The solubility of agcl(s) in water at 25°c is 1.33 x 10-5 mol/l and its δh° of solution is 65.7 kj/mol. what is its solubility at 95°c?

The solubility of agcl(s) in water at 95°C is : 5.4 * 10⁻⁴  mol/L

Given data :

solubility of agcl(s) at 298 k ( 25°c ) = 1.33 * 10⁻⁵ mol/l

ΔH∘ of solution =  65.7 kJ/mol

applying van't hoff equation

ln  -  ΔH∘ / R * ( 1 / T₂ - 1 / T₁ )  --- ( 1 )

where : T₂ = 273 + 95 = 368 k , T₁ = 298 k

Substitute values into equation ( 1 )

ln ( Ksp / 1.7689 * 10⁻¹⁰ ) =  - 65.7 * 10³ / 8.314 * ( 1 / 368 - 1 / 298 )

therefore :

( Ksp / 1.7689 * 10⁻¹⁰ ) = -7.90 * 10³ * -0.00064

                                    = e^5.056

therefore:  Ksp = 1.7689 * 10⁻¹⁰ * 156.96

                         = 2.776 * 10⁻⁸

Given that:   Ksp = S² ( solubility )

solubility ( s ) at 95° C  = 5.4 * 10⁻⁴  mol/L

                                     = 5.4 * 10⁻⁴  mol/L

Hence we can conclude that The solubility of agcl(s) in water at 95°C is : 5.4 * 10⁻⁴  mol/L

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the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.

a) the particles of the chair are strongly held together.