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Chapter 15: Problem 115

To be a weak base in water, a molecular compound must also be a weak electrolyte. What must be one of the ions it produces in water?

Short Answer

Expert verified
One of the ions produced by a weak base when it acts as a weak electrolyte in water must be the hydroxide ion (OH-).

Step by step solution

01

Understand weak bases and weak electrolytes

A weak base is a substance that does not completely ionize or dissociate in water to produce hydroxide ions (OH-) and its conjugate acid. A weak electrolyte is a substance that partially dissociates into its constituent ions in water, and thus does not conduct electricity as efficiently as a strong electrolyte.
02

Identify a common ion produced by weak bases in water

When weak bases dissolve in water, they partially ionize, producing hydroxide ions (OH-) and conjugate acid ions. One of the ions produced by a weak base in water is the hydroxide ion (OH-).
03

Answer the question

One of the ions produced by a weak base when it acts as a weak electrolyte in water must be the hydroxide ion (OH-).

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Most popular questions from this chapter

Is a solution that contains \(0.10 \mathrm{M} \mathrm{HBr}\) and \(0.10 \mathrm{M}\) NaBr a buffered solution? Why or why not?

Without using a calculator, what is the base-10 logarithm of \(10^{13}\) ?

How does a buffer "kill" added strong base?

A \(0.20 \mathrm{M}\) aqueous solution of monoprotic acid HX has a pH of \(2.14\). (a) Is HX a strong acid or a weak acid? (b) Calculate \(K_{\text {eq }}\) for the reaction of HX with water. (Hint: What are the equilibrium concentrations of \(\mathrm{H}_{3} \mathrm{O}^{+}, \mathrm{X}^{-}\), and HX?)

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.
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