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What is the poh of a solution with oh 2.0 10-2?
1.70
Is the concentration of H plus in solution given the OH equals 2.54 x 10-4?
[H+] = Kw / [OH-] = 1.0*10-14 / 2.5*10-4 = 4.0*10-11 mol/L
What is the pH of a solution withOH equals 1 10-4?
-log[1 X 10^-4 M OH(-)] = 4 14 - 4 = 10 pH ----------------
Which of these solutions are acidic a solution with OH equals 2.5 10-9 H plus equals 1.2 10 -4 H plus equals 3.4 10-8 pH equals 4.5 OH equals 1.0 10-4?
solution with [OH-] = 2.5 x 10-9 , A solution with [H+] = 1.2 x 10-4, A solution with pH = 4.5
What is the h3O concentration in 0.45 m hcn ka of hcn 4.0 10-10?
HCN + H20 => CN- + H3O+ 0.45 X X Solve for X (4.0*10^-10) = x^2/0.45M x=1.34e-5= [OH] Find pOH= -log of the above number then 14-4.87=pH= 9.13
What is the pH of a solution with a oh of 3.31 00000000 M?
The pH of a solution can be calculated using the formula pH = 14 - pOH. Given that the pOH is 3.31, we can subtract this value from 14 to find the pH. In this case, the pH of the solution would be approximately 10.69.
If the pH of a solution is 4.0 what is the concentration of oh in the solution?
To find the concentration of hydroxide ions ([OH-]) in a solution when the pH is 4.0, you can use the formula pH + pOH = 14. Since the pH is 4.0, the pOH would be 14 - 4 = 10. To convert pOH to [OH-] concentration, use the formula [OH-] = 10^(-pOH). Thus, [OH-] = 10^(-10) = 1 x 10^(-10) M.
What is the OH- of a solution with pH 5.75?
The hydroxide ion concentration of a solution with pH 5.75 can be calculated using the formula [OH-] = 10^(-pOH). First, find the pOH by subtracting the pH from 14 (pOH = 14 - pH = 14 - 5.75 = 8.25). Then, calculate [OH-] = 10^(-8.25) ≈ 5.62 x 10^(-9) mol/L.
If the pH of a solution is 10.7, what would the pOH be?
The pOH is 6,4.
What is the pOH range of bases?
An acidic solution will have a pOH ranging from 7 to 14
What is the solution's pH and pOH?
To find the pH, calculate -log[H+] using the concentration of hydrogen ions [H+]. To find the pOH, calculate -log[OH-] using the concentration of hydroxide ions [OH-]. The pH and pOH are related by the equation pH + pOH = 14 for a neutral solution.
What is the pH of a 0.0110 M solution of Ba OH2?
The pH of a 0.0110 M solution of Ba(OH)2 can be calculated by finding the hydroxide ion concentration, which is double the concentration of the Ba(OH)2 solution. Therefore, [OH-] = 2 * 0.0110 M = 0.0220 M. From this, you can calculate the pOH using the formula -log[OH-], and then convert pOH to pH using the relation pH + pOH = 14.
The sum of pH plus pOH?
The sum of pH and pOH is always equal to 14 in a neutral solution at 25°C. This is because pH is a measure of the concentration of H+ ions in a solution while pOH is a measure of the concentration of OH- ions. In a neutral solution, the concentration of H+ ions is equal to the concentration of OH- ions, resulting in a sum of 14.
What is the pOH of a solution with OH 1.4 10 13?
The pOH of a solution with an OH- concentration of 1.4 x 10^-13 M is 1.85. This is calculated by taking the negative logarithm of the OH- concentration, which is -log(1.4 x 10^-13) = 12.85, then subtracting it from 14 to find the pOH: 14 - 12.85 = 1.85.
A solution has H plus equals 6.2 x 10-3 What is the pOH of this solution?
7.8
OH- of a solution which has a pH equals 10.95?
The hydroxide ion concentration of a solution with a pH of 10.95 is 1.26 x 10^-11 mol/L. This can be calculated using the formula [OH-] = 10^(-pH).
What is the hydroxide-ion concentrations for solutions with 6.00 pH values?
The hydroxide-ion concentration for a solution with a pH of 6.00 is 1 x 10^-8 M. This can be calculated using the equation: [OH-] = 10^-(14 - pH), where 14 is the sum of the pH and pOH of a solution.
