At (40 .^{circ} mathrm{C}) the value of (K_{mathrm{w}}) is (2.92 times 10^{-14}). a. Calculate the (left[mathrm{H}^{+}ight])and (left[mathrm{OH}^{-}ight])in

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At $40 .^{\circ} \mathrm{C}$ the value of $K_{\mathrm{w}}$ is $2.92 \times 10^{-14}$.

a. Calculate the $\left[\mathrm{H}^{+}ight]$and $\left[\mathrm{OH}^{-}ight]$in pure water at $40 .{ }^{\circ} \mathrm{C}$.

b. What is the $\mathrm{pH}$ of pure water at $40 .^{\circ} \mathrm{C}$ ?

c. If the hydroxide ion concentration in a solution is $0.10 \mathrm{M}$, what is the $\mathrm{pH}$ at $40 .{ }^{\circ} \mathrm{C}$ ?

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Chemical Principles

ISBN: 9780618946907

6th Edition

Authors: Steven S Zumdahl

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Question Posted: Jan 24, 2024 07:01 AM

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At (40 .^{circ} mathrm{C}) the value of (K_{mathrm{w}}) is (2.92 times 10^{-14}). a. Calculate the (left[mathrm{H}^{+}ight])and (left[mathrm{OH}^{-}ight])in

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This question is related to the autoionization of water and the concept of pH and pOH Lets break it ...View the full answer

Chemical Principles

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