An Ionic Problem ⌣ ¨
What is [ A g + ] in a solution made by dissolving both A g 2 C r O 4 and A g 2 C 2 O 4 until saturation is reached with respect to both salts ?
Useful Data :
K s p ( A g 2 C 2 O 4 ) = 2 × 1 0 − 1 1 , K s p ( A g 2 C r O 4 ) = 2 × 1 0 − 1 2
The answer is 0.000352.
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1 solution
if pKb for fluoride ion at 25 C is 10.83, the ionisation constant iof hydrofluoric acid is jn water at this temperature is ?
the answer to this question is 6.75*10^-4. please tell the solution as soon as possible
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Calculate kB from pKB value Then input Ka=kW/Kb (for the conjugate-acid base pair) To get ionisation constant of HF
which of the following solutions will ph exactly equal to8 ?
(A)10^-8M HCl solution at 25 C
(B)10^-8M H+ solution at 25 C
(C) 2*10^-6M Ba(OH)2 solution at 25 C
(D) 10^-6M NaOH solution at 50 C
answer is (B) ,but how???
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Option B directly follows from the definition of pH In option D Notice That the temperature mentioned is 50 C But we know ionic-product of water is 10^(-14) only at 25 C (at 50 C,it will increase) Hence a 10^-6 M NaOH soln at 50 C won't have pH=8
[Ag+]=x. [c2o4]=y [cro4]=z X^2 Y=2.e-11 X^2 Z=2e-12 X=2(x+y) Work out X=3.5e-4