The pH of an NH3 and NH4Cl solution is 9.20. What is the [H3O+]
pH = - log(H3O^+)
Well, it seems like we're dealing with some chemistry here! To find the [H3O+] concentration, we can use the equation:
pH = -log[H3O+]
To solve for [H3O+], we need to rearrange the equation a little:
[H3O+] = 10^(-pH)
Substituting the given pH value of 9.20 into the equation:
[H3O+] = 10^(-9.20)
Now, let me pull out my handy-dandy calculator...
*presses buttons*
And the result is 0.00000000125893! Phew, that's quite a long number. So, the [H3O+] concentration is approximately 1.26 x 10^(-9) moles per liter.
To calculate the [H3O+] (concentration of hydronium ions) in a solution, you can use the formula:
pH = -log[H3O+]
Since you have the pH value of 9.20, you can rearrange the formula and solve for [H3O+]. Using the equation:
[H3O+] = 10^(-pH)
Substituting in the given pH value:
[H3O+] = 10^(-9.20)
Calculating this value:
[H3O+] = 6.31 x 10^(-10)
Therefore, the concentration of hydronium ions, [H3O+], in the solution is approximately 6.31 x 10^(-10) mol/L.
To find the [H3O+] (concentration of hydronium ions) in the solution, we can use the definition of pH. The pH is defined as the negative logarithm (base 10) of the hydronium ion concentration:
pH = -log[H3O+]
In this case, the pH is given as 9.20. We can rearrange the equation to solve for [H3O+]:
[H3O+] = 10^(-pH)
Substituting the given value:
[H3O+] = 10^(-9.20)
Calculating this value using a calculator, we find that [H3O+] is approximately 1.58 x 10^(-10) mol/L.