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Chapter 14: Problem 21

Which of the following conditions indicate a basic solution at \(25^{\circ} \mathrm{C} ?\) a. \(\mathrm{pOH}=11.21\) b. \(\mathrm{pH}=9.42\) c. \(\left[\mathrm{OH}^{-}\right]>\left[\mathrm{H}^{+}\right]\) d. \(\left[\mathrm{OH}^{-}\right]>1.0 \times 10^{-7} M\)

Short Answer

Expert verified
The conditions that indicate a basic solution at 25°C are: b. \(\mathrm{pH}=9.42\), c. \(\left[\mathrm{OH}^{-}\right]>\left[\mathrm{H}^{+}\right]\), and d. \(\left[\mathrm{OH}^{-}\right]>1.0 \times 10^{-7} M\).

Step by step solution

01

pH and pOH relationship

At 25°C, the relationship between the pH and pOH of a solution is given by the following equation: \[pH + pOH = 14\]
02

Analyzing option a

The pOH value given in this option is 11.21. We can use the pH and pOH relationship to find its corresponding pH value: \[pH = 14 - 11.21 = 2.79\] Since pH < 7, option a indicates an acidic solution, not a basic one.
03

Analyzing option b

The pH value given in this option is 9.42. Since pH > 7, option b indicates a basic solution.
04

Analyzing option c

This option states that the concentration of hydroxide ions (OH-) is greater than the concentration of hydrogen ions (H+). As mentioned in the analysis, a solution is considered basic when the concentration of its OH- ions is higher than its H+ ions. Therefore, option c indicates a basic solution.
05

Analyzing option d

This option states that the concentration of OH- ions is greater than 1.0 x 10^(-7) M. The ion product constant of water (Kw) at 25°C is given by: \[K_w = [H^+][OH^-] = 1.0 \times 10^{-14}\] Since the concentration of OH- ions is given to be greater than 1.0 x 10^(-7) M, the concentration of H+ ions will be smaller: \[[H^+] < 1.0 \times 10^{-7} M\] As the concentration of OH- ions is higher than the concentration of H+ ions, option d also indicates a basic solution.
06

Conclusion

Out of the given conditions, options b, c, and d indicate a basic solution at 25°C.

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Most popular questions from this chapter

The \(\mathrm{pOH}\) of a sample of baking soda dissolved in water is \(5.74\) at \(25^{\circ} \mathrm{C}\). Calculate the \(\mathrm{pH},\left[\mathrm{H}^{+}\right]\), and \(\left[\mathrm{OH}^{-}\right]\) for this sample. Is the solution acidic or basic?

Acrylic acid \(\left(\mathrm{CH}_{2}=\mathrm{CHCO}_{2} \mathrm{H}\right)\) is a precursor for many important plastics. \(K_{\mathrm{a}}\) for acrylic acid is \(5.6 \times 10^{-5}\). a. Calculate the \(\mathrm{pH}\) of a \(0.10 \mathrm{M}\) solution of acrylic acid. b. Calculate the percent dissociation of a \(0.10 \mathrm{M}\) solution of acrylic acid. c. Calculate the \(\mathrm{pH}\) of a \(0.050 \mathrm{M}\) solution of sodium acrylate \(\left(\mathrm{NaC}_{3} \mathrm{H}_{3} \mathrm{O}_{2}\right)\)

A \(10.0\) -mL sample of an \(\mathrm{HCl}\) solution has a \(\mathrm{pH}\) of \(2.000\). What volume of water must be added to change the \(\mathrm{pH}\) to \(4.000\) ?

Which of the following represent conjugate acid-base pairs? For those pairs that are not conjugates, write the correct conjugate acid or base for each species in the pair. a. \(\mathrm{H}_{2} \mathrm{O}, \mathrm{OH}\) c. \(\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{SO}_{4}^{2-}\) d. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}, \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\)

Using your results from Exercise 129, place the species in each of the following groups in order of increasing base strength. a. \(\mathrm{OH}^{-}, \mathrm{SH}^{-}, \mathrm{SeH}^{-}\) b. \(\mathrm{NH}_{3}, \mathrm{PH}_{3}\) c. \(\mathrm{NH}_{3}, \mathrm{HONH}_{2}\)
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