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Chapter 16: Problem 22

Calculate the number of moles of \(\mathrm{KOH}\) in \(5.50 \mathrm{~mL}\) of a \(0.360 \mathrm{M}\) KOH solution. What is the \(\mathrm{pOH}\) of the solution?

Short Answer

Expert verified
The number of moles of KOH in \(5.50 \mathrm{~mL}\) of a \0.360 M\ KOH solution is approximately 0.00198 moles, and the pOH of the solution is approximately 0.44.

Step by step solution

01

Calculate the number of moles of KOH

To find the number of moles of a species in solution, multiply the volume of the solution (converted to liters) by the molarity of the solution. First, convert the volume from mL to L: \(5.50 \mathrm{~mL} = 0.00550 \mathrm{~L}\). Next, we multiply this volume by the molarity: moles of KOH = \(0.00550 \mathrm{~L} \times 0.360 \mathrm{M} = 0.00198 \mathrm{~moles}\).
02

Calculate the pOH of the solution

pOH is calculated as the negative logarithm (base 10) of the hydroxide ion concentration, [OH-]. Since KOH fully dissociates in water into K+ and OH- ions, the molarity of the KOH solution is equivalent to the [OH-]. Convert the molarity of KOH solution to [OH-]: \([OH-] = 0.360 \mathrm{M}\). Then, calculate pOH = \( -\log[0.360] = -\log[3.6 \times 10^{-1}]\). After calculation, pOH equals approximately 0.44.

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Most popular questions from this chapter

To which of the following would the addition of an equal volume of \(0.60 \mathrm{M} \mathrm{NaOH}\) lead to a solution having a lower \(\mathrm{pH} ?\) (a) water, (b) \(0.30 \mathrm{M} \mathrm{HCl}\), (c) \(0.70 \mathrm{M} \mathrm{KOH}\) (d) \(0.40 \mathrm{M} \mathrm{NaNO}_{3}\).

In a certain experiment a student finds that the \(\mathrm{pHs}\) of \(0.10 M\) solutions of three potassium salts \(K X, K Y\) and \(\mathrm{KZ}\) are 7.0,9.0 , and 11.0 , respectively. Arrange the acids HX, HY, and HZ in order of increasing acid strength.

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

Prediet the \(\mathrm{pH}(>7,<7,\) or \(\approx 7)\) of the aqueous solutions containing the following salts: (a) \(\mathrm{KBr}\) (b) \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) (c) \(\mathrm{BaCl}_{2}\) (d) \(\mathrm{Bi}\left(\mathrm{NO}_{3}\right)_{3}\).

Calculate the hydrogen ion concentration in moles per liter for each of these solutions: (a) a solution whose \(\mathrm{pH}\) is \(5.20,\) (b) a solution whose \(\mathrm{pH}\) is 16.00 ; (c) a solution whose hydroxide concentration is \(3.7 \times 10^{-9} M\).
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