Calculate the concentration of all species in a 0.225 M C₆H₅NH₃Cl solution.

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Identify the components of the solution: C6H5NH3Cl is an ionic compound that dissociates into C6H5NH3+ (anilinium ion) and Cl- (chloride ion) in water.

Recognize that C6H5NH3+ is a weak acid, which can donate a proton to water, forming C6H5NH2 (aniline) and H3O+ (hydronium ion).

Write the equilibrium expression for the dissociation of C6H5NH3+ in water: C6H5NH3+ + H2O ⇌ C6H5NH2 + H3O+.

Use the acid dissociation constant (Ka) for C6H5NH3+ to set up an ICE (Initial, Change, Equilibrium) table to find the concentrations of C6H5NH2 and H3O+ at equilibrium.

Calculate the concentration of Cl- ions, which is equal to the initial concentration of C6H5NH3Cl, since it fully dissociates in water.

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Acid-Base Chemistry

C6H5NH3Cl, or phenylammonium chloride, is a salt formed from the weak base aniline (C6H5NH2) and hydrochloric acid (HCl). In solution, it dissociates into C6H5NH3+ (the conjugate acid) and Cl-. Understanding the behavior of weak acids and bases is crucial for determining the concentrations of species in solution.

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02:00

Arrhenius Acids and Bases

Dissociation of Salts

When salts dissolve in water, they dissociate into their constituent ions. For C6H5NH3Cl, it dissociates completely into C6H5NH3+ and Cl-. The concentration of each ion in the solution can be directly derived from the initial concentration of the salt, which is 0.225 M in this case.

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00:50

Ionic Salts

Equilibrium and Concentration Calculations

In solutions involving weak acids or bases, equilibrium plays a significant role. The concentration of the conjugate acid (C6H5NH3+) will influence the pH of the solution. To calculate the concentrations of all species, one must consider both the initial concentration and any changes due to dissociation and equilibrium shifts.

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