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Chapter 15: Problem 37

Ammonium ion, \(\mathrm{NH}_{4}^{+}\), is a weak acid. Write the equation for its reaction with water.

Short Answer

Expert verified
The chemical equation for the reaction of the ammonium ion with water is: \( \mathrm{NH}_{4}^{+} \quad + \quad \mathrm{H}_{2}\mathrm{O} \quad \leftrightharpoons \quad \mathrm{NH}_{3} \quad + \quad \mathrm{H}_{3}\mathrm{O}^{+} \).

Step by step solution

01

Identify reactants and products

The ammonium ion (NH4+) will react with water (H2O) as its weak acid. The reaction will involve the transfer of a proton (H+) from the ammonium ion to the water molecule, resulting in the formation of ammonia (NH3) and a hydronium ion (H3O+).
02

Write the chemical equation

The chemical equation for the reaction of the ammonium ion with water can be written as follows: \( \mathrm{NH}_{4}^{+} \quad + \quad \mathrm{H}_{2}\mathrm{O} \quad \leftrightharpoons \quad \mathrm{NH}_{3} \quad + \quad \mathrm{H}_{3}\mathrm{O}^{+} \) In this equation, the reactants are the ammonium ion (NH4+) and water (H2O), and the products are ammonia (NH3) and hydronium ion (H3O+). The equation includes double arrows because the reaction is reversible.

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Most popular questions from this chapter

Does a mixture of carbonic acid, \(\mathrm{H}_{2} \mathrm{CO}_{3}\), a weak acid, and sodium bicarbonate, \(\mathrm{NaHCO}_{3}\), in water constitute a buffer? If no, explain why. If yes, explain why and use chemical equations to show what happens when either \(\mathrm{OH}\) or \(\mathrm{H}_{3} \mathrm{O}^{+}\) is added to the solution.

When a strong acid is added to a buffer, the \(\mathrm{pH}\) changes a little bit. (a) Does the pH increase or decrease? (b) Why does the \(\mathrm{pH}\) change at all? Why doesn't the buffer hold the \(\mathrm{pH}\) constant?

Other than water, what would you expect to find in the highest concentration in an aqueous solution of KOH? Explain.

When \(\mathrm{Fe}^{3+}\) ions dissolve in water, they immediately form \(\left[\mathrm{Fe}\left(\mathrm{OH}_{2}\right)_{6}\right]^{3+}\) aqueous ions in which six molecules of water bind to the iron via six Fe-O bonds. However, this is not all that happens. The solution also becomes acidic. Interestingly, \(\mathrm{Fe}^{2+}\) ions also form similar \(\left[\mathrm{Fe}\left(\mathrm{OH}_{2}\right)_{6}\right]^{2+}\) ions, but the solution does not become acidic. Explain why one solution becomes acidic and the other does not. (Hint: The more positive the metal center, the more it attracts electrons to itself. Think about the effect this has on bonds within the ions.)

Sulfuric acid, \(\mathrm{H}_{2} \mathrm{SO}_{4}\), is a diprotic acid with dissociation equilibrium constants of \(K_{\mathrm{eq}}>1.0 \times 10^{3}\) and \(K_{\mathrm{eq}}=1.2 \times 10^{-2} .\) Write the two dissociation equilibrium equations, and match the proper \(K_{\text {eq }}\) to each. Which species is the weak acid?
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