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Chapter 15: Problem 139

Both the amide ion \(\left(\mathrm{NH}_{2}^{-}\right)\) and the nitride ion \(\left(\mathrm{N}^{3-}\right)\) are stronger bases than the hydroxide ion and hence do not exist in aqueous solutions. (a) Write equations showing the reactions of these ions with water, and identify the Brønsted acid and base in each case. (b) Which of the two is the stronger base?

Short Answer

Expert verified
For the amide ion reaction, \(NH_{2}^{-}\) is the Brønsted base, \(H_{2}O\) is the Brønsted acid. For the nitride ion reaction, \(N^{3-}\) is the Brønsted base, \(H_{2}O\) is the Brønsted acid. The nitride ion (\(N^{3-}\)) is the stronger base amongst the two.

Step by step solution

01

Write Equations

Start by writing the chemical equations for the reaction of the ions with water using the general acid-base reaction model, wherein bases accept a proton (\(H^{+}\)) from water:For the amide ion:\(NH_{2}^{-} + H_{2}O \rightarrow NH_{3} + OH^{-}\)For the nitride ion:\(N^{3-} + 3H_{2}O \rightarrow NH_{3} + 3OH^{-}\)
02

Identify Brønsted Acids and Bases

Next, identify the Brønsted acids and bases on each side of the equations:For the amide ion reaction:- Amide Ion (\(NH_{2}^{-}\)) is the Brønsted base as it accepts a proton.- Water (\(H_{2}O\)) is the Brønsted acid as it donates a proton.For the nitride ion reaction:- Nitride Ion (\(N^{3-}\)) is the Brønsted base as it accepts a proton.- Water (\(H_{2}O\)) is the Brønsted acid as it donates a proton.
03

Determine the Stronger Base

In order to determine which one is the stronger base, examine the reactions. Nitride ion, upon accepting three protons, produces three hydroxide ions. It's more ready to accept a proton than the amide ion. Hence, the nitride ion (\(N^{3-}\)) is the stronger base. The higher the charge and smaller the size of the ion, the greater its ability to attract a proton, thus behaving as a stronger base.

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Most popular questions from this chapter

When chlorine reacts with water, the resulting solution is weakly acidic and reacts with 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.

Hydrocyanic acid (HCN) is a weak acid and a deadly poisonous compound -in the gaseous form (hydrogen cyanide) it is used in gas chambers. Why is it dangerous to treat sodium cyanide with acids (such as HCl) without proper ventilation?

List the factors on which the \(K_{\mathrm{a}}\) of a weak acid depends.

Determine the concentration of a \(\mathrm{NH}_{4} \mathrm{Cl}\) solution that has a pH of 5.64 .

Calculate the hydrogen ion concentration in \(\mathrm{mol} / \mathrm{L}\) for solutions with the following pH values: (a) 2.42 , (b) \(11.21,(\mathrm{c}) 6.96\) (d) 15.00 .
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