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Chapter 15: Problem 28
Which solution is less acidic, solution \(A\) with \(\mathrm{pH} 2\) or solution \(\mathrm{B}\) with \(\mathrm{pH} 6\), and by how much?
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Write the mathematical expression that allows you to solve for the \(\mathrm{OH}^{-}\) concentration in water when you know only the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration.
Consider the neutralization reaction that occurs upon the reaction of aqueous potassium hydroxide with aqueous hydrochloric acid. (a) Write a complete ionic equation for this neutralization reaction. (b) Write a net ionic equation for this neutralization reaction.
Acetic acid is a weak acid. Upon losing a proton, acetic acid yields the acetate anion. (a) Draw a dot diagram for the acetate anion. (b) Hydrogen atoms that are bound to carbon atoms are not acidic. Knowing this, is it possible for the acetate anion to serve as an acid? Explain. (c) In fact, acetate ion is a weak base. Write a chemical equilibrium with unequal-length arrows showing how acetate in water produces a weakly basic solution. (d) Is water acting as an acid or a base? Explain.
Name one biological system in which control of \(\mathrm{pH}\) (buffering ability) is important, and name the buffer that is in control.
If you dissolve \(0.250 \mathrm{~g}\) of \(\mathrm{Ba}(\mathrm{OH})_{2}\) in \(3.00 \mathrm{~L}\) of water, what is the \(\mathrm{pH}\) of the solution?
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