Arrange the following 0.10 M solutions in order of most acidic to most basic. See Appendix 5 for K a and K b values. KCl Sr(OH) 2 HONH 3 ClO 4 HNO 3 KF Solution Ka or the acid dissociation constant gives the measure of the strength of a given acid.It is the equilibrium constant for reaction involving weak acids dissociation. For a weak acid,say,HA HA<--->H + +A - Ka=[H + ][A - ]/[HA] Higher the ka ,stronger is the acid. for strong acids,ka>1 Similarly,kb or the base dissociation constant gives the measure of the strength of a given weak base.It is the equilibrium constant for reaction involving weak base dissociation. For a weak base,say,BOH BOH<--->OH - +B + Kb=[B + ][OH - ]/[BOH] Higher the kb ,stronger is the base KCl is a salt of strong base KOH and strong acid HCl, it is neutral Sr(OH)2 has ka >0 (weak base) HONH3ClO4 <---> HONH3 + + ClO4 - HONH3 + <-->H+ +HONH2 (releases proton so acidic) ka=9.09*10^-7 HNO3 --->H + +NO3- (strong acid ka>1) KF is a salt of strong base KOH and weak acid HF so it is a basic salt In solution, F- base hydrolysis takes place as folllows, KF--->K + +F- F- +H2O <--> HF +OH- order from most acidic to most basic: HNO3>HONH3ClO4>KCl>KF>Sr(OH)2 . for strong acids,ka>1 for a .