At 298 K, the solubility of silver chloride in water is 1.434 × 10-3 g L -1. The value of - log K 3 p for silver chloride is (Given mass of Ag is 107.9 g mol -1 and mass of Cl is 35.5 g mol -1 )

Question

At 298 K, the solubility of silver chloride in water is 1.434 × 10-3 g L -1. The value of - log K 3 p for silver chloride is (Given mass of Ag is 107.9 g mol -1 and mass of Cl is 35.5 g mol -1 ) (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

AgCl ( s ) arrow undersetSAg +(aq.) + undersetSCl -(aq.) K sp = S 2=((1.43/143.4) × 10-3)2=10-10 - log K sp =10

Q. At $298 K$ , the solubility of silver chloride in water is $1.434 \times 1 0^{- 3} g L^{- 1}$ . The value of $- lo g K_{3 p}$ for silver chloride is
(Given mass of $A g$ is $107.9 g m o l^{- 1}$ and mass of $Cl$ is $35.5 g m o l^{- 1}$ )

$A g Cl (s) \to S A g^{+}$ (aq.) $+ S C l^{-}$ (aq.)
$K_{s p} = S^{2} = (\frac{1.43}{143.4} \times 1 0^{- 3})^{2} = 1 0^{- 10}$
$- lo g K_{s p} = 10$

Q. At 298K, the solubility of silver chloride in water is 1.434×10−3gL−1. The value of −logK3p​ for silver chloride is (Given mass of Ag is 107.9gmol−1 and mass of Cl is 35.5gmol−1 )

AgCl(s)→SAg+​(aq.) +SCl−​(aq.) Ksp​=S2=(143.41.43​×10−3)2=10−10 −logKsp​=10

Q. At $298 K$ , the solubility of silver chloride in water is $1.434 \times 1 0^{- 3} g L^{- 1}$ . The value of $- lo g K_{3 p}$ for silver chloride is
(Given mass of $A g$ is $107.9 g m o l^{- 1}$ and mass of $Cl$ is $35.5 g m o l^{- 1}$ )

$A g Cl (s) \to S A g^{+}$ (aq.) $+ S C l^{-}$ (aq.)
$K_{s p} = S^{2} = (\frac{1.43}{143.4} \times 1 0^{- 3})^{2} = 1 0^{- 10}$
$- lo g K_{s p} = 10$