CaF2 dissolves as follows:
Hence, given that the solution is saturated, the equilibrium constant Ksp of the above reaction can be written as
Note that CaF2 concentration does not appear in the equilibrium expression as it is a pure solid with concentration unity.
Now, it is given that the concentrations are
Hence, Ksp for CaF2 can be calculated as
Hence, the Ksp value calculated for CaF2 is . ( rounded to three significant figures).
tion 12 of 27 > In a saturated aqueous solution of CaF , the calcium ion...
A student measures the Ca2+ concentration in a saturated aqueous solution of calcium fluoride to be 2.18x10-6 M. Based on her data, the solubility product constant for calcium fluoride is Submit Answer Retry Entire Group 9 more group attempts remaining
55. In a saturated solution of calcium fluoride, the concentration of the calcium ions is measured to be 2.4x10 M. What is the solubility product of calcium fluoride? 5.1 x 10 (1) 5.7 x 10 (2) 5.7 x 10-10 (3) (4) 5.5 x 101 (5) 2.4 x 10
1. The concentration of Ag+ ion is a saturated aqueous solution of Ag2CrO4 was found potentiometrically equal to 1.56 x 10-4 M. Calculate the solubility in grams per liter and its solubility product. 2. The solubility product of a compound with a general formula M2X was found equal to 3.58 x 10-13 on the basis of solubility measurements and on the assumption that the ions formed are M7 and X-2. A more careful determination of the ionic species determined that...
QUESTION 6 (15 points) A) A saturated solution of calcium fluoride CaF2 is found to contain a concentration of fluoride ions [F] = 3.0 x 10-6 M. What is the value of the solubility product of this salt?
A student measures the F- concentration in a saturated aqueous solution of barium fluoride to be 1.46×10-2 M. Based on her data, the solubility product constant for barium fluoride is .
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...
4. The pH of a saturated aqueous solution of zinc ammonium phosphate (ZnNH4P04) is 7.20, whereas the concentration of the zinc ion in the solution is 8.4 x 10-5 M. Calculate the solubility product of ZnNH4PO4. 5. What is the minimum concentration of excess Agt required to quantitatively precipitate (99.9%) oxalate from a 0.0303 M NaC204 solution buffered at pH 4.00 6. Calculate the molar solubility of Ag2CrO4 in a) water, b) 0.050 M Na2CrO4, c) 0.050 M AgNO3. (Disregard...
Given the average concentration of calcium ion in natural water is 3.8×10^-4 M, and that the solubility product Ksp for CaF2 is 4×10^-11, calculate the maximum molar concentration of fluoride ion. Find the concentration fluoride in ppm scale as well.
1. The equilibrium concentration of zinc ion in a saturated zinc carbonate solution is M. Concentration of zinc ion is 2.5x10^-10 2. A student measures the Br- concentration in a saturated aqueous solution of lead bromide to be 2.27×10-2 M. Based on her data, the solubility product constant for lead bromide is
Write a solubility product constant expression, K_sp, for an equilibrium in a saturated aqueous solution of the slightly soluble salts Magnesium fluoride, MgF_2 Zinc phosphate, Zn_3(PO_4)_2 Chromium(II) hydroxide, Cr(OH)_3 Strontinum sulfate, SrSO_4. Calculate the solubility in g/L for calcium carbonate, CaCO_3, in pure water given the K_sp = 2.8 times 10^-9. Calculate the solubility in g/L for CaCO_3, in 0.050 M Na_2CO_3.