The answers to these two questions must be calculated accurately to at least three decimal places. Use the Extended Debye-Hückel equation to calculate the activity coefficient of Ca2+ in a solution of ionic strength = 0.0083 M at 25 °C. Y 0695 Submit Alwer Incorrect. Tries 3/5 Previous Tries Now, determine a value for this same activity coefficient by linear interpolation from the values listed in Table 7-1, D.C. Harris, "Quantitative Chemical Analysis", 8th ed.

The answers to these two questions must be calculated accurately to at least three decimal places. Use the Extended Debye-Hückel equation to calculate the activity coefficient of Ca2+ in a solution of ionic strength = 0.0083 M at 25 °C. Y 0695 Submit Alwer Incorrect. Tries 3/5 Previous Tries Now, determine a value for this same activity coefficient by linear interpolation from the values listed in Table 7-1, D.C. Harris, "Quantitative Chemical Analysis", 8th ed.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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3
What is the solubility of Mn(OH)2 at a pH of 11.37? Ksp(Mn(OH)2) = 1.200e-11.
What is the solubility of Cd(OH)2 at a pH of 11.08? Ksp(Cd(OH)2) = 5.000e-15.
Calculate the ionic strength of 0.00041 M La(IO3)3. Assume complete dissociation at this low concentration and no hydrolysis reaction to form LaOH²+. μ = M
A chemist mixes 10.0 mg of Ca(NO3)2 to a 100.0 mL sample of 0.010 M Na2C2O4 at 25 oC. Assume the volume of solution does not change. Given that for CaC2O4, Ksp = 2.7 x 10-9 at 25 oC, determine a) the value of Qsp (number and magnitude) of CaC2O4 dissolution and b) whether a precipitate should form.
The Ksp for an ionic solid, AB2, is 3.559*10-11. Calculate the molar solubility, in µM, of this ionic solid in a solution of 0.013 M A+ ions. Recall, 106 µM = 1 M.
For nos. 4 - 7: Consider a saturated solution of barium iodate in 0.025 M BaCl2. For the salt: Ba(1O3)2(s) Ba2+ + 2103 Ksp = 1.57 x 10-9 at 25°C %3D
Calculate the solubility at 25°C of CuBr in pure water and in a 0.0060M CoBr2 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits.
5 Activity Coefficients at Different lonic Strengths What is the activity coefficient for each ion at the given ionic strength at 25 °C? Activity coefficients at various ionic strengths can be found in this table. [1-] = X 3 8.9x10^-14 4 CrO42 (μ = 0.05) y = X 0.35 (CH3CH2)2NH (μ = 0.05 M) Y = Find the concentration of I in 0.0010 M AgNO3 saturated with Agl. Include activity coefficients in the solubility-product expression. The Ksp of Agl is 8.3x10-17. Refer to the table of activity coefficients at various ionic strengths as needed. Enter as scientific notation. X 0.77 Mail
3. Including activity coefficients, find the concentration of Ba2+ in a 0.050 M (CH3)4N+IO3 solution saturated with Ba(IO3)2 (Ksp = 1.5 x 109). Consider that the solubility of Ba(IO3)2 is small, and it contributes negligible IO3 to 0.050 M (CH3)4NIO3. -
Calculate the ionic strength of a saturated solution of La(IO3)3 with 0.010 M La(NO3)3. Kp = 1.0 x 10-I| 9.05 x 10- 6.05 x 10-2 4.68 x 10-3 1.21 x 10- 9.36 x 10-3