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)`

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_b ( CH_3NH_2)= 4.4 xx 10^(-5)

Calculate the degree of hydrolysis of 0.1 M solution of sodium acetate at 298 K : K_(a) = 1.8 xx 10^(-5) .

It is given that 0.001 mol each of Cd^(2+) and Fe^(2+) ions are contained in 1.0L of 0.02M HC1 solution. This solutions is now saturated with H_(2)S gas at 25^(@)C . a. Determine whether or not each of these ions will be precipitated as sulphide? b. How much Cd^(2+) ions remains in the solution at equilibrium? K_(1)(H_(2)S) = 1.0 xx 10^(-7), K_(2) (H_(2)S) = 1.0 xx 10^(-14) : ltbRgt K_(sp) (CdS) = 8 xx 10^(-27): K_(sp) (FeS) = 3.7 xx 10^(-19) .

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 :

An aqueous solution contains 0.10 MH_2 S and 0.20 M HCl if the equilibrium constants for the formation of HS^(-) " from " H_2S " is " 1.0 xx 10^(-7) and " that of " S^(2-) " from " HS^(-) ions is 1.2 xx 10 ^(-13) then the concentration of S^(2-) ions in aqueous solution is 5 xx 10 ^(-8) 3 xx 10 ^(-20) 6 xx 10 ^(-21) 5 xx 10 ^(-19)

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 entropy change for a reaction: XrarrY Given that DeltaH^(Theta) = 28.40 kJ mol^(-1) and equilibrium constant is 1.8 xx 10^(-7) at 298K .

Identify the reaction order form each of the following rate constants: a. k = 7.06 xx 10^(-3) mol L^(-1) s^(-1) b. k = 5.6 xx 10^(-5) s^(-1) c. k = 1.25 xx 10^(-2) mol^(-1)l s^(-1) d. k = 1.25 xx 10^(-2) mol L^(2)s^(-1) e. k = 5.0 xx 10^(-6) atm^(-1)s^(-1)