Calculate the `pH` at which the concentration of a monobasic acid HA equals the concentration of its conjugate base at equilibrium. `(K_(a)=2times10^(-5)`, `log2=0.3)`

Calculate the H^(+) ion concentration of 0.01 weak monobase acid . The value of dissociation contant is 4.0 xx 10^(-10)

Calculate the concentration of hydrogen ion in the acidic solution with pH a. 4.3

In a gaseous reaction A+2B iff 2C+D the initial concentration of B was 1.5 times that of A. At equilibrium the concentration of A and D were equal. Calculate the equilibrium constant K_(C) .

Calculate the concentration of the formate ion present in 0.100 M formic acid (HCOOH) solution at equilibrium (K_(a) = 1.7xx10^(-4)) .

A buffer solution is prepared in which the concentration of NH_(3) is 0.30 M and the concentration of NH_(4)^(+) is 0.20 M . If the equilibrium constant, K_(b) for NH_(3) equals 1.8xx10^(-5) , what is the pH of this solution? ( log 2.7=0.43 )

Calculate the concentration of overset(Θ)OH in the solution of base with pH a. 10.4771

In an equilibrium A+B hArr C+D , A and B are mixed in vesel at temperature T. The initial concentration of A was twice the initial concentration of B. After the equilibrium has reaches, concentration of C was thrice the equilibrium concentration of B. Calculate K_(c) .

Calculate pH at which an acid indicator Hin with concentration 0.1M changes its colour ( K_(a) for "Hin" = 1 xx 10^(-5) )

What is pH of 7.0 xx 10^(-8)M acetic acid. What is the concentration of un-ionsed acetic acid. K_(a) of CH_(3)COOH = 1.8 xx 10^(-5) .

Calculate the pH value of the solution in which the concentration of OH^(-) " ions is " 5.0 xx 10^(-9) " mol " L^(-1) at 298 K