Use your experimentally determined value of ksp and show, by calculations, that ag2cro4 should precipitate when 5ml of 0.004m agno3 are added to 5ml of 0.0024 m k2cro4.

When the value of Ksp = 3.83 x 10^-11 (should be given - missing in your Q)

So, according to the balanced equation of the reaction:

and by using ICE table:

              Ag2CrO4(s)  → 2Ag+ (Aq) + CrO4^2-(aq)

initial                                     0                   0

change                              +2X                 +X

Equ                                       2X                   X

∴ Ksp = [Ag+]^2[CrO42-]

so by substitution:

∴ 3.83 x 10^-11 = (2X)^2* X

3.83 x 10^-11 = 4 X^3

∴X = 2.1 x 10^-4 

∴[CrO42-] = X = 2.1 x 10^-4 M

[Ag+] = 2X = 2 * (2.1 x 10^-4) 

                  = 4.2 x 10^-4 M

when we comparing with the actual concentration of [Ag+] and [CrO42-]

when moles Ag+ = molarity * volume

                               = 0.004 m * 0.005L

                               = 2 x 10^-5 moles
[Ag+] = moles / total volume
     
          = 2 x 10^-5 / 0.01L

          = 0.002 M

moles CrO42- = molarity * volume

                         = 0.0024 m * 0.005 L

                         = 1.2 x 10^-5 mol

∴[CrO42-] = moles / total volume

                 = (1.2 x 10^-5)mol / 0.01 L 

                 = 0.0012 M

by comparing this values with the max concentration that is saturation in the solution 

and when the 2 values of ions concentration are >>> than the max values o the concentrations that are will be saturated.

∴ the excess will precipitate out       

A. 40 degrees celsius

If the water vapor content stays the same and the temperature drops, then the relative humidity increases. its vise versa.if the water vapor content stats the same and the temperature rises, the relative humidity decreases. so, yes, i'd say that temperature and humidity have a strong relationship.