Q36.The molar solubility of Cd(OH)2 is 1.84 × 10−5M in water. The expectes solunility of Cd(OH)2 in a buffer solution of pH = 12 is: (1) 2.49 × 10−10M (2) 2.491.84 × 10−9M (3) 1.84 × 10−9M (4) 6.23 × 10−11M
What This Question Tests
This question requires calculating the solubility product (Ksp) of Cd(OH)₂ from its solubility in water, and then using Ksp along with the common ion concentration (from the given pH) to determine its solubility in the buffer solution.
Concepts Tested
Formulas Used
Ksp = [Cd2+][OH-]^2
pOH = 14 - pH
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2.4 Calculate the standard cell potentials of galvanic cell in which the following reactions take place: (i) 2Cr(s) + 3Cd2+(aq) ® 2Cr3+(aq) + 3Cd (ii) Fe2+(aq) + Ag+(aq) ® Fe3+(aq) + Ag(s) Calculate the DrGo and equilibrium constant of the reactions. 2.5 Write the Nernst equation and emf of the following cells at 298 K: (i) Mg(s)|Mg2+(0.001M)||Cu2+(0.0001 M)|Cu(s) (ii) Fe(s)|Fe2+(0.001M)||H+(1M)|H2(g)(1bar)| Pt(s) (iii) Sn(s)|Sn2+(0.050 M)||H+(0.020 M)|H2(g) (1 bar)|Pt(s) (iv) Pt(s)|Br–(0.010 M)|Br2(l )||H+(0.030 M)| H2(g) (1 bar)|Pt(s).
📋 Question Details
- Chapter
- Ionic Equilibrium
- Topic
- Solubility Product and Common Ion Effect
- Year
- 2019
- Shift
- 12 Apr Shift 2
- Q Number
- Q36
- Type
- Numerical
- NCERT Ref
- Class 11 Chemistry Ch 7: Equilibrium
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