Questions values, not affected by the different volumes of de-ionized water used
ID: 230019 • Letter: Q
Question
Questions values, not affected by the different volumes of de-ionized water used to prepare the saturated solution? 1. Why are the equilibrium concentrations of Ca and 10, in the saturated solution, and the ing reactant, Ca(NOsh or K1O,, in the preparation of Ca(IOs2 precipitate? ich ion, Ca? or IO,, would be present in excess if Ca(IOs2 was not properly rinsed during filtration to isolate the precipitate? 2. Which is the limit 3. Would the determined Kp values be lower or higher than expected if the precipitate of Ca(lO,)2 was not properly washed during filtration to isolate the precipitate? Explain. (Think carefully) Hint: Note that the calculation of Kp in this experiment was based on the titration results to determine molar concentrations of 10, in saturated solution. The presence of any ions that affect the solubility of Ca(lO)h and the concentration of 10, would affect the value of K During the filtration to separate the saturated solution from the excess solid, a student mistakenly wetted the filter paper and rinsed the precipitate on the filter paper. How would this error affect the value of Ki? Would it make the Kp value higher or lower than expected? Explain. 4.Explanation / Answer
1)
Ca(IO3)2---> Ca2+ + (IO3)2-
Ksp = [1S1] [ 2S2]
Ca(IO3) is least soluble in water and the equilibrium is slow, even if we have changed the volumes, it will not dissolute the ions that much. The dissolution will keep the stoichiometry ( 2 equivalents of iodate for ine Ca2+ ion) during the entire reaction.
There for concentration of calcium ions is half of the concentration of the iodate ions, so if either one of the concentaration of ions changed, the other also change. it will neglect the chnage.
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