Selenious acid `(H_(2)SeO_(3))`, a diprotic acid has `K_(a1)=3.0xx10^(-3)` and `K_(a2)=5.0xx10^(-8)`. What is the `[OH^(-)]` of a 0.30 M solution of selenious acid?
H_3A is a weak triprotic acid (K_(a_1) =10^(-5) ,K_(a_2) =10^(-13) ) . What is the value of pX of 0.1 M H_3 A(aq.) solution ? Where pX =- log X and X = ([A^(3-)])/([HA^(2-)])
The pH of 0.05 M acetic acid is (K_(a) = 2 xx 10^(-5))
Calculate pH of 0.1 M acetic acid having K_(a)=1.8xx10^(-5)
K_(a_1) and K_(b_1) of oxalic acid are 6 xx 10^(-2) and 7.2 xx 10^(-5) respectively. Calculate the pH of 0.06 M oxalic acid solution
The ionization constant of chloroacetic acid is 1.65xx10^(-3) . What will be the pH of 0.1M acid and its 0.1M sodium salt solution ?
A solution containing a weak acid and its conjugate acts as an acidic buffer. In a buffer the dissociation of the well acid is suppressed by its conjugate base. (K_(1),K_(2), and K_(3), of H_(3)PO_(4) , are 10_(-4), 10^(-4), 10^(-13) respectively What is the P^(H) of a solution obtained by mixing 100ml of 0.1 MH(3) PO_(4) , and 150ml of 0.IM NaOH
K_a for HF is 3.2 xx 10^(-4) . Calculate the percentage of dissociation in 0.02 M HF solution.
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
