What is the concentration of H^+ and OH^- ions in a spring water with pH= 8.22 ? Is it acidic or basic?

To determine the concentration of $H^{+}$ and $OH^{-}$ ions in spring water with a pH of 8.22, we can use the following relationships:<br /><br />1. pH is defined as the negative logarithm of the hydrogen ion concentration:<br /> \[ \text{pH} = -\log[H^+] \]<br /><br />2. The product of the hydrogen ion concentration and the hydroxide ion concentration in water at 25°C (298 K) is always equal to the ion product constant for water, $K_w$, which is $1.0 \times 10^{-14}$:<br /> \[ [H^+][OH^-] = K_w = 1.0 \times 10^{-14} \]<br /><br />Given that the pH of the spring water is 8.22, we can calculate the hydrogen ion concentration as follows:<br />\[ [H^+] = 10^{-\text{pH}} = 10^{-8.22} \]<br /><br />Now, we can calculate the hydrogen ion concentration:<br />\[ [H^+] = 10^{-8.22} \approx 6.31 \times 10^{-9} \, \text{M} \]<br /><br />Next, we can find the hydroxide ion concentration using the ion product constant for water:<br />\[ [OH^-] = \frac{K_w}{[H^+]} = \frac{1.0 \times 10^{-14}}{6.31 \times 10^{-9}} \approx 1.58 \times 10^{-6} \, \text{M} \]<br /><br />Therefore, the concentration of $H^{+}$ ions in the spring water is approximately $6.31 \times 10^{-9} \, \text{M}$, and the concentration of $OH^{-}$ ions is approximately $1.58 \times 10^{-6} \, \text{M}$.<br /><br />Since the pH value is greater than 7, the spring water is considered basic.