How many mg/L of [Mg+2] will remain in a solution that has a hydroxide ion concentration of 0.015 M. The solubility product (Ksp) , at 25 degrees C, for magnesium hydroxide is 1.82 x 10-11. In addition, calculate the pH of the solution.
Solution
Given Data
Hydroxide ion concentration of 0.015 M
The solubility product (Ksp) , at 25 degrees C, for magnesium hydroxide is 1.82 x 10-11.
By using the K sp expression to calculate the [Mg 2+ ]:
K sp = [Mg 2+ ] [OH-] 2
1.82 x 10¯ 11 = (x) (0.015) 2
x = 1.82 * 10¯ 11 / 0.015
= 121.34 * 10¯ 11 M
For to the pH of a solution all we need to know the concentration of the hydronium ion in moles per liter
The pH is then calculated using the expression:
pH = - log [H 3 O + ].
= 1.88
.
How many mg-L of -Mg+2- will remain in a solution that has a hydroxide.docx
1. How many mg/L of [Mg+2] will remain in a solution that has a hydroxide ion concentration of
0.015 M. The solubility product (Ksp) , at 25 degrees C, for magnesium hydroxide is 1.82 x 10-
11. In addition, calculate the pH of the solution.
Solution
Given Data
Hydroxide ion concentration of 0.015 M
The solubility product (Ksp) , at 25 degrees C, for magnesium hydroxide is 1.82 x 10-11.
By using the K sp expression to calculate the [Mg 2+
]:
K sp = [Mg 2+
] [OH-] 2
1.82 x 10¯ 11
= (x) (0.015) 2
x = 1.82 * 10¯ 11
/ 0.015
= 121.34 * 10¯ 11
M
For to the pH of a solution all we need to know the concentration of the hydronium ion in moles
per liter
The pH is then calculated using the expression:
pH = - log [H 3 O +
].
= 1.88
![How many mg/L of [Mg+2] will remain in a solution that has a hydroxide ion concentration of
0.015 M. The solubility product (Ksp) , at 25 degrees C, for magnesium hydroxide is 1.82 x 10-
11. In addition, calculate the pH of the solution.
Solution
Given Data
Hydroxide ion concentration of 0.015 M
The solubility product (Ksp) , at 25 degrees C, for magnesium hydroxide is 1.82 x 10-11.
By using the K sp expression to calculate the [Mg 2+
]:
K sp = [Mg 2+
] [OH-] 2
1.82 x 10¯ 11
= (x) (0.015) 2
x = 1.82 * 10¯ 11
/ 0.015
= 121.34 * 10¯ 11
M
For to the pH of a solution all we need to know the concentration of the hydronium ion in moles
per liter
The pH is then calculated using the expression:
pH = - log [H 3 O +
].
= 1.88](https://image.slidesharecdn.com/howmanymg-lof-mg2-willremaininasolutionthathasahydroxide-230128055326-6fe34eae/85/How-many-mg-L-of-Mg-2-will-remain-in-a-solution-that-has-a-hydroxide-docx-1-320.jpg)
