Answer:
The purpose of a lab report is to organize and communicate what you did in your experiment.
Explanation:
Answer: 72L of 30% and 128L of 80%
You can determine the weight of the acid by multiplying the concentration with the volume. Let say v1 is the volume of 30% solution needed and v2 is the volume of 80% solution.
The weight of acid from the used solution should be equal to the product. You can get this equation
final solution= solution1 + solution2
200l * 62%= v1 * 30% + v2*80%
124L= 0.3v1 + 0.8v2
124L- 0.3v1= 0.8v2
v2=155L- 0.375v1
The total volume of both should be 200l. If you use the previous equation, you can calculate:
v1+v2=200L
v1+ (155L- 0.375v1)= 200L
0.625v1= 200L - 155L
v1= 45/ 0.625= 72L
v1+v2=200L
v2= 200L- 72L= 128L
Answer:
8.73
Explanation:
The concentration of acetic acid can be determined as follows:
Moles of 
= 
=0.0090 moles
Moles of 
= 0.0090 moles
The equation for the reaction can be expressed as :
-----> 
Concentration of 
ion = 
= 
= 0.052 M
Hydrolysis of ion:
-----> 
⇒ 
= 
As K is so less, then x appears to be a very infinitesimal small number
0.052-x ≅ x
![[OH] = x =0.535*10^{-5}](https://tex.z-dn.net/?f=%5BOH%5D%20%3D%20x%20%3D0.535%2A10%5E%7B-5%7D)
![pOH = -log[OH^-]](https://tex.z-dn.net/?f=pOH%20%3D%20-log%5BOH%5E-%5D)
![pOH = -log[0.535*10^{-5}]](https://tex.z-dn.net/?f=pOH%20%3D%20-log%5B0.535%2A10%5E%7B-5%7D%5D)
pH = 14 - pOH
pH = 14 - 5.27
pH = 8.73
Hence, the pH of the titration mixture = 8.73
