1. Find the pH of a solution whose [H3O+] is 9.5 X 10^ -8 M.
2. What is the [H3O+] concentration of a solution with a pH of 5.45?
3. What is the pOH of a solution with a [OH -] concentration of 2.97 X 10^ -10 M?
1)
pH = -log(H^+)
2)
pH = -log(H^+)
3)
pOH = -log(OH^-)
is this right?
-log(concentration of h3o+ or h+)
ph= -log(9.5*10^-8)
1) 7.022
right. Very good. But I would round it to 7.02. You have two significant figures in 9.5E-8 so you are allowed just two in 7.02 (since it's a log the 7 doesn't count as a significant figures).
1. Oh, that's an acidic situation! To find the pH, just take the negative logarithm of the [H3O+] concentration. So in this case, the pH would be approximately 7.0 minus log(9.5 × 10^-8). Grab your calculator and let's find out!
2. Ah, the old pH game. To find the [H3O+] concentration, you'll need to flip the pH like a pancake. So, for a pH of 5.45, the [H3O+] concentration would be 10 raised to the power of -5.45. Get your calculator ready to crunch those numbers!
3. Oh, the pOH roller coaster! To find the pOH, you'll want to take the negative logarithm of the [OH-] concentration. So, for a [OH-] concentration of 2.97 × 10^-10 M, the pOH would be approximately -log(2.97 × 10^-10). It's time to dive into the world of logarithms, my friend!
1. To find the pH of a solution, you need to know the concentration of the hydronium ion, which is represented as [H3O+]. The pH is calculated using the mathematical formula pH = -log[H3O+].
In this case, the [H3O+] is given as 9.5 X 10^-8 M. Using the formula, you can plug in this value to find the pH:
pH = -log(9.5 X 10^-8)
= -log(9.5) + log(10^-8) [using logarithmic properties]
= -log(9.5) - 8 [log(10^-8) = -8 using logarithmic properties]
≈ -(-7.022) - 8 [taking logarithm of 9.5 to four decimal places]
≈ 7.022 - 8
≈ -0.978
Therefore, the pH of the solution is approximately -0.978.
2. To find the concentration of the hydronium ion ([H3O+]) from the given pH, you can use the reverse of the formula mentioned above.
In this case, the pH is given as 5.45. To find the [H3O+] concentration, we can use the formula [H3O+] = 10^(-pH):
[H3O+] = 10^(-5.45)
= 3.55 x 10^(-6)
Therefore, the [H3O+] concentration of the solution with a pH of 5.45 is approximately 3.55 x 10^(-6) M.
3. The pOH of a solution can be calculated using the formula pOH = -log[OH-].
In this case, the [OH-] concentration is given as 2.97 X 10^ -10 M. To find the pOH, we can plug this value into the formula:
pOH = -log(2.97 X 10^ -10)
= -log(2.97) + log(10^ -10) [using logarithmic properties]
= -log(2.97) - 10 [log(10^ -10) = -10 using logarithmic properties]
≈ -(-9.526) - 10 [taking logarithm of 2.97 to three decimal places]
≈ 9.526 - 10
≈ -0.474
Therefore, the pOH of the solution with a [OH-] concentration of 2.97 X 10^ -10 M is approximately -0.474.