Normal 0false false falseEN-US X-NONE X-NONE/* Style Definitions */table.MsoNormalTable{mso-style-name:Table Normal;mso-tstyle-rowband-size:0;mso-tstyle-colband-size:0;mso-style-noshow:yes;mso-style-priority:99;mso-style-parent:;mso-padding-alt:0in 5.4pt 0in 5.4pt;mso-para-margin-top:0in;mso-para-margin-right:0in;mso-para-margin-bottom:10.0pt;mso-para-margin-left:0in;line-height:115%;mso-pagination:widow-orphan;font-size:11.0pt;font-family:Calibri,sans-serif;mso-ascii-font-family:Calibri;mso-ascii-theme-font:minor-latin;mso-hansi-font-family:Calibri;mso-hansi-theme-font:minor-latin;mso-bidi-font-family:Times New Roman;mso-bidi-theme-font:minor-bidi;}The solubility of silver chloride in 0.2 M NaCl is (Given Ksp AgCl = 1.8 × 10−10)(A) 9 × 10−10 M(B) 3.6 × 10−10 M(C) 1.8 × 10−11 M(D) 7.2 × 10−10 M
Radhika Batra , 11 Years ago
Grade 11
2 Answers
Amit Saxena
Last Activity: 11 Years ago
Since NaCl is a strong electrolyte therefore the entire conc. of Cl− ions comes from NaCl Ksp AgCl = [Ag+] [Cl−]. If solubility of Ag+ = s in NaCl then
India VK
Last Activity: 11 Years ago
(A)
NaCl dissociates fully to give [Cl-] = 0.2 and contribution of [Cl-] from AgCl is negligible compared to it.
So, Ksp = [Ag+][Cl-] = 1.8*10^(-10)
Find [Ag+] which will be the solubility.
Provide a better Answer & Earn Cool Goodies
Enter text here...
LIVE ONLINE CLASSES
Prepraring for the competition made easy just by live online class.
Full Live Access
Study Material
Live Doubts Solving
Daily Class Assignments
Ask a Doubt
Get your questions answered by the expert for free