28.4% is the answer and that is ur answer
6.022 × 10^23 × 1.45 × 10^24 = 8.7319 × 10^47
Answer:
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Answer:
Explanation:
Below is the equation of the chemical reaction:
CH3COOH (aq) + NaOH (aq) ----------> CH3COONa (aq) + H2O (l)
The mole ratio of acid and base in the balanced equation is:
Ma = 1, Mb = 1
Cb = 0.1001 mole/Kg
Ca = ???
Va = 10 grams
Vb = 131.44 - 48.11 = 83.33 grams
From the acid-base mole ration formula



The number of moles of acetic acid in the sample = 
Therefore 0.008341333 moles of acetic acid are in the sample.
Answer: The ratio of conjugate base to weak acid in the buffer system is 758 : 1
Explanation:
The dissociation constant for acid =
pH = 6.34
First we have to calculate the value of
.
The expression used for the calculation of
is,

Now put the value of
in this expression, we get:


Now we have to calculate the ratio of conjugate base to weak acid in the buffer system
Using Henderson Hesselbach equation :
![pH=pK_a+\log \frac{[\text {conjugate base}]}{[Acid]}](https://tex.z-dn.net/?f=pH%3DpK_a%2B%5Clog%20%5Cfrac%7B%5B%5Ctext%20%7Bconjugate%20base%7D%5D%7D%7B%5BAcid%5D%7D)
Now put all the given values in this expression, we get:
![6.34=3.46+\log \frac{[\text {conjugate base}]}{[Acid]}](https://tex.z-dn.net/?f=6.34%3D3.46%2B%5Clog%20%5Cfrac%7B%5B%5Ctext%20%7Bconjugate%20base%7D%5D%7D%7B%5BAcid%5D%7D)
![\frac{[\text {conjugate base}]}{[Acid]}=758](https://tex.z-dn.net/?f=%5Cfrac%7B%5B%5Ctext%20%7Bconjugate%20base%7D%5D%7D%7B%5BAcid%5D%7D%3D758)
Therefore, the ratio of conjugate base to weak acid in the buffer system is 758: 1