Given `K_(a)` values of `5.76xx10^(-10)` and `4.8xx10^(-10)` for `NH_(4)^(+)` and HCN respectively. What is the equilibrium constant for the following reaction?
`NH_(4)^(+)(aq.)+CN^(-)(aq.)hArrNH_(3)(aq.)+HCN(aq.)`

Write the equilibrium constant expressions for the following reactions. NH_3( aq) +H_2O (l) hArr NH_4^(+) (aq) +OH^(-) (aq)

The reaction NH_(4)^(+)+CN rarr HCN(aq)+NH_(3)(aq) proceeds in

The reaction NH_(4)^(+)+CN rarr HCN(aq)+NH_(3)(aq) proceeds in

Balance the following equation : KCN (aq) +H_2SO_4(aq) rarr K_2SO_4(aq)+HCN(g)

K_a for CH_3 COOH and HCN are respectively 1.8 xx 10^(-5) and 5 xx 10^(-10) Calculate the equilibrium constant for the reaction CH_3 COOH + NaCN hArr CH_3 COONa + HCN .

If K_(sp) (PbSO_(4)) =1.8 xx 10^(-8) and K_(a) (HSO_(4)^(Theta)) = 1.0 xx 10^(-2) the equilibrium constant for the reaction. PbSO_(4)(s) +H^(o+)(aq) hArr HSO_(4)^(Theta)(aq) +Pb^(2+)(aq) is

If K_(sp) (PbSO_(4)) =1.8 xx 10^(-8) and K_(a) (HSO_(4)^(Theta)) = 1.0 xx 10^(-2) the equilibrium constant for the reaction. PbSO_(4)(s) +H^(o+)(aq) hArr HSO_(4)^(Theta)(aq) +Pb^(2+)(aq) is

Identify the oxidant and reductant in the following reactions: 10H^(+)(aq)+4Zn(s)+NO_3^(-) (aq)to4Zn^(2+) (aq)+NH_4^(+) +3H_2O(l)

If K_(a) of HCN =4xx10^(-10) , then the pH of 2.4 xx 10^(-1) molar HCN(aq) is

Equilibrium const. {:(H_2S(aq)hArr H^+(aq)+HS^(-)(aq)," " K_1=9.5xx10^(-8)),(HS^(-)(aq)hArr H^+(aq)+S^(2-)(aq)," " K_2=1.0xx10^(-19)):} What is the equilibrium constant for the reaction ? S^(2-)(aq)+2H^(+)(aq) hArr H_2S(aq) " " K=?