A 1 litre solution containing `NH_(4)Cl` and `NH_(4)OH` has hydroxide ion ion concentration of `10^-6)` mol//litre. Which of the following hydroxides could be precipitated when the solution is added to 1 litre solution of 0.1 M metal ions? (I) `Ba(OH)_(2)(K_(sp)=5xx10^(-3))` , (II) `Ni(OH)_(2)(K_(sp)=1.6xx10^(-16))` (III) `Mn(OH)_(2) (K_(sp)=2xx10^(-13))` , (IV) `Fe(OH)_(2) (K_(sp)=8xx10^(-16))`
The H^(+) ion concentration of a solution is 4xx10^(-5) M. Then the OH^(-) ion concentration of the same solution is
The solubility of AgCl in 0.1M NaCI is (K_(sp) " of AgCl" = 1.2 xx 10^(-10))
What is the molar solubility of Fe(OH)_2 (K_(sp) =8.0 xx 10^(-16) ) at pH 13.0 ?
The H ion concentration of a solution is 4.75xx10^(-5) M. Then the OH ion concentration of the same solution is
Find the concentration of hydroxide ion in a 0.25 M solution of trimethylamine, a weak base. (CH_(3))_(3)N+H_(2)OhArr(CH_(3))_(3)+OH^(-),K_(b)=7.4xx10^(-5)
A solution is 0.01 M Kl and 0. 1 M KCl . If solid AgNO_3 is added to the solution, what is the [1^(-) ] when AgCl begins to precipitate [K_(sp) (Agl) =1.5 xx 10^(-16) , K_(sp) (AgCl) =1.8 xx 10^(-10)]
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions