Chapter 15: Problem 154
The \(\mathrm{pH}\) of a solution is 4 . (a) What is the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration? (b) What is the \(\mathrm{OH}^{-}\) concentration? (c) Is this solution acidic or basic?
Chapter 15: Problem 154
The \(\mathrm{pH}\) of a solution is 4 . (a) What is the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration? (b) What is the \(\mathrm{OH}^{-}\) concentration? (c) Is this solution acidic or basic?
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Get started for freeWhat is the \(\mathrm{pH}\) of a solution whose \(\mathrm{OH}^{-}\) concentration is \(10^{-14} \mathrm{M} ?\) Is the solution acidic or basic?
\(\mathrm{HClO}_{4}\) is a strong acid, and \(\mathrm{HClO}_{2}\) is a weak acid. If you had a \(1.0 \mathrm{M}\) solution of \(\mathrm{NaClO}_{4}\) and a \(1.0 \mathrm{M}\) solution of \(\mathrm{NaClO}_{2}\), which would have the higher pH? Explain.
Ethanol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\), and hydride ion, \(\mathrm{H}^{-}\), react to produce \(\mathrm{H}_{2}\) gas and the \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{O}^{-}\) anion. Arrhenius could not tell you what is going on, but Bronsted and Lowry would have no trouble. How would they explain this reaction?
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.)
What is the molar concentration of hydronium ion and hydroxide ion in pure water at \(25{ }^{\circ} \mathrm{C}\) ?
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