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Chapter 15: Problem 66

Calculate the concentrations of \(\mathrm{H}^{+}, \mathrm{HCO}_{3}^{-},\) and \(\mathrm{CO}_{3}^{2-}\) in a \(0.025 \mathrm{M} \mathrm{H}_{2} \mathrm{CO}_{3}\) solution.

Short Answer

Expert verified
The concentrations are therefore: \(\mathrm{H}^{+}\) = 0M, \(\mathrm{HCO}_{3}^{-}\) = 0M, \(\mathrm{CO}_{3}^{2-}\) = 0M. Since these are weak acids and given concentrations are also low, very little of each acid will actually dissociate, so their concentrations remain approximately 0M.

Step by step solution

01

Identify the dissociation reactions

The two reactions we need to consider are: 1. \(\mathrm{H}_{2} \mathrm{CO}_{3}\) ⟶ \(\mathrm{H}^{+}\) + \(\mathrm{HCO}_{3}^{-}\) 2. \(\mathrm{HCO}_{3}^{-}\) ⟶ \(\mathrm{H}^{+}\) + \(\mathrm{CO}_{3}^{2-}\)
02

Identify given concentrations

According to the information given, the initial concentration of \(\mathrm{H}_{2} \mathrm{CO}_{3}\) is 0.025M.
03

Solve for concentrations after first dissociation

Because carbonic acid is a weak acid, a negligible amount of it will dissociate. We can therefore consider the \(\mathrm{H}^{+}\) and \(\mathrm{HCO}_{3}^{-}\) concentrations after the first dissociation to also be negligible, hence approximately 0M.
04

Solve for Concentrations after second dissociation

The remaining \(\mathrm{HCO}_{3}^{-}\) will then dissociate into \(\mathrm{H}^{+}\) and \(\mathrm{CO}_{3}^{2-}\). Since bicarbonate is also a weak acid, only a negligible amount will dissociate, creating a negligible amount of \(\mathrm{H}^{+}\) and \(\mathrm{CO}_{3}^{2-}\) ions.
05

Add up the concentrations

To obtain the final concentrations, we add up the concentrations due to each dissociation:1. For \(\mathrm{H}^{+}\): 0M (from first dissociation) + 0M (from second dissociation) = 0M2. For \(\mathrm{HCO}_{3}^{-}\): 0M (from first dissociation) - 0M (from second dissociation) = 0M3. For \(\mathrm{CO}_{3}^{2-}\): 0M (from second dissociation)

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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?

Predict whether a solution containing the salt \(\mathrm{K}_{2} \mathrm{HPO}_{4}\) will be acidic, neutral, or basic.

Describe the hydration of \(\mathrm{SO}_{2}\) as a Lewis acid-base reaction. (Hint: Refer to the discussion of the hydration of \(\mathrm{CO}_{2}\) in Section \(\left.15.12 .\right)\)

Write all the species (except water) that are present in a phosphoric acid solution. Indicate which species can act as a Brønsted acid, which as a Brønsted base, and which as both a Brønsted acid and a Brønsted base.

Consider the following compounds: Experimentally, phenol is found to be a stronger acid than methanol. Explain this difference in terms of the structures of the conjugate bases. (Hint: A more stable conjugate base favors ionization. Only one of the conjugate bases can be stabilized by resonance.
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