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)

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)

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

What is pH of 0.02 M solution of ammonium chloride at 25^(@) C ? K_(b) (NH_(3)) = 1.8 xx 10^(-5) .

Write balanced equation for B_2 H_6 + NH_3 to

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 )

The molarity of NH_(3) of pH = 12 at 25^(@)C is (K_(b) = 1.8 xx 10^(-5))

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 :

The hydrolysis constant of 0.1M aqueous solution of sodium acetate if K_(a) of CH_(3)COOH = 1.8 xx 10^(-5) is