A Ca(OH)2 solution has a pH of 8.0. [H3O+] = 1.0 x 10^-8 and [OH-] = 1.0 x 10^-6
Determine [Ca(OH)2].
To determine the concentration of Ca(OH)2, we can start by writing the equation for the dissociation of Ca(OH)2 in water.
Ca(OH)2 -> Ca2+ + 2OH-
From the equation, we can see that for every molecule of Ca(OH)2 that dissociates, we get one Ca2+ ion and two OH- ions.
Given that the concentration of OH- ions ([OH-]) is given as 1.0 x 10^-6, we know that the concentration of Ca2+ ions ([Ca2+]) will also be equal to 1.0 x 10^-6 M. This is because the concentration of Ca2+ ions is equal to half the concentration of OH- ions due to the stoichiometry of the dissociation reaction.
Now, we need to find the concentration of Ca(OH)2. Since Ca(OH)2 dissociates into Ca2+ and OH- ions in a 1:2 ratio, we can assume that twice the concentration of Ca(OH)2 will result in the same concentration of OH- ions.
Therefore, the concentration of Ca(OH)2 will be equal to 2 times the concentration of OH-:
[Ca(OH)2] = 2 x 1.0 x 10^-6 M
= 2.0 x 10^-6 M
So, the concentration of Ca(OH)2 in the given solution is 2.0 x 10^-6 M.
To determine the concentration of Ca(OH)2, we need to use the relationship between [OH-] and [Ca(OH)2]. The balanced equation for the dissociation of Ca(OH)2 is:
Ca(OH)2 ↔ Ca2+ + 2OH-
From the equation, we can see that for every Ca(OH)2 molecule that dissociates, it produces one Ca2+ ion and two OH- ions. Therefore, the concentration of Ca(OH)2 is half the concentration of OH-, since two OH- ions are produced for every Ca(OH)2 molecule.
Given that [OH-] = 1.0 x 10^-6, we can calculate [Ca(OH)2] as follows:
[Ca(OH)2] = 0.5 * [OH-]
= 0.5 * 1.0 x 10^-6
= 5.0 x 10^-7
Therefore, the concentration of Ca(OH)2 is 5.0 x 10^-7.
Ca(OH)2 WHAT? Ksp? perhaps?
........Ca(OH)2 ==> Ca^2+ + 2OH^-
Ksp = (Ca^2+)(OH^-)^2
(OH^-) = 1E-6 and (Ca&2+) = 1/2 that. Substitute into the Ksp expression and solve.