If K_(sp) for HgSO_(4) is 6.4xx10^(-5) , then solubility of this substance in mole per m^(3) is
Find: 1.3xx10
The molar solubility of ferric hydroxide in aqueous solution is 6xx10^(-38) at 298 K. the solubility of Fe^(3+) ion will increase when the :
AgBr (s) + 2S_(2)O_(3)^(2)(aq.)hArrAg(S_(2)O_(3))_(2)^(3-)(aq.)+Br^(-)(aq) "[""Using":K_(sp)(AgBr)=5xx10^(-13)" " K_(f)(Ag(S_(2)O_(3))_(2)^(3-))=5xx10^(13)"]" What is the molar solubility of AgBr in 0.1 M Na_(2)SO_(3) ?
The simultaneous solubility of AgCN(K_(sp)=2.5xx10^(-16)) and AgCl(K_(sp)=1.6xx10^(-10)) in 1.0 M NH_(3)(aq.) are respectively: [Given: K_(f1)[Ag(NH_(3))_(2)^(+)=10^(7)
Solubility of AgCl in 0.2 M NaCl is x and that in 0.1 M AgNO_(3) is y. Then which of the following is correct?
The K_(sp) for AgCl at 298K is 1.0xx10^-10 . Calculate the electrode potential for Ag^+|Ag electrode immersed in 1.0M KCl solution. Given: E_(Ag^+|Ag)^@=0.80V
The solubility product of AgCl is 10^(-10)M^(2) . The minimum volume ( in m^(3)) of water required to dissolve 14.35 mg of AgCl is approximately :
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
