It's lone a little distinction (103 degrees versus 104 degrees in water), and I trust the standard rationalization is that since F is more electronegative than H, the electrons in the O-F bond invest more energy far from the O (and near the F) than the electrons in the O-H bond. That moves the powerful focal point of the unpleasant constrain between the bonding sets far from the O, and thus far from each other. So the shock between the bonding sets is marginally less, while the repugnance between the solitary matches on the O is the same - the outcome is the edge between the bonds is somewhat less.
Answer is: b. more than 7.
The endpoint is the point at which the indicator changes colour in a colourimetric titration and that is point when titration must stop.
For example, basic salt sodium acetate CH₃COONa is formed from the reaction between weak acid (in this example acetic acid CH₃COOH) and strong base (in this example sodium acetate NaOH).
Balanced chemical reaction of acetic acid and sodium hydroxide:
CH₃COOH(aq) + NaOH(aq) → CH₃COONa(aq) + H₂O(l).
Neutralization is is reaction in which an acid (in this example vinegar or acetic acid CH₃COOH) and a base react quantitatively with each other.
The answer is D. Effective collisions lead to chemical reactions!
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
