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Chapter 16: Problem 19

Complete this table for a solution: $$\begin{array}{c|c|c}\mathrm{pH} & {\left[\mathrm{H}^{+}\right]} & \text {Solution is } \\\\\hline<7 & & \\\\\hline & <1.0 \times 10^{-7} M & \\\\\hline & & \text { Neutral }\end{array}$$

Short Answer

Expert verified
The completed table is as followed: \[\begin{array}{c|c|c}\text{pH} & \left[\mathrm{H}^{+}\right] & \text{Solution is} \\<7 & >1.0 \times 10^{-7} M & \text{Acidic} \ & <1.0 \times 10^{-7} M & \text{Basic} \ 7 & =1.0 \times 10^{-7} M & \text{Neutral}\end{array}\]

Step by step solution

01

Fill in the acidity or alkalinity of the solution

Looking at the first row with pH < 7, the solution is acidic. Then in the third row where it says 'neutral', the solution is not acidic nor basic, therefore the pH is 7.
02

Determine the concentration of hydronium ions based on pH

Since the pH < 7 in the first row, the concentration of \( \mathrm{H}^{+} \) ions will be > \(1.0 \times 10^{-7} M\). In the last row where it's neutral, the concentration of \( \mathrm{H}^{+} \) ions will be = \(1.0 \times 10^{-7} M\).
03

Determine the acidity or alkalinity based on concentration of hydronium ions

In the second row, where it states that \( \mathrm{H}^{+} \) ions is < \(1.0 \times 10^{-7} M\), the solution will be basic as the concentration of hydrogen ions is lower than that for a neutral solution.
04

Now we will fill out the entire table

Now that we have the information for each condition, we can fill in the entire table as such : \[\begin{array}{c|c|c}\text{pH} & \left[\mathrm{H}^{+}\right] & \text{Solution is} \\<7 & >1.0 \times 10^{-7} M & \text{Acidic} \ & <1.0 \times 10^{-7} M & \text{Basic} \ 7 & =1.0 \times 10^{-7} M & \text{Neutral}\end{array}\]

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Most popular questions from this chapter

Write an equation relating \(\left[\mathrm{H}^{+}\right]\) and \(\left[\mathrm{OH}^{-}\right]\) in solution at \(25^{\circ} \mathrm{C}\).

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? (Hint: \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a strong acid: \(K_{\mathrm{a}}\) for \(\left.\mathrm{HSO}_{4}^{-}=1.3 \times 10^{-2} .\right)\)

How many milliliters of a strong monoprotic acid solution at \(\mathrm{pH}=4.12\) must be added to \(528 \mathrm{~mL}\) of the same acid solution at \(\mathrm{pH}=5.76\) to change its \(\mathrm{pH}\) to \(5.34 ?\) Assume that the volumes are additive.

Novocaine, used as a local anesthetic by dentists, is a weak base \(\left(K_{\mathrm{b}}=8.91 \times 10^{-6}\right)\). What is the ratio of the concentration of the base to that of its acid in the blood plasma \((\mathrm{pH}=7.40)\) of a patient?

Classify each of these species as a weak or strong base: (a) LiOH, (b) \(\mathrm{CN}^{-}\) (c) \(\mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{ClO}_{4}^{-},(\mathrm{e}) \mathrm{NH}_{2}^{-}\)
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