What is the pH of a solution made of 0.1 M acetic acid and 0.1 M potassium acetate to which 0.001 mol of KOH has been added?
Ka = 1.8 x 10-5
a)pH = 8.92
b)pH = 4.74
c)pH = 11.55
d)pH = 4.46
e)pH = 4.73
I tried subtracting .001 moles from .1 moles from acetic acid and adding .001 moles to potassium acetate (I assumed that there was 1 liter of solution) and when I use the Henderson-Hasselbalch equationI get 4.74. The practice quiz is marking it wrong, so I'm not sure what I'm doing wrong...
Ka = 1.8 x 10-5
a)pH = 8.92
b)pH = 4.74
c)pH = 11.55
d)pH = 4.46
e)pH = 4.73
I tried subtracting .001 moles from .1 moles from acetic acid and adding .001 moles to potassium acetate (I assumed that there was 1 liter of solution) and when I use the Henderson-Hasselbalch equationI get 4.74. The practice quiz is marking it wrong, so I'm not sure what I'm doing wrong...
Here's what I got.
Now, when you have equal concentrations of the weak acid and of the conjugate base, you get
and
So before adding the potassium hydroxide, your buffer has
and
Now, adding the strong base will cause the concentration of the weak acid to decrease and the concentration of the conjugate base to increase.
So after you add the potassium hydroxide, you have
This means that
and so
which gets you
This time, the strong acid would consume some of the conjugate base and produce weak acid, so
This means that
and so
which gets you
And so
As predicted, we have
By signing up, you agree to our Terms of Service and Privacy Policy
The pH of the solution would be approximately 4.74.
By signing up, you agree to our Terms of Service and Privacy Policy
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- Could a buffered solution be made by mixing aqueous solutions of HCl and NaOH? Explain. Why isn't a mixture of a strong acid and its conjugate base considered a buffered solution?
- How many grams of aluminum are required to react with 35 mL of 2.0 M hydrochloric acid, HCl? __ HCl + __ Al __ AlCl3 + __ H2
- How do you solve titration problems step by step?
- What are two ways to measure the pH of a solution?
- Titration of an unknown amount of ascorbic acid, #C_6H_8O_6#, requires 25.4 mL of 0.100 M sodium hydroxide, #NaOH#. How do you calculate the grams of the ascorbic acid?
- 98% accuracy study help
- Covers math, physics, chemistry, biology, and more
- Step-by-step, in-depth guides
- Readily available 24/7