[" 13.A solution of "0.10M" NaZ has pH "],[=8.90." The "K_(a)" of "HZ" is : "]

A solution of 0.1M NaZ has pH = 8.90 . The K_(a) of HZ is

A solution of 0.1M NaZ has pH = 8.90 . The K_(a) of HZ is

A solution of 0.1 M NaZ has PH = 8.90 . The K_a of HZ is.

A buffer solution contains 0.04 M HA and 0.01 M CaA_(2) . If K_(b) of A^(-) is 10^(-12) then pH of buffer solution is Given : log 2 = 0.3

A buffer solution contains 0.04 M HA and 0.01 M CaA_(2) . If K_(b) of A^(-) is 10^(-12) then pH of buffer solution is Given : log 2 = 0.3

A solution of pH 9.0 is 1000 times as basic as a solution. The pH of this solution is

Calculate the pH of 0.10 M solution of Nh_(4)Cl. The dissociation constant (K_(b)) of NH_(3) is 1.8xx10^(-5)

Calculate the pH of 0.10 M solution of NH_(4)Cl. The dissociation constant (K_(b)) of NH_(3) is 1.8 X 10^(-5)

When 0.0030 mol of HCI is added to 100 mL of a 0.10 M solution of a weak base, R_(2)NH , the solution has a pH of 11.10. What is 1 K_(b) for the weak base ?