Calculate \(\left[\mathrm{H}^{+}\right]\) and \(\left[\mathrm{OH}^{-}\right]\) for each solution at \(25^{\circ} \mathrm{C}\). Identify each solution as neutral, acidic, or basic. a. \(\mathrm{pH}=7.40\) (the normal \(\mathrm{pH}\) of blood) b. \(\mathrm{pII}=15.3\) c. \(\mathrm{pH}=-1.0\) d. \(\mathrm{pH}=3.20\) e. \(\mathrm{pOH}=5.0\) f. \(\mathrm{pOH}=9.60\)

a. \(\left[\mathrm{H}^{+}\right] = 3.98 \times 10^{-8} \mathrm{M}\), \(\left[\mathrm{OH}^{-}\right] = 2.51 \times 10^{-7} \mathrm{M}\), basic. b. \(\left[\mathrm{H}^{+}\right] = 5.01 \times 10^{-16} \mathrm{M}\), \(\left[\mathrm{OH}^{-}\right] = 2 \times 10^2 \mathrm{M}\), basic. c. \(\left[\mathrm{H}^{+}\right] = 1 \times 10^1 \mathrm{M}\), \(\left[\mathrm{OH}^{-}\right] = 1 \times 10^{-15} \mathrm{M}\), acidic. d. \(\left[\mathrm{H}^{+}\right] = 6.31 \times 10^{-4} \mathrm{M}\), \(\left[\mathrm{OH}^{-}\right] = 1.58 \times 10^{-11} \mathrm{M}\), acidic. e. \(\left[\mathrm{H}^{+}\right] = 1 \times 10^{-9} \mathrm{M}\), \(\left[\mathrm{OH}^{-}\right] = 1 \times 10^{-5} \mathrm{M}\), basic. f. \(\left[\mathrm{H}^{+}\right] = 2.51 \times 10^{-5} \mathrm{M}\), \(\left[\mathrm{OH}^{-}\right] = 3.98 \times 10^{-10} \mathrm{M}\), acidic.