meaning they can act both as an acid and as a base. Their contribution to the hydroxide ion concentration in solution depends on the specific equilibrium in the system, as well as the relative strengths of their acidic and basic forms.

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