The pH of a 0.0050 M aqueous solution of calcium hydroxide is? Make sure to include all equations.
Ca(OH)2 ==> Ca^+2 + 2OH^-
0.0050M Ca(ON)2 = 2*0.005M OH^-.
pOH = -log(OH^-) = ??
pH + pOH = pKw = 14
Solve for pH.
Calculate the pH of a 0.0050M solution of slaked lime ca(OH)2
To determine the pH of a solution of calcium hydroxide, we need to consider the dissociation of calcium hydroxide.
The balanced equation for the dissociation of calcium hydroxide is:
Ca(OH)2(s) ⇌ Ca2+(aq) + 2OH-(aq)
Since calcium hydroxide is a strong electrolyte, it dissociates completely in water. This means that in a 0.0050 M solution of calcium hydroxide, the concentration of calcium ions (Ca2+) would also be 0.0050 M, and the concentration of hydroxide ions (OH-) would be twice that, or 0.010 M.
The pH of a solution is a measure of the concentration of hydrogen ions (H+). In this case, we can calculate the concentration of hydrogen ions by using the equation for the autoionization of water:
H2O(l) ⇌ H+(aq) + OH-(aq)
Since the concentration of hydroxide ions is known to be 0.010 M, the concentration of hydrogen ions (and therefore, the pH) can be determined by utilizing the equation Kw = [H+][OH-].
The value of Kw (the ion product of water) at 25°C is 1.0 x 10^-14. We can rearrange the equation to solve for [H+]:
[H+][OH-] = Kw
[H+] = Kw / [OH-] = (1.0 x 10^-14) / (0.010) = 1.0 x 10^-12 M
Since the concentration of hydrogen ions (H+) is 1.0 x 10^-12 M, the pH of the 0.0050 M aqueous solution of calcium hydroxide would be approximately 12.
To determine the pH of a solution of calcium hydroxide (Ca(OH)2), we need to consider the hydrolysis of the hydroxide ions (OH-) present in the solution.
The dissociation equation for calcium hydroxide is:
Ca(OH)2(s) ⇌ Ca2+(aq) + 2OH-(aq)
Since calcium hydroxide is a strong base, it will completely dissociate in water. So, for every 1 mole of Ca(OH)2, we get 1 mole of Ca2+ ions and 2 moles of OH- ions.
Since we are given the concentration of the solution (0.0050 M), we can assume that the concentration of hydroxide ions is also 0.0050 M. This is because the concentration of hydroxide ions is twice that of calcium hydroxide due to the stoichiometry of the dissolution equation.
Now, we can use the pOH formula to calculate the pOH of the solution:
pOH = -log10([OH-])
Substituting the value of [OH-] into the equation, we get:
pOH = -log10(0.0050) ≈ 2.30
Finally, to find the pH, we can use the relation:
pH + pOH = 14
So, the pH of the 0.0050 M solution of calcium hydroxide is approximately:
pH = 14 - 2.30 = 11.70