To determine the Ksp of barium oxalate at 12°C, a 100.0 mL saturated solution was prepared by adding the solid in distilled water maintained at 12°C until it no longer dissolves. The solution was filtered and from this, a 10.0 mL aliquot of the filtrate was drawn. It was found out that 10.70 mL of 5.60 x 104 M HCI was used to reach the endpoint.

To determine the Ksp of barium oxalate at 12°C, a 100.0 mL saturated solution was prepared by adding the solid in distilled water maintained at 12°C until it no longer dissolves. The solution was filtered and from this, a 10.0 mL aliquot of the filtrate was drawn. It was found out that 10.70 mL of 5.60 x 104 M HCI was used to reach the endpoint.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 29QRT

See similar textbooks

Similar questions

A solution of NaF is added dropwise to a solution that is 0.0614 M in Mg2+ and 3.53e-05 M in Y³+. The Ksp of MgF₂ is 5.16e-11. The Ksp of YF3 is 8.62e-21. (a) What concentration of F" is necessary to begin precipitation? (Neglect volume changes.) [F"] = M. (b) Which cation precipitates first? O Mg2+ O y3+ (c) What is the concentration of F" when the second cation begins to precipitate? [F] = M.
Lead(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?
To determine the Kgp of barium oxalate at 12°C, a 100.0 mL saturated solution was prepared by adding the solid in distilled water maintained at 12°C until it no longer dissolves. The solution was filtered and from this, a 10.0 mL aliquot of the filtrate was drawn. It was found out that 10.70 mL of 5.60 x 104 M HCI was used to reach the endpoint. Given that two moles of HCl react for every mole of dissolved oxalate during the titration, determine the amount of dissolved oxalate in the titration flask (in mol/L). Do not include the unit in your answer below. For those who will be using scientific notation, please follow the format below: Example: 0.00487 -> 4.87E-3 58000 -> 5.8E+4
A 725 mL sample of a saturated aqueous solution of calcium oxalate, CaC2O4, at 95°C is cooled to 13°C. How many milligrams of calcium oxalate will precipitate? For CaC₂O4, Ksp = 1.2 x 10-8 at 95°C and 2.7 x 10-⁹ at 13°C
The aqueous solubility of AgOCN at 20°C is 7.00 mg/100mL. What is the Ksp of AgOCN at 20°C?
1a) Calculate the molar solubility of CrF3 (Ksp = 6.6 x 10-11) in a 0.015 M CrCl3solution.
FeS has a Ksp of 3.72 x 10-19. What is the molar solubility of FeS? Write your answer to 3 sig figs, in the format 1.23E-4.
Solubility tests of benzoic acid with a dissolution enthalpy of -32kJ / mol were performed at 2 different temperatures. In the first experiment carried out at 27 ° C, 5 mL of the sample taken from the benzoic acid solution is taken into 25 mL of water and titrated with 0.02M NaOH. As a result of the titration, there is 8 mL consumption, respectively. In the second experiment performed at a different temperature under the same conditions, 22 mL was consumed. Taking advantage of these results a) What is the solubility of benzoic acid at 27 ° C? b) What is the solubility of benzoic acid at different temperatures? c) What is the second test temperature? (M (benzoic acid): 122.12 g / mol)
The Ksp of Ba(IO3)2 at 25 °C is 6.0 * 10-10. What is the molar solubility of Ba(IO3)2?
What is the molar solubility (in mol L-1) of a salt in pure water with general molecular formula MX2 (where M is a cation and X is an anion) that has Ksp = 5.01 x 10-10 ?
You have a solution containing (7.0x10^-1) mol L1 F ions and (1.0x10^-1) mol L-1 SO.2- ions. To this solution you gradually add solid Ba(NO3)2 to precipitate the anions. Determine the concentration of SO42 (in mol L) when BaF2 just starts to precipitate. Assume negligible volume change. (Ksp(BaF2) = 2.45 x 10-5; Ksp(BaSO4) = 1.07 x 10-10) %3D %3D Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: M x10 Answer units
Tooth enamel is composed of hydroxyapatite, whose simplest formula is Ca5(PO4)3OH, and whose corresponding Ksp = 6.8 * 10-27. As, fluoride in fluorinated water or in toothpaste reacts with hydroxyapatite to form fluoroapatite, Ca5(PO4)3F, whose Ksp = 1.0 * 10-60. Write the expression for the solubility-constant for hydroxyapatite and for fluoroapatite.