91Ó°ÊÓ

In an acidic solution, how does the concentration of \(\mathrm{H}_{3} \mathrm{O}^{+}\) compare to the concentration of \(\mathrm{OH}^{-}\) ?

If a base is added to pure water, why does the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) decrease?

Indicate whether each of the following solutions is acidic, basic, or neutral: a. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=2.0 \times 10^{-5} \mathrm{M}\) b. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.4 \times 10^{-9} \mathrm{M}\) c. \(\left[\mathrm{OH}^{-}\right]=8.0 \times 10^{-3} \mathrm{M}\) d. \(\left[\mathrm{OH}^{-}\right]=3.5 \times 10^{-10} \mathrm{M}\)

Calculate the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) of each aqueous solution with the following [OH ]: a. coffee, \(1.0 \times 10^{-9} \mathrm{M}\) b. soap, \(1.0 \times 10^{-6} \mathrm{M}\) c. cleanser, \(2.0 \times 10^{-5} \mathrm{M}\) d. lemon juice, \(4.0 \times 10^{-13} \mathrm{M}\)

Calculate the \(\left[\mathrm{OH}^{-}\right]\) of each aqueous solution with the following \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) : a. stomach acid, \(4.0 \times 10^{-2} \mathrm{M}\) b. urine, \(5.0 \times 10^{-6} \mathrm{M}\) c. orange juice, \(2.0 \times 10^{-4} \mathrm{M}\) d. bile, \(7.9 \times 10^{-9} \mathrm{M}\)

Calculate the \(\left[\mathrm{OH}^{-}\right]\) of each aqueous solution with the following \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]:\) a. baking soda, \(1.0 \times 10^{-8} \mathrm{M}\) b. blood, \(4.2 \times 10^{-8} \mathrm{M}\) c. milk, \(5.0 \times 10^{-7} \mathrm{M}\) d. pancreatic juice, \(4.0 \times 10^{-9} \mathrm{M}\)

State whether each of the following solutions is acidic, basic, or neutral: a. blood plasma, \(\mathrm{pH} 7.38\) b. vinegar, \(\mathrm{pH} 2.8\) c. drain cleaner, \(\mathrm{pOH} 2.8\) d. coffee, \(\mathrm{pH} 5.52\) e. tomatoes, \(\mathrm{pH} 4.2\) f. chocolate cake, \(\mathrm{pH} 7.6\)

A solution with a pH of 3 is 10 times more acidic than a solution with \(\mathrm{pH} 4\). Explain.

A solution with a pH of 10 is 100 times more basic than a solution with \(\mathrm{pH}\) 8. Explain.

Calculate the pH of each solution given the following: a. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1 \times 10^{-4} \mathrm{M}\) b. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=3 \times 10^{-9} \mathrm{M}\) c. \(\left[\mathrm{OH}^{-}\right]=1 \times 10^{-5} \mathrm{M}\) d. \(\left[\mathrm{OH}^{-}\right]=2.5 \times 10^{-11} \mathrm{M}\) e. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=6.7 \times 10^{-8} \mathrm{M}\) f. \(\left[\mathrm{OH}^{-}\right]=8.2 \times 10^{-4} \mathrm{M}\)