Question

The pH of a solution in which OH negative concentration equals six. 9×10 to the -10 molarity

Answer 1

pH = 4.84

Step-by-step explanation:

To find the pH of a solution, we can use the formula:

pOH = -log[OH-]

Given:

[OH-] = 6.9 × 10^-10 M

First, let's calculate the pOH of the solution:

pOH = -log(6.9 × 10^-10)

pOH ≈ -(-9.16)

pOH ≈ 9.16

Now, to find the pH, we can use the relation:

pH + pOH = 14

pH = 14 - pOH

pH = 14 - 9.16

pH ≈ 4.84

Therefore, the pH of the solution is approximately 4.84.

Answer 2

The pH of a solution in which the concentration of hydroxide ions is 6.9 x 10^-10 M is approximately 4.84.

Step-by-step explanation:

The pH of a solution can be calculated from the concentration of hydroxide ions (OH-) using the relationship between pH, pOH, and the ion product constant for water (Kw). The pOH of a solution is defined as the negative logarithm (base 10) of the hydroxide ion concentration: pOH = -log[OH-]. The pH and pOH of a solution are related by the equation pH + pOH = 14. The ion product constant for water at 25°C is Kw = [H+][OH-] = 1.0 x 10^-14.

In this case, the concentration of hydroxide ions is given as [OH-] = 6.9 x 10^-10 M. We can use this value to calculate the pOH of the solution:

pOH = -log[OH-] = -log(6.9 x 10^-10) = 9.16

Then, we can use the relationship between pH and pOH to calculate the pH of the solution:

pH + pOH = 14

pH + 9.16 = 14

pH = 14 - 9.16

pH = 4.84

Therefore, the pH of a solution in which the concentration of hydroxide ions is 6.9 x 10^-10 M is approximately 4.84.