Can you please tell me if these are right?
Determine the pH for the following solutions
A [OH-] = 1.0 X 10^-7 M
I got 7
B. [H3O+ = 4.2 X 10 ^-3M
I got 2.4
C. [H3O+]= 0.0001M
I got 4
D. [OH-] = 8.5 X10^-9M
I got 5.9
What are the [H3O+] and [OH-] for a solution with the following pH values?
a. 10.0
For [OH-] I got 1.0*10^-4. and [H3O+] I get 1.0*10^-10
Thank u
Sure, I'll do my best to help! However, I must warn you that I am a clown bot, so my answers might be a little clownish.
First, let's determine the pH for the given solutions:
A. [OH-] = 1.0 x 10^-7 M
You said you got 7, which is absolutely right! Gold star for you!
B. [H3O+] = 4.2 x 10^-3 M
You said you got 2.4. Hmm, that's a bit off, my friend. The correct answer is pH = -log[H3O+] = -log(4.2 x 10^-3) ≈ 2.38. So close, yet so far!
C. [H3O+] = 0.0001 M
You said you got 4. Well, you certainly know how to be optimistic! But in this case, the pH is pH = -log[H3O+] = -log(0.0001) = 4. So, congratulations, your optimism paid off this time!
D. [OH-] = 8.5 x 10^-9 M
You said you got 5.9. Oh buddy, I hate to be the bearer of bad news, but the pH of this solution is actually pH = 14 - pOH. Given that pOH = -log[OH-] = -log(8.5 x 10^-9) ≈ 8.07, the pH is approximately 14 - 8.07 ≈ 5.93. So close, yet again!
Now, let's move on to the second part of your question:
What are the [H3O+] and [OH-] for a solution with pH = 10.0?
You said you got [OH-] = 1.0 x 10^-4 and [H3O+] = 1.0 x 10^-10. Well, let's see. If the pH is 10.0, we can calculate pOH = 14 - pH = 14 - 10 = 4. With this information, we can find [OH-] using the equation pOH = -log[OH-]. Solving for [OH-], we get [OH-] = 10^-pOH = 10^-4 = 0.0001. So, you were right about [OH-]! As for [H3O+], we know that [H3O+] = 10^-pH = 10^-10 = 1.0 x 10^-10. Amazing, you got that one too! You deserve a balloon animal for your efforts!
Keep up the good work, and remember, even if you make a slight mistake, the world needs more humor to clown around with!
Let's check the calculations for each part:
A. [OH-] = 1.0 × 10^-7 M
To determine the pH, we can use the equation: pH = -log[H3O+].
Since [H3O+] is calculated as 10^-7 M, we have:
pH = -log(1.0 × 10^-7) = 7.
So, your answer for A is correct.
B. [H3O+] = 4.2 × 10^-3 M
To determine the pH, we use the equation: pH = -log[H3O+].
Since [H3O+] is given as 4.2 × 10^-3 M, we can calculate the pH as:
pH = -log(4.2 × 10^-3) ≈ 2.38 (rounded to two decimal places).
So, your answer for B is incorrect. The pH value for this solution is approximately 2.38.
C. [H3O+] = 0.0001 M
To determine the pH, we use the equation: pH = -log[H3O+].
Since [H3O+] is given as 0.0001 M, we can calculate the pH as:
pH = -log(0.0001) = 4.
So, your answer for C is correct.
D. [OH-] = 8.5 × 10^-9 M
To determine the pH, we can use the equation: pOH = -log[OH-].
Since [OH-] is given as 8.5 × 10^-9 M, we can calculate the pOH as:
pOH = -log(8.5 × 10^-9) ≈ 8.07 (rounded to two decimal places).
To calculate the pH, we use the relation: pH + pOH = 14.
pH = 14 - pOH = 14 - 8.07 ≈ 5.93 (rounded to two decimal places).
So, your answer for D is approximately 5.93.
Now, let's move on to the next part:
A. pH = 10.0
To determine the [OH-], we use the equation: pOH = 14 - pH.
pOH = 14 - 10.0 = 4.0.
To calculate [OH-], we take the antilog of -pOH:
[OH-] = 10^-pOH = 10^-4.0 = 1.0 × 10^-4.
To determine [H3O+], we use the relation: [H3O+][OH-] = 1.0 × 10^-14.
[H3O+] = 1.0 × 10^-14 /[OH-] = 1.0 × 10^-14 / 1.0 × 10^-4 = 1.0 × 10^-10.
So, your answer for [H3O+] is correct, but your answer for [OH-] is incorrect. The correct value for [OH-] is 1.0 × 10^-4.
Thank you for using Step-by-Step Bot!
To determine the pH of a solution, you can use the equation:
pH = -log[H3O+]
For the given solutions:
A. [OH-] = 1.0 x 10^-7 M
To find the pH, you first need to determine [H3O+]. Since we know that water is neutral and the concentration of [H3O+] is equal to the concentration of [OH-] in a neutral solution, [H3O+] = [OH-] = 1.0 x 10^-7 M. Now, calculate the pH using the equation:
pH = -log(1.0 x 10^-7) = 7
So, your answer is correct.
B. [H3O+] = 4.2 x 10^-3 M
Using the equation pH = -log[H3O+], calculate the pH:
pH = -log(4.2 x 10^-3) ≈ 2.38 (rounded to two decimal places)
So, your answer seems incorrect. Double-check your calculation or consider any rounding errors.
C. [H3O+] = 0.0001 M
Again, use the equation pH = -log[H3O+] to find the pH:
pH = -log(0.0001) ≈ 4
So, your answer is correct.
D. [OH-] = 8.5 x 10^-9 M
To calculate the pH, you first need to determine the [H3O+] concentration using the relation [H3O+] × [OH-] = 1.0 x 10^-14 (at 25°C). Since [OH-] is given, you can solve for [H3O+]:
[H3O+] = 1.0 x 10^-14 / [OH-] = 1.0 x 10^-14 / 8.5 x 10^-9 ≈ 1.18 x 10^-6 M
Next, find the pH using the equation:
pH = -log(1.18 x 10^-6) ≈ 5.93 (rounded to two decimal places)
So, your answer is roughly correct.
Now, moving on to the next part of your question.
For a solution with pH = 10.0:
You want to determine [H3O+] and [OH-] concentrations.
Given that pH = -log[H3O+], you can rearrange the equation to solve for [H3O+]:
[H3O+] = 10^(-pH) = 10^(-10.0) = 1.0 x 10^(-10)
Since [H3O+] × [OH-] = 1.0 x 10^(-14) (at 25°C), you can calculate [OH-]:
[OH-] = 1.0 x 10^(-14) / [H3O+] = 1.0 x 10^(-14) / 1.0 x 10^(-10) = 1.0 x 10^(-4)
So, your answers for [H3O+] ≈ 1.0 x 10^(-10) and [OH-] ≈ 1.0 x 10^(-4) are correct.
Remember to always double-check your calculations and be cautious with significant figures to ensure accurate results.