In a saturated solution of Al(OH)3 the concentration of OH^1- is 2.6 x 10^5 mol/L. The concentration of Al3+ in mol/L is what?
Al(OH)3 ==> Al^+3 + 3OH^-
If the concn of OH^- is 2.6 x 10^-5 mol/L, then the Al^+3 concn must be 1/3 of that. Note: I think you meant the concn OH^- was 2.6 x 10^-5 and NOT 2.6 x 10^5.
Well, isn't that an acidic situation for Aluminum Hydroxide (Al(OH)3)! It's like the OH^- ions are throwing a party, and the Al^3+ ions are feeling left out! Let's see if we can calculate their concentration and get them back together, shall we?
To figure out the concentration of Al^3+ ions, we need to remember that Aluminum Hydroxide dissociates in water according to the equation: Al(OH)3 ⇌ Al^3+ + 3OH^-.
Now, we know the concentration of OH^- ions is 2.6 x 10^5 mol/L. Since there's a 1:1 ratio between Al^3+ and OH^-, that means the concentration of Al^3+ is also 2.6 x 10^5 mol/L.
Voila! The concentration of Al^3+ ions in the saturated solution of Al(OH)3 is 2.6 x 10^5 mol/L. It looks like Aluminum finally got the invite to the OH^- party! Cheers!
To find the concentration of Al3+ in a saturated solution of Al(OH)3, we need to use the solubility product constant (Ksp) of Al(OH)3. The balanced equation for the dissociation of Al(OH)3 is:
Al(OH)3 ⇌ Al3+ + 3 OH^-
The expression for the solubility product constant is:
Ksp = [Al3+] * [OH^-]^3
Given that the concentration of OH^- is 2.6 x 10^5 mol/L, we can substitute this value into the Ksp expression:
Ksp = [Al3+] * (2.6 x 10^5)^3
To solve for [Al3+], we need to know the value of Ksp. The Ksp value for Al(OH)3 can be found in reference materials or given in the problem statement. Once we have that value, we can solve for [Al3+] by rearranging the equation.
To find the concentration of Al3+ in a saturated solution of Al(OH)3, we need to use the solubility product constant (Ksp) of Al(OH)3.
The balanced equation for the dissociation of Al(OH)3 is:
Al(OH)3 ⇌ Al3+ + 3OH^-
The Ksp expression for this equation is:
Ksp = [Al3+][OH^-]^3
We are given the concentration of OH^- in the saturated solution, which is 2.6 x 10^5 mol/L. Let's denote this concentration as [OH^-] = 2.6 x 10^5 mol/L.
Now, we can substitute the given concentration of OH^- into the Ksp expression:
Ksp = [Al3+](2.6 x 10^5 mol/L)^3
Since we want to find the concentration of Al3+ ([Al3+]), we can rearrange the equation:
[Al3+] = Ksp / (2.6 x 10^5 mol/L)^3
To calculate the concentration of Al3+, we need the value of the Ksp constant for Al(OH)3. Unfortunately, that value is not provided in the question.
If you have the value of Ksp for Al(OH)3, you can substitute it into the equation above along with the given concentration of OH^- to find the concentration of Al3+.