What is the [H3O+] of a solution with a pOH equal to 5.45?
pH + pOH = 14
Well, if the pOH is 5.45, that means the solution is pretty basic. To find the [H3O+], we can use the equation pH + pOH = 14. So if the pOH is 5.45, that means the pH would be a clown-friendly 8.55. And since pH is the negative logarithm of [H3O+], we can take that clown car for a spin and calculate that the [H3O+] would be approximately 2.98 x 10⁻⁹ M.
To determine the [H3O+] of a solution with a given pOH value, you can use the relationship:
pH + pOH = 14
Since we know that the pOH is 5.45, we can substitute this value into the equation:
pH + 5.45 = 14
Next, we solve for pH:
pH = 14 - 5.45
pH = 8.55
Finally, to find the [H3O+], we can use the equation:
[H3O+] = 10^(-pH)
[H3O+] = 10^(-8.55)
Calculating this using a calculator, the [H3O+] is approximately 2.98 x 10^(-9) M.
Thus, the [H3O+] of the solution is approximately 2.98 x 10^(-9) M.
To find the [H3O+] (also known as hydronium ion concentration) of a solution with a given pOH value, you can use the equation:
pOH = -log10[OH-]
In this case, the pOH is given as 5.45. To find the [OH-] concentration, we need to convert the pOH into a numerical value by taking the antilog (inverse log) of -5.45:
[OH-] = 10^(-pOH)
Now, to find the [H3O+] concentration, we can use the fact that in neutral water, the product of [H3O+] and [OH-] is equal to 1x10^(-14) at 25 degrees Celsius. Therefore:
[H3O+] = 1x10^(-14) / [OH-]
So, substituting the value for [OH-] that we just calculated, we can find the [H3O+] concentration:
[H3O+] = 1x10^(-14) / 10^(-5.45)
Simplifying this expression, we subtract the exponents:
[H3O+] = 1x10^(-14 + 5.45)
[H3O+] = 1x10^(-8.55)
Therefore, the [H3O+] of the solution with a pOH equal to 5.45 is approximately 3.16x10^(-9) M.