Before you come to lab, find the solubility product of silver(I) acetate. The es

Question

Before you come to lab, find the solubility product of silver(I) acetate. The estimate the quantity of silver(l) acetate solution that should consume a known quantity of 0.050 M KCl for each of the four different silver(I) acetate solutions. Take note of the quantity of silver ion solution required to consume the standard KCl solution. This relationship must be used to determine how the subsequent trials will be modified (if necessary). Set up a procedure for each solution so the data collected results in four significant figures, assumes using 5-, 10-, and 25-mL volumetric pipets for dispensing the KCl only, and requires a minimum volume of the saturated silver(I) acetate. For each solution: Determine the volume of standard KCl needed. Determine the theoretical volume of silver(l) acetate required to react with the KCl. Determine volume of silver(l) acetate that you will need to filter for buret rinsing and three trials. In your laboratory notebook, prepare a summary table for the quantities that meet the precision criteria noted above and indicate which volume of KCl you plan to use: Theoretical Ksp = AgC2H3O2(in water) Volume of KCl (for one trial) mL Volume of AgC2H3O2 (for one trial) mL Total volume of AgC2H3O2 mL AgC2H3O2 (in KNO3) etc.

Explanation / Answer

The solubility product of silver acetate ,KSp = S2

s= solubilty of Ag and acetate ions. note that both are univalent.

0.05 M of KCl = 0.05* 74.55 =3.73 g of KCl

as here all are univalent ions 0.05M of silver acetate needed = 167*0.05 = 8.35 g

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