Would your calculated Ksp value be greater, less, or the same, if the following occurred, please explain your reasoning.
a. The CaSO4 was not saturated
b. You accurately measured 20.00 mL instead of 25.00 mL using a pipet
c. The CaSO4 solution contained 1.0 M NaCl (aq)
d. When the CaSO4 was being dissolved, solid, soluble CaCl2
e. The end point of the titration was 2 mL before the equivalence point
I don't know the pro you used so I don't know what;s going on in part b. Part d needs work.
okay what about the others?
Of course you could have typed the procedure you followed.
Part d still needs to be completed.
For a, if the CaSO4 is not saturated solution then both Ca^2+ and SO4^2- wil be less than they should be and Ksp (experimentsl value) will be smaller than the actual value.
c. In freshman courses the addition of NaCl will not significantly affect the Ksp value. In more advanced classes you learn it will.
d. Some words are missing at the end.
e. End point before means Ca and SO4 are too small and Ksp experimental value will be too small.
a. If the CaSO4 was not saturated, it means that the solution contains less dissolved CaSO4 than the maximum amount it can hold at that temperature. Therefore, the concentration of calcium (Ca2+) and sulfate (SO42-) ions in the solution would be lower than if the CaSO4 was saturated. As a result, the Ksp value would be smaller because the numerator (concentration of ions) would be lower.
b. Accurately measuring 20.00 mL instead of 25.00 mL using a pipet would affect the volume of the solution used in the calculation of the molar solubility. However, since the Ksp is an equilibrium constant and does not depend on the volume, this change would not directly affect the calculated Ksp value.
c. The presence of 1.0 M NaCl (aq) in the CaSO4 solution would introduce additional chloride ions (Cl-) into the solution. These chloride ions can react with the calcium ions (Ca2+) from the CaSO4, forming soluble CaCl2. The solubility product constant (Ksp) only considers the concentration of calcium and sulfate ions, so the presence of excess chloride ions does not have a direct impact on the Ksp value.
d. If solid, soluble CaCl2 is present when the CaSO4 is being dissolved, it would introduce additional calcium (Ca2+) and chloride (Cl-) ions into the solution. These additional ions could react with the sulfate ions (SO42-) from the CaSO4, forming more CaSO4. This reaction would shift the equilibrium and increase the concentration of calcium and sulfate ions in the solution. Consequently, the Ksp value would be higher because the numerator (concentration of ions) would increase.
e. The end point of the titration being 2 mL before the equivalence point would imply that less titrant has been added compared to reaching the equivalence point. The equivalence point is the point at which the stoichiometrically equivalent amounts of reactants have been added, therefore representing complete reaction. Since the titration is stopped before complete reaction, there would still be some unreacted calcium and sulfate ions present, resulting in a lower concentration of these ions in the solution. Consequently, the Ksp value would be smaller because the numerator (concentration of ions) would decrease.