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Chapter 15: Problem 84

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

Short Answer

Expert verified
The solution of the salt K2HPO4 will be basic.

Step by step solution

01

Identifying the source of the ions

SyntaxHighlighterFirstly, identify the source of the ions in the salt. The salt K2HPO4 is composed of K+ ions, which come from the strong base KOH, and HPO4^2- ions, which come from the weak base H3PO4.
02

Determine the likelihood of hydrolysis

The next step is to determine which ions are likely to undergo hydrolysis. Ions that have come from a strong acid or strong base would not hydrolyze and therefore do not affect the final pH of the solution. In our case, K+ is a product of KOH (a strong base) and will therefore not undergo hydrolysis. However, HPO4^2-, being a derivative of a weak acid (H3PO4), is prone to hydrolyze according to the equation: \[\mathrm{HPO}_{4}^{2-} + \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{2} \mathrm{PO}_{4}^{-} + \mathrm{OH}^{-}\]The reaction generates OH-, which makes the solution basic.
03

Analyzing the pH

Since the anion of the salt goes to hydrolyzation and produces OH- ions, this means the solution turns basic. Thus, the pH of the solution will be more than 7.

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Most popular questions from this chapter

Specify which of the following salts will undergo hydrolysis: \(\mathrm{KF}, \mathrm{NaNO}_{3}, \mathrm{NH}_{4} \mathrm{NO}_{2}, \mathrm{MgSO}_{4}, \mathrm{KCN}\) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COONa}, \mathrm{RbI}, \mathrm{Na}_{2} \mathrm{CO}_{3}, \mathrm{CaCl}_{2}, \mathrm{HCOOK}\).

\(\mathrm{Zn}(\mathrm{OH})_{2}\) is an amphoteric hydroxide. Write balanced ionic equations to show its reaction with (a) \(\mathrm{HCl},\) (b) \(\mathrm{NaOH}\) [the product is \(\left.\mathrm{Zn}(\mathrm{OH})_{4}^{2-}\right]\).

What are the concentrations of \(\mathrm{HSO}_{4}^{-}, \mathrm{SO}_{4}^{2-},\) and \(\mathrm{H}^{+}\) in a \(0.20 \mathrm{M} \mathrm{KHSO}_{4}\) solution?

Write equations for the reactions between (a) \(\mathrm{CO}_{2}\) and \(\mathrm{NaOH}(a q),\) (b) \(\mathrm{Na}_{2} \mathrm{O}\) and \(\mathrm{HNO}_{3}(a q)\).

The ion product of \(\mathrm{D}_{2} \mathrm{O}\) is \(1.35 \times 10^{-15}\) at \(25^{\circ} \mathrm{C}\). (a) Calculate \(\mathrm{pD}\) where \(\mathrm{pD}=-\log \left[\mathrm{D}^{+}\right]\). (b) For what values of \(\mathrm{pD}\) will a solution be acidic in \(\mathrm{D}_{2} \mathrm{O} ?\) (c) Derive a relation between \(\mathrm{pD}\) and \(\mathrm{pOD}\).
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