not sure
Ka= [H+] [H2BO3-]
___________
[H3BO3]
ka=[H+][H2BO3-]/[H3BO3]
ka=[H+][NO2_]/[HNO2]
Ka= [H+][NO2-] [HNO2]
ka=[H+][CN-]/[HCN]
Ka= [H+] [H2BO3-] / [h3BO3] (Apex)
Ka= [h+][HCO3-]/[H2CO3]
Ka= [H+][NO2-] [HNO2]
ka=[H+][NO2_]/[HNO2]
ka=[H+][CN-]/[HCN]
Ka= [H+] [H2BO3-] / [h3BO3] (Apex)
Ka= [h+][HCO3-]/[H2CO3]
ka=[H+][NO2_]/[HNO2]
HCN(aq) ==> H^+(aq) + CN^-(aq)Ka = [H+][CN-]/[HCN] and the value can be looked up in a book or on line.
Since H3PO4 has 3 ionizable hydrogens, it will have three Ka values. Approximate values areKa1 = 7x10^-3; Ka2 = 6x10^-8 and Ka3 = 4.5x10^-13
HCl (aq) + H2O (L) ---------> H3O+ (aq) + Cl- (aq)
H+(aq)+ Br-(aq) +Na+(aq) + OH-(aq)----->H+(l)+OH-(l) +Br-(S) +Na+(S)By cancelling out the spectator ions we are left with...H+(aq) + OH-(aq) ------> H(l)+ + OH(l)-
Molecular Eq HC2H3O2(aq) + NH3(aq) -> NH4+(aq) + C2H3O2-(aq) Ionic Eq H+(aq) + C2H3O2-(aq) + NH3(aq) -> NH4+(aq) + C2H3O2-(aq) Net Ionic Eq H+(aq) + NH3(aq) -> NH4+(aq)
NaHCO3 ---> Na+(aq) + HCO3-(aq) CH3COOH <--> H+(aq) + CH3COO-(aq) H+ + HCO3- ---> H2CO3 H2CO3 ---> H2O + CO2