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JEE Main 202331 JanuaryEvening Shift
Exam
JEE Main
Year
2023
Date
31 January
Shift
Evening Shift
Subject
Chemistry
Chapter
Ionic Equilibrium

JEE Main 2023 · 31 January · Evening Shift · Chemistry · Ionic Equilibrium

At 298K , the solubility of silver chloride in water is 1 . 434 ×...

At 298K298K, the solubility of silver chloride in water is 1.434×10−3gL−11 . 434 \times {10}^{- 3}g{L}^{- 1}. The value of −logKsp- {logK}_{sp} for silver chloride is
(Given mass of Ag is 107.9gmol−1107 . 9g{mol}^{- 1}, and mass of ClCl is 35.5gmol−135 . 5g{mol}^{- 1} )

Correct answer

0

Step-by-step solution

Formula unit mass of Silver chloride = 108+35.5gmol−1=143.5gmol−1108 + 35 . 5{gmol}^{- 1} = 143 . 5{gmol}^{- 1}
Solubility(s)=1.434143.4×10−3=10−5M( s ) = \dfrac{1 . 434}{143 . 4} \times {10}^{- 3} = {10}^{- 5}M

∴Ksp(AgCl)=[Ag][Cl]=(s)2∴ {K}_{sp} ( AgCl ) = [ Ag ] [ Cl ] = ( s{)}^{2}

⇒Ksp(AgCl)=10−10⇒ {K}_{sp} ( AgCl ) = {10}^{- 10}

⇒−log⁡(Ksp)=10⇒ - \log \left({K}_{sp}\right) = 10

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