For full marks in the following questions, you must provide the Ksp algebraic expression and all relevant chemical equations including source equations.
For full marks in the following questions, you must provide the Ksp algebraic expression and all...
The solubility of Ce(IO3)3 in a 0.14-M KIO3 solution is 1.3 x 10-7 mol/L. Calculate Ksp for Ce(IO3)3 - Ksp = Submit Answer Try Another Version 10 item attempts remaining Which of the following two compounds is expected to be more soluble in acidic solution than in pure water? a. Agi AgNO2 b. Mn(NO3) Mn(CN)2 Submit Answer Try Another Version 10 item attempts remaining Calculate the solubility of solid Ca3(PO4)2 (Ksp = 1.3x10-32) in a 0.16 M Na3PO4 solution. S...
1)Use the virtual lab to determine the solubility product (Ksp) for the following solids. Show all work for credit. *should be able to use the lab to determine the ion concentrations at equilibrium and use these for the formulas for KSP and then the KSP'S for solubility. The lab is just to help you get the ion concentration (a). AgCl (b). SrSO4 (c). Ag2CO3 (d). Sr(IO3)2 2) What is the solubility of the solids listed in question 1, in moles/liter?...
A saturated solution of calcium iodate contains 2.37 g/L of Ca(IO3)2. (a) What is the solubility of calcium iodate in mol/L? (b) What are the concentrations of Ca2+ and IO3 – ion, respectively, in the saturated solution? (c) Calculate the Ksp value for Ca(IO3)2. Part b ) Silver ion, Ag+ , readily forms complex ion, Ag(S2O3)2 3– , with thiosulfate, S2O3 2– , according to the following equation: Ag+ (aq) + 2S2O3 2– (aq) ⇌ Ag(S2O3)2 3– (aq); Kf =...
The Ksp for lead chloride (PbCl2) is 1.6 x 10. Calculate the solubility of lead chloride in each of the following a. water Solubility mol/L b. 0.11 M Pb(NO3)2 Solubility= mol/L c. 0.011 M NaCl Solubility mol/L
13.54 Describe how you would prepare each of the following aque- ous solutions: (a) 1.50 L of 0.110 M (NH4)2SO4 solution, starting with solid (NH4)2SO4; (b) 225 g of a solution that is 0.65 m in Na2CO3, starting with the solid solute; (c) 1.20 L of a solution that is 15.0% Pb(NO3) 2 by mass (the density of the solution is 1.16 g/mL), starting with solid solute; (d) a 0.50 M solution of HCI that would just neutralize 5.5 g...
Solubility Product of Calcium Hydroxide Post-Lab Questions (40 Points) 1. A. Determine the molar solubility of PbI2. The Ksp values for PbI2 is 8.7 x 10-9. B. Determine the molar solubility of 100 mL of a solution of PbI2 to which 0.01 mole of lead nitrate, Pb(NO3)2 has been added. Assume the total volume remains at 100 mL. C. The molar solubility of cadmium hydroxide, Cd(OH)2 is 1.842 x 10-5 M. What is the Ksp value of cadmium hydroxide?
to answer number 28. you refer back to 24. but im stuck on it ans confused. 2NaC1 HOH c. + MgC12 + H2S04> Na2S04+2HCI d. Ca(OH)2+ Pb(NO3)2> Ca(NO3)2 + Pb(OH)2 3 parts) What is the H+ concentration and pH of a 0.20 M solution of hypochlorous acid, Ka 3.5 x 10*? (SHOW ALL STEPS FOR CR CONC. AND SOLVE FOR 22.pH ) 20. ICE CHART, sOLVE FOR 21 23. What is the hydroxide ion concentration and pH of a 0.10...
Muyuulin (1JJ. Part III: Determination of a Solubility Product In Part Ill you will prepare a saturated solution of silver carbonate (Ag2CO3) and deten solubility product constant of Ag2CO3. Ag2CO3(s) = 2 Agt(aq) + CO32-(aq) (17) In making the solution, 1.0 mL of 0.10 mol/L AgNO3 will be added to specified volume mol/L Na2CO3. The limiting reagent in this reaction will be the silver ions. Use of an excess an of anion allows for a relatively simple calculation of the...
Ksp = [Ba²+][10,1 2. 10. mL of 0.10 M Ba(NO), is mixed with 10. mL of 0.10 M KIO,, a precipitate forms. for barium a. Which ion will still be present at appreciable concentration in the equilibrium mixture if K iodate is very small? b. What would that concentration be? 3. Lead chloride, PbCly, is slightly soluble with K equal to 1.7 x 10. a. What is the solubility of lead chloride in pure water? b. What would the solubility...
The Ksp of Ca3(PO4)2 is 1x 10-33. What is the solubility in moles per liter (mol/L) of Ca3(PO4)2 (s) in a 0.01 M Ca(NO3)2 (aq) solution? (Note: The molar mass of Ca3(PO4)2 is not needed in this problem, which asks for moles per L.) a. 3.2 x 10-14 mol/L b.3.0 x 10-15 mol/L c. 9.8 x 10 mol/L d. 1.6 x 10-14 mol/L e. 5.0 x 10-32 mol/L