Write the correctly balanced net ionic equations for the reations whose equilibrium constant at 298 K are
` K_b ( CH_3NH_2)= 4.4 xx 10^(-5)`

Write the correctly balanced net ionic equations for the reations whose equilibrium constant at 298 K are K_a (H_2C_2O_4)= 5.4 xx 10 ^(-2)

Write the correctly balanced net ionic equations for the reations whose equilibrium constant at 298 K are K_b( NH_3) = 1.8 xx 10 ^(-5)

Write the correctly balanced net ionic equations for the reations whose equilibrium constant at 298 K are K_a ( H_2S ) = 1.0 xx 10 ^(-7)

Consider the following reaction. The reaction is first order in each direction, with an equilibrium constant of 10^(4) . For the conversion of chair form to boat form, e^(-Ea//RT)=4.35xx10^(-8) at 298 K with pre-exponential factor of 10^(12)s^(-1) . Apparent rate constant (k_(A)) at 298 K is :

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 equilibrium constant (K) for the formation of NH^ in the following reaction: N_2(g) + 3H_2(g) At equilibrium, the concentration of NH_3 , H_2 and N_2 are 1.2 xx 10^(-2) ,3.0 xx 10^(-2) and 1.5 xx 10^(-2) M respectively.

Calculate the hydrolysis constant of the salt containing NO_(2)^(-) . Given the K_(a) " for " HNO_(2) = 4.5 xx 10^(-10)

What is the concentration of CH_(3)COOH which can be added to 0.5M HCOOH solution so that dissociation of both is same. K_(CH_(3)COOH) = 1.8 xx 10^(-5), K_(HCOOH) = 2.4 xx 10^(-4)

Calculate [H^(+)] " and "% dissociation of 0.1 M solution of ammonium hydroxide solution . The ionisation constant for NH_(4)OH " is " K_(b) = 2.0 xx xx 10^(-5) .

Calculate [H^(+)] " and "% dissociation of 0.1 M solution of ammonium hydroxide solution . The ionisation constant for NH_(4)OH " is " K_(b) = 2.0 xx xx 10^(-5) .