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Chapter 15: Problem 226

What is the \(\mathrm{OH}^{-}\) concentration of a solution that has a pH of \(9.66\) ? Is this solution acidic or basic?

Short Answer

Expert verified
The OH⁻ concentration of the solution is approximately \(4.57 \times 10^{-5} \, M\), and the solution is basic.

Step by step solution

01

Calculate pOH

To find pOH, we'll use the following equation: \(pH + pOH = 14\). We want to find pOH, so let's solve for it: \[pOH = 14 - pH\] Now, plug in the given pH value: \[pOH = 14 - 9.66\]
02

Evaluate pOH

Now, compute the pOH value: \[pOH = 4.34\]
03

Calculate OH⁻ concentration

To find the OH⁻ concentration, we'll use the following equation, where we relate pOH to the concentration of hydroxide ions: \[pOH = -\log_{10}[\mathrm{OH}^{-}]\] We want to find the hydroxide ion concentration, so let's solve for \([\mathrm{OH}^{-}]\): \[[\mathrm{OH}^{-}] = 10^{-pOH}\] Now, substitute the pOH value we found in step 2: \[[\mathrm{OH}^{-}] = 10^{-4.34}\]
04

Evaluate OH⁻ concentration

Now, compute the OH⁻ concentration: \[[\mathrm{OH}^{-}] \approx 4.57 \times 10^{-5} \, M\]
05

Determine if the solution is acidic or basic

Since the given pH value (9.66) is greater than 7, the solution is considered basic. The OH⁻ concentration of the solution is approximately \(4.57 \times 10^{-5} \, M\), and the solution is basic.

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Most popular questions from this chapter

When \(\mathrm{Fe}^{3+}\) ions dissolve in water, they immediately form \(\left[\mathrm{Fe}\left(\mathrm{OH}_{2}\right)_{6}\right]^{3+}\) aqueous ions in which six molecules of water bind to the iron via six Fe-O bonds. However, this is not all that happens. The solution also becomes acidic. Interestingly, \(\mathrm{Fe}^{2+}\) ions also form similar \(\left[\mathrm{Fe}\left(\mathrm{OH}_{2}\right)_{6}\right]^{2+}\) ions, but the solution does not become acidic. Explain why one solution becomes acidic and the other does not. (Hint: The more positive the metal center, the more it attracts electrons to itself. Think about the effect this has on bonds within the ions.)

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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?

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