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Unformatted text preview: aq) + Cl (aq) [Ag + ][Cl ] [AgCl] · Due to slight solubilit y o f these salts [AgCl] remains constant the equilibrium expressio n can be summarized as shown below: +
Keq [AgCl] = [Ag ] [Cl ] Solubility product constant + –
Ksp = [Ag ] [Cl ] Examples: –
1. The solubilit y o f silver chloride is water is 1.3x10 5 M. Calculate the Ksp value for AgCl. +
When 1 mo l of AgCl disso lves it produces 1 mo l of Ag and 1 mol o f Cl . + –
Therefore, [Ag ] = [Cl ] = 1.3x10 5 M +
Ksp = [Ag ] [Cl ] = (1.3x10 5)(1.3x10 5 ) = 1.7x10 10 –
2. The Ksp value for PbSO4 is 1.3 x 10 8 . Calculate the solubilit y of PbSO4 in M. ˆˆ
PbSO4 (s) ‡ˆ† Ksp = –
3. The solubilit y o f silver chro mate, Ag2CrO4, is 7.8x10 5 M. Calculate the Ksp value for this salt. 15 Chemistry 52 Chapter 16 THE COMMON ION EFFECT
· A shift in the equilibrium posit ion upon addit ion of an io n already contained in the so lut ion is known as the common ion effect.
· As an example, silver chloride forms the fo llowing equilibrium: ˆˆ
AgCl (s) ‡ˆ† + –
Ag (aq) + Cl (aq) · When so lid silver nitrate (as soluble salt) is added to this so lution, it dissociates as fo llows: + AgNO3 (s) ® Ag (aq) + NO3– (aq) +
· Silver ions (Ag ) are commo n in both eq...
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