In a titration, for an acid to neutralize a base, at the equivalence point, there should be an equal number of moles of H+ and OH-.
Moles of OH- can be found by multiplying the concentration of the base by the volume. (You will need to keep in mind the stoichimetric coefficients if the strong base is Ca(OH)₂, Ba(OH)₂, or Sr(OH)₂.
Moles of OH- = moles of H+
(0.253 M) * 0.005 L = 0.01000 L * c
c = 0.1265 M
The concentration of HBr is 0.127 M.
The exact opposite end of the earth or 180degrees
Answer:

Explanation:
The amount adsorbed (solute) is the acetic acid, and the adsorbent is the activated charcoal. The mass of the adsorbent is 10 g.
So, we need to calculate the mass of the acetic acid as follows:

Where:
n: is the number of moles = C*V
M: is the molecular mass = 60.052 g/mol
C: is the final concentration of the acid = 0.5*0.2 mol/L = 0.10 mol/L
V: is the volume = 50 ml = 0.050 L

Now, the amount of solute adsorbed per gram of the adsorbent is:

Therefore, the amount of solute adsorbed per gram of the adsorbent is 0.03 g/g.
I hope it helps you!
Answer:
The periodic table is also split into four blocks: s = red, p = green, d = yellow, and f = blue.