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Chapter 13: Problem 35

Calculate \(K_{a}\) for the weak acids that have the following \(\mathrm{pK}_{\mathrm{a}}\) values. (a) \(3.9\) (b) \(10.12\) (c) \(13.07\)

Short Answer

Expert verified
Question: Calculate the Ka values for weak acids with the following pKa values: (a) 3.9, (b) 10.12, (c) 13.07. Answer: The Ka values for the weak acids with the given pKa values are: (a) 1.26 × 10^-4, (b) 7.58 × 10^-11, (c) 8.56 × 10^-14.

Step by step solution

01

Write down the given values and formula

(Write the \(\mathrm{pK}_a\) values for each part (a), (b), and (c) and the formula \(\mathrm{pK}_a = -\log_{10}(K_a)\). (a) \(\mathrm{pK}_a = 3.9\) (b) \(\mathrm{pK}_a = 10.12\) (c) \(\mathrm{pK}_a = 13.07\) Formula: \(\mathrm{pK}_a = -\log_{10}(K_a)\)
02

Calculate the \(K_a\) values

(Use the formula to find the \(K_a\) values for each part (a), (b), and (c).) (a) \(K_a = 10^{-\mathrm{pK}_a} = 10^{-3.9}\) The \(K_a\) for part (a) is: \(K_{a} \approx 1.26 \times 10^{-4}\) (b) \(K_a = 10^{-\mathrm{pK}_a} = 10^{-10.12}\) The \(K_a\) for part (b) is: \(K_{a} \approx 7.58 \times 10^{-11}\) (c) \(K_a = 10^{-\mathrm{pK}_a} = 10^{-13.07}\) The \(K_a\) for part (c) is: \(K_{a} \approx 8.56 \times 10^{-14}\) The \(K_a\) values for the weak acids with the given \(\mathrm{pK}_a\) values are: (a) \(1.26 \times 10^{-4}\) (b) \(7.58 \times 10^{-11}\) (c) \(8.56 \times 10^{-14}\)

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Most popular questions from this chapter

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