A solution is 0.1M in Cl- and 0.001M in
. Solid AgNo3 is gradually added to it. Assuming that the addition does not change in volume and Ksp(AgCl) = 1.7 × 10-10M2 and Ksp (Ag2CrO4) = 1.9 × 10-12M3
A solution is 0.1M in Cl- and 0.001M in . Solid AgNo3 is gradually added to it. Assuming that the addition does not change in volume and Ksp(AgCl) = 1.7 × 10-10M2 and Ksp (Ag2CrO4) = 1.9 × 10-12M3
Option 1 -
Ag2CroO4 precipitates first because the amount of Ag+ of needed is low.
Option 2 -
Ag2CrO4 precipitates first as its Ksp is low.
Option 3 -
AgCl will precipitate first as the amount of Ag+ needed to precipitate is low.
Option 4 -
AgCl precipitates first because its Ksp is high.
-
1 Answer
-
Correct Option - 3
Detailed Solution:for AgCl ppt1,
For Ag2CrO4ppt2,
Being lower concentration of [Ag+] in case of AgCl, it will precipitate first.
Similar Questions for you
0.01 M NaOH,
M = 1 * 10-2
pOH = 2
pH = 2
Kp = Kc (RT)Dng
36 * 10–2 = Kc (0.0821 * 300)–1
Kc = 0.36 * 0.0821 * 300 = 8.86 » 9
A(g) ->B(g) + (g)
Initial moles n 0 0
Eqb. moles n(1 – a) na
total moles =
Eqb. pressure
On increasing pressure, equilibrium moves in that direction where number of gaseous moles decreases.
Taking an Exam? Selecting a College?
Get authentic answers from experts, students and alumni that you won't find anywhere else
Sign Up on ShikshaOn Shiksha, get access to
- 65k Colleges
- 1.2k Exams
- 687k Reviews
- 1800k Answers