Chapter 15: Problem 176
A buffer works by replacing added strong acid with weak acid. Explain how.
Chapter 15: Problem 176
A buffer works by replacing added strong acid with weak acid. Explain how.
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Consider the following statement: "As the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration in an aqueous solution increases, the \(\mathrm{OH}^{-}\) concentration must decrease." (a) Why is this true? (b) Is there any way to stop the \(\mathrm{OH}^{-}\) concentration from decreasing as you increase the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration?
Why is a pH of 7 equal to neutrality?
You mix \(500 \mathrm{~mL}\) of \(1.00 \mathrm{M} \mathrm{NaOCl}\) with \(500 \mathrm{~mL}\) of \(0.500 \mathrm{MHNO}_{3}\). Write an equation for the reaction that occurs. Besides water, what species are in the solution after reaction? Is this solution a buffer?
\(\mathrm{HClO}_{4}\) 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.
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