Saved Bookmarks
| 1. |
The acid ionization constantfor Zn^(2+)+H_(2)O hArr (OH^(+)) + H^(+) is 1.0 xx 10^(-9).Calculatethe pH of 0.0010M solution of ZnCl_(2) . Also calculate basic dissociation constant of Zn(OH)^(+) |
|
Answer» Solution : `Zn^(2+) +H_(2)O hArrZn(OH)^(+) + H^(+) ` ` :.[H^(+)] = C.h =Csqrt((K_(H))/(C)) = sqrt((K_(H))/(C))` ` = sqrt((K_(W))/(K_(b).C))"" [("where "K_(b) " is basic dissociation CONSTANT "),("of " Zn(OH) "i.e ., " Zn(OH)^(+) hArr Zn^(2+) +OH^(-))]` We know`Zn^(2+)`and `Zn(OH)^(+)`are conjugate acid and base. ` :. K_(a) xx K_(b) = 10^(-14)` or `K_(b) = (10^(14))/(10^(-9)) = 10^(-5)` Now, `[H^(+)] = sqrt((10^(-14))/(10^(-5)xx0.001)) = sqrt(10^(-12)) = 10^(-6)` pH = 6 |
|