The Ksp for calcium iodate at 25℃ is 6.47 x 10-6. What is the molarity of iodate in a saturated solution of calcium iodate at 25℃?
The Ksp for calcium iodate at 25℃ is 6.47 x 10-6. What is the molarity of iodate in a saturated solution of calcium ioda...
1. Calculate the expected concentration of Ca2+ in saturated calcium iodate, ksp=6.47 x 10^-6. 2. Use this result to calculate the concentration of IO3- in saturated calcium iodate.
Suppose the solubility product constant of calcium iodate is 6.47 x 10-6. If the concentration of calcium iodate is 0.45 M. What would be the concentrations of Ca2+ and IO3- at equilibrium? Would this solution form a precipitate? Is the solution unsaturated, saturated, or supersaturated? Note* Ksp = [Ca2+][IO3-]2
Using the Ksp for calcium iodate hexahydrate, calculate the molarity of calcium ions. Using the Ksp for calcium iodate hexahydrate, calculate the molarity of iodide ions Ksp=7.10*10^-7. This is the reaction: Ca(IO3)2--->Ca+2IO3 I did an ice table, and using the Ksp of calcium iodate hexahydrate, I derived the solution as following: cuberoot(7.10*10^-7)/(4), the answer I got was .00561995. Since this is the value of S, twice that amount should be the Iodide ions, which is around .0112399. So did I...
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 =...
Q1) A) calculate the concentration of hydroxide in a saturated solution of calcium hydroxide (Ksp= 6.5*10^-6). B) what is the pH of the calcium hydroxide solution above?
A 10.00 ml sample of saturated calcium iodate in 0.0100 M potassium iodate was then titrated against the standardized sodium thiosilfate. The initial volume reading was 0.22 ml. The final volume reading was 17.33 ml. Calculate the solubility product constant for a saturated solution of calcium iodate dissolved in 0.0100 M potassium iodate
(6 points) The concentration of calcium in a saturated aqueous solution of calcium carbonate (CaCO3) at 25°C is 6.71x10-SM. What is the Ksp of this sparingly soluble salt? CaCO3(s) = Ca2+(aq) + CO32- (aq) Ksp = (Ca2+)( CO32-)
Calculate the molar solubility of Ca(IO3)2 in each solution below. The Ksp of calcium iodate is 7.1*10^-7. a) 0.070 M Ca(NO3)2 b).070 M NaIO3
1. The Molar Solubility of Ca(10), in Pure Water Temperature of the saturated solution of calcium iodate: Volume (or mass) of saturated calcium iodate solution titrated: 25 °C 10 ml (or g) Dat Trial 1 Trial 2 Trial 3 Volume of Na S o titrant Final buret reading Initial buret reading ml mL mL mL Net volume of Na So 26.621 mL 30.019 mL Calculated concentration of 10 Standardized 0.05 M sodium thiosulfate (Na,8,0,) solution (10,51(E) - TIL 10 mols.0.2...
1. The Molar Solubility of Ca(10), in Pure Water Temperature of the saturated solution of calcium iodate: Volume (or mass) of saturated calcium iodate solution titrated: 25 °C 10 ml (or g) Dat Trial 1 Trial 2 Trial 3 Volume of Na S o titrant Final buret reading Initial buret reading ml mL mL mL Net volume of Na So 26.621 mL 30.019 mL Calculated concentration of 10 Standardized 0.05 M sodium thiosulfate (Na,8,0,) solution (10,51(E) - TIL 10 mols.0.2...