Practice Exercises: (17.51) 45 mL of 0.0015 M Barium Chloride is mixed with 75 mL off 0.0025M Potassium Fluoride. Predict if the mixture will form a precipitate or not by using the "ion-product" comparison with the Ksp. Given that the Ksp for BariumFluoride is given as 1.0 x 10-6
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- 1. How many g of Ag2CrO4 will precipitate when 86 mL of 0.200M AgNO3 is added to 50mL of 0.3 M K2CrO4 ? Show short method of solvingWe received 15000 Ci of 28Mg, present as Mg(NO3)2 and want to dissolve is in 10 mL water at pH8. Will we form a precipitate or will the solid entirely dissolve? Only typed solutionIf you had used 40mL of wash water to was .8555g of AgCl precipitate, and yhe wash water became 60% maximum saturation, how many grams of AgCl would you be washing away? Ksp for AgCl=1.8x10^-10 what % error too low would be in ur final answer, ie what % of the solid would be washed away
- When 40.0 mL of 0.0800 M Sr(NO3)2 and 80.0 mL of0.0500 M KF are mixed, a precipitate of strontium fluoride (SrF2) is formed. The solubility product Ksp of strontium fluoride in water at 25°C is 2.8 × 10-9. Calculate the [Sr2+] and [F-] remaining in solution at equilibrium.A solution is prepared by mixing 150.0 mL of 0.150 mol/L iron(II) nitrate and 100.0 mL of 0.340 mol/L sodium fluoride. Will a precipitate form? Use ICE table.If 21 mL of 3.2 x 10–5 M magnesium chloride and 15 mL of 1.5 x 10–4 M sodium fluoride are mixed, what are the concentrations of magnesium chloride and sodium fluoride after mixing? Keep an extra sig fig. Question 8 options: sodium fluoride magnesium chloride 1. 1.87 x 10–5 M 2. 3.73 x 10–5 M 3. 6.25 x 10–5 M 4. 1.25 x 10–4 M 5. 1.50 x 10–4 M
- The solubility of PbBr2 is 0.00101 M. What is the solubility product, Ksp for PbBr2. Report answer in scientific notation with one place past the decimal point.When we mix together, from separate sources, the ions of a slightly soluble ionic salt, the salt will precipitate if Qsp _____ Ksp, and will continue to precipitate until Qsp _____ Ksp.Will a precipitate of BaSO4 form when 200.0 mL of 0.000515 M Ba(NO3)2 is added to 150.0 mL of 0.000825 M Na2SO4? Ksp= 1.08x10-10=(Ba2+)(SO42-) True if precipitate forms or false if precipitate does not form
- The solubility product constants of PbSO4 and SrSO4 are 6.3 * 10-7 and 3.2 * 10-7, respectively. What are the values of [SO42-], [Pb2+], and [Sr2+] in a solution at equilibrium with both substances?What is the possible precipitate if 21 mL of 3.2 x 10–5 M magnesium chloride and 15 mL of 1.5 x 10–4 M sodium fluoride are mixed? Question 7 options: MgCl2 MgF NaCl2 MgF2 NaCl Answer and ExplainLead(II) carbonate, PbCO3, is one of the components of thepassivating layer that forms inside lead pipes. (a) If the Kspfor PbCO3 is 7.4 x 10 - 14 what is the molarity of Pb2+ ina saturated solution of lead(II) carbonate? (b) What is theconcentration in ppb of Pb2+ ions in a saturated solution?(c) Will the solubility of PbCO3 increase or decrease as thepH is lowered? (d) The EPA threshold for acceptable levelsof lead ions in water is 15 ppb. Does a saturated solution oflead(II) carbonate produce a solution that exceeds the EPAlimit?