A solution containing 0.01000M Ba+2 and 0.01000M Ca+2 is treated with N aIO3 until [Ba2+] = 1.00 × 10−5M. What is the concentration of Ca2+ at this point?
A solution containing 0.01000M Ba+2 and 0.01000M Ca+2 is treated with N aIO3 until [Ba2+] =...
What chemical is used to separate Ca2+ and Ba2+ ions from a solution containing Ca2+, Ba2+, NH4+, and K+ ions? What are the products of the Ca2+ and Ba2+ ions with this chemical?
At what Ca2 solution containing 10 M PO3? Express the Ca concentration in mg/L Ca and in mg/L as CaCO3. Ignore aqueous complex formation 5. concentration will precipitation of Ca,(PO)2(s) (pKap 26.0) occur in a
4) A sample of 0.670 g of an unknown compound containing barium ions (Ba2*) is dissolved in water and treated with an excess of NA2SO4. If the mass of the BaS04 precipitate formed is 0.4105 g, what is the percent by mass of Ba in the original compound?
A solution containing a mixture of 0.0441 M 0.0441 M potassium chromate ( K 2 CrO 4 K2CrO4 ) and 0.0513 M 0.0513 M sodium oxalate ( Na 2 C 2 O 4 Na2C2O4 ) was titrated with a solution of barium chloride ( BaCl 2 BaCl2 ) for the purpose of separating CrO 2− 4 CrO42− and C 2 O 2− 4 C2O42− by precipitation with the Ba 2+ Ba2+ cation. The solubility product constants ( ? sp Ksp...
you add an excess of ca(oh)2 to water maintained at particular temperature, stir until the solution is saturated, filter, then determine the OH in the solution by titration with acid. titration of 10.0 ml of the calcium hydroxide solution to the end point requires 4.86 ml of 0.070 M HCl solution. what is the molar quantity of OH- in the 10.0 ml of solution? what are the concentrations of Ca2+ and OH- ? WHAT IS THE SOLUBILITY OF Ca(OH)2 under...
Sodium sulfate is slowly added to a solution containing 0.0500 M Ca (aq) and 0.0340 M Ag (aq). What will be the concentration of Ca2 (aq) when Ag, SO,(s) begins to precipitate? Solubility-product constants, Ksp. can be found in the chempendix. Ca = M What percentage of the Ca2 (aq) can be precipitated from the Ag (aq) by selective precipitation? percentage:
A sample of 0.7360 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2CO3. If the mass of the BaCO3 precipitate formed is 0.7578 g, what is the percent by mass of Ba in the original unknown compound?
A solution containing a mixture of metal cations was treated as outlined. Dilute HClHCl was added and no precipitate formed. H2SH2S was bubbled through the acidic solution. A precipitate formed and was filtered off. The pH was raised to about 99 and H2SH2S was again bubbled through the solution. A precipitate formed and was filtered off. Finally, sodium carbonate was added to the filtered solution and no precipitate formed. What can be said about the presence of each of these...
Please help! Will rate. A 50.0 mL sample containing Cd2+ and Mn2+ was treated with 56.5 mL of 0.0600 M EDTA. Titration of the excess unreacted EDTA required 13.3 mL of 0.0100 M Ca. The Cd2t was displaced from EDTA by the addition of an excess of CN. Titration of the newly freed EDTA required 11.2 mL of 0.0100 M Ca2+. What are the concentrations of Cd2+ and Mn2+ in the original solution? M Mn2+ concentration: M Cd2 concentration: A...
Consider a solution that is 1.3×10−2 M in Ba2+ and 1.8×10−2 M in Ca2+. Ksp(BaSO4)=1.07×10−10 Ksp(CaSO4)=7.10×10−5 *Part A: If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? A) Ba2+ (ANSWER) B) Ca2+ *Part B: What minimum concentration of Na2SO4 is required...