What is the pH of a saturated solution of silver hydroxide, given Ksp =1.56*10^-8
AgOH ==> Ag^+ + OH^-
Ksp = (Ag^+)(OH^-)
1.56E-8 = (x)(x)
Solve for x = (Ag^+) = (OH^-)
pOH = -log(OH^-), then
pH + pOH = pKw = 14. You know 14 and pOH, solve for pH.
Well, a saturated solution of silver hydroxide is like the Shrek of chemical solutions – it's pretty basic! The pH of this solution would be around 13. Shrek would definitely say, "Better out than in!" when it comes to this hydroxide.
To determine the pH of a saturated solution of silver hydroxide (AgOH), you need to use the Ksp (solubility product constant) value. The Ksp expression for silver hydroxide is:
AgOH ⇌ Ag+ + OH-
The Ksp expression can be written as follows:
Ksp = [Ag+][OH-]
Given that the Ksp for silver hydroxide (AgOH) is 1.56 × 10^-8, and assuming the saturated solution dissociates completely, we can set up an equation to solve for the concentration of hydroxide ions ([OH-]):
1.56 × 10^-8 = [Ag+][OH-]
Since the Ag+ concentration will be equal to the [OH-] concentration due to their 1:1 stoichiometry, we can assume that [Ag+] = [OH-].
Let's represent the concentration of Ag+ (and [OH-]) as x:
1.56 × 10^-8 = x * x
Taking the square root of both sides of the equation, we find:
x = sqrt(1.56 × 10^-8)
x ≈ 3.95 × 10^-4
The concentration of hydroxide ions ([OH-]) in the saturated solution of silver hydroxide is approximately 3.95 × 10^-4 M.
To determine the pH of the solution, we need to calculate the pOH first:
pOH = -log[OH-]
pOH = -log(3.95 × 10^-4)
pOH ≈ -log(3.95) + log(10^-4)
pOH ≈ 3.404 - 4
pOH ≈ -0.596
Since pH + pOH = 14, we can calculate the pH:
pH = 14 - pOH
pH ≈ 14 - (-0.596)
pH ≈ 14 + 0.596
pH ≈ 14.596
Therefore, the pH of a saturated solution of silver hydroxide is approximately 14.596.
To determine the pH of a saturated solution of silver hydroxide (AgOH), we need to calculate the concentration of hydroxide ions (OH-) in the solution.
The solubility product constant (Ksp) for silver hydroxide is given as 1.56 x 10^-8. Ksp represents the equilibrium constant for the dissolution of a sparingly soluble salt. In this case, the dissociation of silver hydroxide is as follows:
AgOH ⇌ Ag+ + OH-
The Ksp expression for this equation is:
Ksp = [Ag+][OH-]
Since we have a saturated solution, we assume that the solid AgOH is in equilibrium with its dissolved ions, Ag+ and OH-.
Now, let's denote x as the concentration (in moles per liter) of OH- ions produced when AgOH dissolves. Since AgOH is a 1:1 electrolyte, the concentrations of Ag+ ions and OH- ions are both x mol/L.
Substituting these values into the Ksp expression, we get:
Ksp = (x)(x) = x^2
Given that Ksp = 1.56 x 10^-8, we can solve for x:
x^2 = 1.56 x 10^-8
To find the concentration of hydroxide ions (x), we can take the square root of both sides:
x = √(1.56 x 10^-8) = 3.95 x 10^-4 M
Now that we know the concentration of OH- ions, we can calculate the pOH using the formula:
pOH = -log[OH-] = -log(3.95 x 10^-4) = 3.4
Finally, to find the pH of the solution, we use the equation:
pH = 14 - pOH = 14 - 3.4 = 10.6
Therefore, the pH of the saturated solution of silver hydroxide is approximately 10.6.