What are the (a) H+ ion concentration, (b) pH, (c) OH" ion
concentration, and (d) pOH of a 0.001 M solution of HC1?
HCl is a strong acid and ionizes 100%.
HCl ==> H^+ + Cl^-
Therefore, 0.001 m HCl will give you 0.001 M H^+.
pH = -log (H^+)
pH + pOH = 14. Solve for pOH.
pOH = -log (OH^-)
To find the (a) H+ ion concentration, (b) pH, (c) OH- ion concentration, and (d) pOH of a 0.001 M solution of HCl, we can use the concept of acidity, pH, and pOH.
(a) H+ ion concentration:
The HCl solution fully dissociates in water to form H+ ions and Cl- ions. Since the concentration of HCl is 0.001 M, the concentration of H+ ions will also be 0.001 M.
(b) pH:
The pH of a solution is a measure of its acidity. It is defined as the negative logarithm (base 10) of the H+ ion concentration. To find the pH of the HCl solution, we calculate -log(0.001) = 3.
(c) OH- ion concentration:
In an aqueous solution, the concentration of H+ ions and OH- ions are related by the equation [H+]*[OH-] = 1x10^-14. Since the concentration of H+ ions in the HCl solution is 0.001 M, we can rearrange the equation to find the OH- ion concentration. Therefore, [OH-] = 1x10^-14 / [H+]. Plugging in the values, we find [OH-] = 1x10^-14 / 0.001 = 1x10^-11 M.
(d) pOH:
The pOH of a solution is the negative logarithm (base 10) of the OH- ion concentration. To find the pOH of the HCl solution, we calculate -log(1x10^-11) = 11.
To summarize:
(a) H+ ion concentration = 0.001 M
(b) pH = 3
(c) OH- ion concentration = 1x10^-11 M
(d) pOH = 11