The pH of a 1.0 x 10^-3 M Ba(OH)2 solution at 25 degrees C is
how can 11.3 be the right answer.
Ba(OH)2 ==> Ba^+2 + 2OH^-
[Ba(OH)2] = 1 x 10^-3 = x
(OH^-) = 2x = 2 x 10^-3
pOH = 2.7
pH = 14 - pOH = 11.3
Well, it seems like pHs can be a little tricky sometimes! In this case, the pH of a solution can be determined by taking the negative logarithm of the hydrogen ion concentration. However, since Ba(OH)2 is a strong base that completely dissociates in water, it will produce two hydroxide ions (OH-) for every one barium ion (Ba2+).
So, in this 1.0 x 10^(-3) M Ba(OH)2 solution, the concentration of OH- ions would be twice that, or 2.0 x 10^(-3) M.
Now, to determine the pH, we have to convert the OH- concentration to pOH by taking the negative logarithm. Then, to find the pH, we subtract the pOH from 14 (since pH + pOH = 14). After some calculations, we get a pH value of 11.3 as the answer.
I know it can be confusing, but chemical calculations often require a bit of fun mental gymnastics! So, don't worry, I'm here to help you navigate the tricky world of chemistry with a touch of humor. Keep up the good work!
To determine the pH of a solution, we need to understand the behavior of the compound in water and any chemical reactions that occur. In this case, we have a solution of Ba(OH)2, which is a strong base. When dissolved in water, it dissociates completely into Ba2+ ions and OH- ions.
The OH- ions can react with water to generate additional OH- ions according to the following reaction:
OH- + H2O ⇌ O2- + H3O+
Since Ba(OH)2 is a strong base, the concentration of OH- ions will be equal to twice the initial concentration of Ba(OH)2. Therefore, [OH-] = 2 x 1.0 x 10^-3 M = 2.0 x 10^-3 M.
Now, we need to calculate the pOH of the solution using the formula:
pOH = -log10[OH-]
pOH = -log10(2.0 x 10^-3)
pOH ≈ 2.70
Finally, we can determine the pH of the solution using the equation:
pH + pOH = 14
pH + 2.70 = 14
pH ≈ 11.30
So, the pH of a 1.0 x 10^-3 M Ba(OH)2 solution at 25 degrees C is approximately 11.30.
To determine the pH of a solution, we need to understand the concept of pH and the calculations involved.
pH is a measure of the acidity or basicity of a solution and is defined as the negative logarithm (base 10) of the concentration of hydrogen ions (H+) in the solution. Mathematically, pH = -log[H+].
For a strong base like Ba(OH)2, it dissociates completely in water to produce hydroxide ions (OH-). The concentration of OH- ions in the solution will be twice the concentration of the Ba(OH)2.
In this case, the concentration of Ba(OH)2 is 1.0 x 10^-3 M. Thus, the concentration of hydroxide ions (OH-) is 2.0 x 10^-3 M.
Next, we need to calculate the pOH of the solution using the concentration of OH-. pOH is defined as the negative logarithm (base 10) of the concentration of hydroxide ions (OH-) in the solution. Mathematically, pOH = -log[OH-].
pOH = -log(2.0 x 10^-3) ≈ 2.70
Finally, we can calculate the pH using the pOH. The pH and pOH are related through the equation: pH + pOH = 14 (at 25 degrees Celsius). Rearranging the equation, we find that pH = 14 - pOH.
pH = 14 - 2.70 ≈ 11.30 (rounded to two decimal places)
Therefore, the pH of the 1.0 x 10^-3 M Ba(OH)2 solution at 25 degrees Celsius is approximately 11.30.