The equilibrium constant for the reaction `OCl^(-)(aq)+H_(2)O(l) iff HOCl(aq)+OH_((aq))^(-)` at 298 K is `3.6 times 10^(-7)`. The Ka of HOCl at 298 K is
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The equilibrium constant for the reaction HCO_(3)^(-)(aq)+HPO_(4)^(2-)(aq) iff CO_(3)^(2-)(aq)+H_(2)PO_(4)^(-)(aq) is approximately 10^(-3) . The strongest conjugate base in this reaction is
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In a saturated solution of the sparingly soluble salt AgIO_(3) (Mol. Mass = 283 g mol^(-1) ), the equilibrium which sets in is AgIO_(3)(s) iff Ag^(+)(aq)+IO_(3)^(-)(aq) . If the K_(sp) of AglO_(3) is 1 times 10^(-8)M^(2) at 298 K. What is the mass of AglO_(3) contained in 100 ml of its saturated solution at 298 K?
Equilibrium constant of a reaction is 10, what will be the value of Delta G^(@) (in kcal mol^(-1) ) at 298 K?
For the cell reaction, A(s) + 2B^(-)"(aq) rarr A^(2+) (aq) + 2B(s) , the value of Kc is 3.98 xx 10^(15) .Calculate E_(cell)^(@) at 298 K.
For the equilibrium (autoprotolysis of water), 2H_(2)O iff H_(3)O^(+)+OH^(-) , the value of DeltaG^(0) at 298 K is approximately?
The following equilibria and their equilibrium constants are given N_(2)+3H_(2) iff 2NH_(3)(K_(1)) N_(2)+O_(2) iff 2NO(K_(2)) H_(2)+1/2O_(2) iff H_(2)O(K_(3)) Therefore, the equilibrium constant of the reaction 2NH_(3)+5/2O_(2) iff 2NO+3H_(2)O in terms of K_(1), K_(2) and K_(3) is :
The equilibrium constant of the following redox reaction at 298 K is 1 xx 10^(8) 2Fe^(3+) (aq.)+ 2I^(-) (aq.) rarr 2Fe^(2+) (aq)+I_(2) (s) If the standard reduction potential of iodine becoming iodide is +0.54 V. What is the standard reduction potential of (Fe^(3+))/(Fe^(2+)) ?
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