The pOH is 5,23.
pH and pOH are a measure of the concentration of the hydronium ions and hydroxyl ions respectively in the solution. pH = -log[H+] pOH = -log[OH-] and they are related: pH + pOH = 14
pH + pOH = 14 If the pH is 3.4, the pOH is 10.6
7.8
pH and pOH are both logarithmic scales measuring the acidity (or basicness) of a solution. pH is based on the amount of H+ (hydrogen ions), and pOH is based on the amount of OH- (hydroxide ions) in the solution. You can calculate pH if you know the H+ activity: pH = - log10 (H+) pOH is calculated the same way, except with OH- instead of the H+ ions. pOH is also equal to 14 - pH. This is because the pH and pOH scales go from 0 to 14. A solution that is very acidic will have a low pH number and a high pOH number. Conversely, a very basic solution will have a low pOH and a high pH. Water is a neutral solution and has a pH and pOH of 7, which is in the middle.
pOH = -log(10)[OH^-] pOH = -log(10) [ 48. x 10^-2] pOH = - (-1.31875...) pOH = 1.31875... pH = 14 - pOH pH = 14 - 1.31875... pH = 12.68124... pH = 12.68
7.5
pH and pOH are a measure of the concentration of the hydronium ions and hydroxyl ions respectively in the solution. pH = -log[H+] pOH = -log[OH-] and they are related: pH + pOH = 14
pH + pOH = 14 If the pH is 3.4, the pOH is 10.6
1.79x10^-14 M
5.6
7.8
pH and pOH are both logarithmic scales measuring the acidity (or basicness) of a solution. pH is based on the amount of H+ (hydrogen ions), and pOH is based on the amount of OH- (hydroxide ions) in the solution. You can calculate pH if you know the H+ activity: pH = - log10 (H+) pOH is calculated the same way, except with OH- instead of the H+ ions. pOH is also equal to 14 - pH. This is because the pH and pOH scales go from 0 to 14. A solution that is very acidic will have a low pH number and a high pOH number. Conversely, a very basic solution will have a low pOH and a high pH. Water is a neutral solution and has a pH and pOH of 7, which is in the middle.
pOH = -log(10)[OH^-] pOH = -log(10) [ 48. x 10^-2] pOH = - (-1.31875...) pOH = 1.31875... pH = 14 - pOH pH = 14 - 1.31875... pH = 12.68124... pH = 12.68
10.01 is wrong, that's the pH i need the H+ concentration thanks again
No, pOH is the opposite of pH. They are both based on molarity "amount of solute per unit volume of solution". pH stands for "power of H+ ions in solution" (H+ = (hydrogen ion) pOH stands for "power of OH- ions in solution" (OH- = hydroxide ion) Hope that helps, -Coda
pH = - log([H+]) , pOH = - log([OH-] , pH + pOH = 14 [X] = concentration of X
We can subtract pOH from 14, using the formula pH + pOH = 14. This is only true at 14 degrees Celsius.