ective precipitation (which salts containing precipitating ion would you add and in what order) to purify wastewater contaminated with Ag+, Ba2+, Fe3+ and Na+. The purified water should only contain Na+ which is safe to drink

A solution is prepared by combining 20.00ml of 0.150 molar Ba2+ and 25.00ml of 0.125 molar Cl- Using concentrations and volumes above, determine if a precipitate will form when these solutions are mixed at 25C. Provide a calculation to support your answer, keep in mind the system is not at standard state.  Ba2+ (aq)    -560.77 kJ/mol Delta Gfo Cl- (aq)     -131.228 kJ/mol Delta Gfo BaCl2       -1296.32 kJ/mol Delta Gfo

a) The concentra=on of Mg2+ in seawater is 0.052 M. If the Ksp for Mg(OH)2 is 8.9 × 10–12, at what pH will >99.9% of the Mg2+ be precipitated from seawater as its hydroxide salt? b) The solubility of the ionic compound M2X3, having a molecular mass of 288 g/mol, is 3.60 × 10–7g/L. Calculate the Ksp of the compound.

Suppose that the solubility of calcium iodate are 2.5 g/L at 20oC and 5.5 g/L at 60oC. What are the solubility in mol/L at 20oC and at 60oC? How many milliliters (mL) of 0.045 M Na2S2O3 will be required to titrate a 10.0-mL sample of saturated Ca(IO3)2 solution collected at 20oC and 60oC, respectively?

10.00mL of 0.10M acetic acid were collected in an Erlenmeyer flask, and then diluted to 100mL with distilled water. After that, two drops of indicator were added. Then, the buret was filled with 0.100M NaOH. The titration was started by slowly adding NaOH to acetic acid. (Note: Ignore the volume of the indicator added, as the volume is tiny compared to 100mL.) What is the pH of the solution in the Erlenmeyer flask after adding 10.00mL of 0.100M NaOH?   Question 3 options:   7.22   6.9   8.35   7.00

If a student combines specific amount CaCl2. 9H2O and Na2CO3 and obtained a solid precipitate. The student dissolve 1.37 gram of CaCl2. 9H2O in 25.0 mL of water and 0.984 g of Na2CO3 in 25.0 mL of water.  The student is then combining the two solutions and observed the formation of a solid precipitate. The student filter the solution and recovered the precipitate. The following data were obtained for the experiment.   Initial Mass of CaCl2. 9H2O 1.37 g    Initial Mass of Na2CO3 0.984 g % yield of this experiment 87.4% 1. What is the balanced equation for this experiment?

The solubility of salts that contain the conjugates of weak acids increase in acidic solution. Given the reaction of CUCN (Ksp = 3.47 x 10-20) with an acid in the form H3O+ shown below, find the equilibrium constant for this reaction given that Ka HCN = 4.9 x 10-10. CUCN(s) + H:O*(aq) = Cu"(aq) + HCN(aq) + H2O(1)

A solution is titrated with AgNO, to determine the CI concentration. At the endpoint is a colloidal suspension of AgCl in a slight excess of Ag* and NO, ions. Which of the procedures would promote coagulation of the particles so that the precipitate can be filtered and weighed? heating the suspension adding more AGNO, solution cooling the suspension adding an electrolyte such as 0.1 mol HNO, adding more NaCl solution

A solution is prepared by mixing 20.0 mL of 0.100M Fe(NO3)3 with 20.0 mL of 0.00300M KSCN and 10.0 mL of DI water. Calculate the initial concentration of Fe^3+ in this solution? Give answer with correct amount of sig figs.

12b.