Here the added HCl is a strong acid and all the given bases are weak bases
Now when w strong acid is added to a weak base (HB), then it form a conjugate acid salt HB+
H+ + HB -----------> HB+
Thus due to addition of strong acid, amount of HB form the solution decreases and that of HB+ increases to the same extent.
Now the pOH of such basic solution is calculated y Henderson-Hasselbalch equation
pOH = pKb + loh [salt]/[base]
And pH = 14 - pOH
pKb for different weak bases are always fixed.
Now the concepts are-
Based on the above concepts, for
1-
(CH3)2-NH = dimethyl amine, pKb = 3.27
CH3-CH2-NH2 = Ethyl amine, pKb = 3.35
Thus upon addition of HCl, change in pH for CH3-CH2-NH2 > change in pH for (CH3)2-NH
2-
CO32- = Carbonate ion, pKb = 0.999
CN- = Cyanide anion, pKb = 4.60
Thus upon addition of HCl, change in pH for CN- > change in pH for CO32-
Lets prove this by taking an example-
7. Identify the titrant in each pair that wou ld provide a greater pH change about the equivalence point in the tit...
6. Identify the titrant in each pair that would provide a greater pH change about the equivalence point in the titration of a 0.100 M NaOH solution. Explain your reasoning for your choice for each pair. a) 0.10 M benzoic acid (C6H5CO2H) or 0.10 M chloroacetic acid (CICH2CH2CO2H) (2 pts) b) 0.10 M hydrofluoric acid (HF) or 0.10 M formic acid (HCO2H) (2 pts)