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First, since NaOH is a base you have to find the pOH first
so you use the equation -> pOH = -log[NaOH]
pOH = -log[NaOH]
= -log[0.0111]
pOH = 1.955
Then you use this equation -> 14 = pH + pOH to find the pH
14 = pH + pOH
pH = 14 - pOH
= 14 - 1.955
pH = 12.045
and that makes it basic
Hope that helped. ^_^
What else can I help you with?
What is the pH and pOH of a 2.34x10-5 NaOH solution?
The pH of a 2.34x10^-5 NaOH solution is 12.33 (calculated as -log[OH^-]). The pOH of the same solution is 1.67 (calculated as -log[NaOH]).
How do you calculate the pH of a 0.001 M NaOH solution?
To calculate the pH of a 0.001 M NaOH solution, you can use the formula pH = 14 - pOH. Since NaOH is a strong base that completely dissociates in water, the pOH can be directly calculated as -log(0.001) = 3. Thus, the pH of the solution would be 14 - 3 = 11.
What if the pH of a solution is 7.6 what is the pOH?
The pOH is 6,4.
PH of 1.0 M NaOH?
The pH of a 1.0 M NaOH solution is approximately 14. NaOH is a strong base that dissociates completely in water to produce hydroxide ions, resulting in a highly alkaline solution with a pH at the upper end of the scale.
A solution of HCl has H 2.5 x 10-5 What is the pOH of this solution?
pH + pOH = 14 If the pH is 3.4, the pOH is 10.6
What is the pH and pOH of a 2.34x10-5 NaOH solution?
The pH of a 2.34x10^-5 NaOH solution is 12.33 (calculated as -log[OH^-]). The pOH of the same solution is 1.67 (calculated as -log[NaOH]).
A solution of NaOH has OH- 1.9 x 10-6 What is the pOH of this solution?
5.7
What is the pH of a 0.6M NAOH solution?
To find the pH of a 0.6 M NaOH solution, first, note that NaOH is a strong base that dissociates completely in water. The concentration of hydroxide ions (OH⁻) will also be 0.6 M. The pOH can be calculated as -log(0.6), which is approximately 0.22. Since pH + pOH = 14, the pH of the solution is about 13.78.
What is the pOH of a solution with OH- 1.410-13?
To find the pOH of a solution, you can use the formula pOH = -log[OH⁻]. Given that [OH⁻] = 1.41 × 10⁻¹³, calculate the pOH: pOH = -log(1.41 × 10⁻¹³) ≈ 12.85. Therefore, the pOH of the solution is approximately 12.85.
How do you calculate the pH of a 0.001 M NaOH solution?
To calculate the pH of a 0.001 M NaOH solution, you can use the formula pH = 14 - pOH. Since NaOH is a strong base that completely dissociates in water, the pOH can be directly calculated as -log(0.001) = 3. Thus, the pH of the solution would be 14 - 3 = 11.
What if the pH of a solution is 7.6 what is the pOH?
The pOH is 6,4.
PH of 1.0 M NaOH?
The pH of a 1.0 M NaOH solution is approximately 14. NaOH is a strong base that dissociates completely in water to produce hydroxide ions, resulting in a highly alkaline solution with a pH at the upper end of the scale.
A solution has 0.000001 moles of hydroxide ions per liter - what is the pH of the solution?
The pOH of the solution would be 6. If you subtract the pOH from 14 (pH + pOH = 14), you would find that the pH of the solution is 8.
A solution of HCl has H 2.5 x 10-5 What is the pOH of this solution?
pH + pOH = 14 If the pH is 3.4, the pOH is 10.6
How much NaOH is needed to prepare 546 mL of solution with a pH of 10.00?
To prepare a solution with a pH of 10.00, you will need to calculate the concentration of hydroxide ions. Once you have this concentration, you can determine the amount of NaOH needed to achieve this pH in 546 mL of solution.
What is the pH of a 1 millimolar NaOH soluiton?
The pH of a 1 millimolar NaOH solution is approximately 11. The concentration of a 1 millimolar solution is 0.001 mol/L, and NaOH is a strong base that completely dissociates in water to produce hydroxide ions, leading to a basic pH.
If the pH solution is 6.2 what would the pOH be?
To find the pOH, subtract the pH value from 14. In this case, for a pH of 6.2, the pOH would be 7.8.
