186 Experiment 7 Solubility Product Constant of Copper (II) lodate 4. The slightly soluble salt AB, ionizes as shown. (1) AB2 (s) A2+ (aq) + 2B (aq) When a solution of CX is titrated into a saturated solution of AB2, the equivalence point is reached when B is completely consumed by the added C2+ ion. (2) C2+ (aq) + 2 B (aq) CB2 (aq) It takes 5.00 mL of 0.10 M CX solution to reach the equivalence point when titrated into a 20.0 mL saturated AB, solution. Refer to the Introduction and Data Sheet to solve the following problems: a) Refer to equation 1 above and write the K expression for AB2 in terms of the ion concentrations and in terms of the molar solubility, s. b) Calculate how many moles of C2+ were titrated to reach the equivalence point. c) Based on your result to part b, calculate the number of moles of B in the saturated AB, solution. Consider the stoichiometry of equation 2. d) Based on your result to part c, calculate the number of moles of AB, in the saturated solution. Consider the stoichiometry of equation 1. e) Based on your result to part d, calculate the molar solubility, s, of AB. f) Based on your result to part e, calculate the Kp value for AB,

186 Experiment 7 Solubility Product Constant of Copper (II) lodate 4. The slightly soluble salt AB, ionizes as shown. (1) AB2 (s) A2+ (aq) + 2B (aq) When a solution of CX is titrated into a saturated solution of AB2, the equivalence point is reached when B is completely consumed by the added C2+ ion. (2) C2+ (aq) + 2 B (aq) CB2 (aq) It takes 5.00 mL of 0.10 M CX solution to reach the equivalence point when titrated into a 20.0 mL saturated AB, solution. Refer to the Introduction and Data Sheet to solve the following problems: a) Refer to equation 1 above and write the K expression for AB2 in terms of the ion concentrations and in terms of the molar solubility, s. b) Calculate how many moles of C2+ were titrated to reach the equivalence point. c) Based on your result to part b, calculate the number of moles of B in the saturated AB, solution. Consider the stoichiometry of equation 2. d) Based on your result to part c, calculate the number of moles of AB, in the saturated solution. Consider the stoichiometry of equation 1. e) Based on your result to part d, calculate the molar solubility, s, of AB. f) Based on your result to part e, calculate the Kp value for AB,

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...

See similar textbooks

Similar questions

Every year Every second (1 year 365 days).
) Ph CO0OH 2) EALI, H30* 3)PCC
Which one of the following is an intensive property? O density O mass O heat content O volume O moles
Agar plates typically contain 1.5% agar by weight. To make 500 ml of TSA, how many grams of agar would you add to your flask before filling it with TS broth for a total volume of 500 ml? (Assume the density of TS broth is the same as H2O).
Which molecules are enantiomers? Which molecules are the same? (A). H Br
A sample of volume 270 cm³ has a mass of 0.645 kg. (a) What is the density of the sample? (b) Is the material gaseous or condensed? g/cm3
3. Now that you know the physical state of each of the reactants and products in this chemical reaction lets think about what you might observe as the reaction is running. CH_3COOH(aq) + NaHCO_3(aq) → H_2O(l) + CO_2(g) + CH_3COONa(aq) Upload a screenshot that shows how you performed all the calculations in Q3.
40 X x 2008 xample 8. The laboratory reagent, concentrated nitric acid, is generally 69 per cent by mass of nitric acid (HNO3). Calculate volume of this solution which contains 19.9 g of HNO3 (density of concentrated nitric acid solution is 1.41 g cm -3). If th I of II
sodium is not kept in a petrol b k oil c n hexane d water
Which piece of equipment would you use to measure 7.10 mL of CuSO4 (aq)?
A chemist prepares a solution of silver(I) nitrate AgNO3 by measuring out 6.4102 x 10^2 μmol of silver(I) nitrate into a 450.mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's silver(I) nitrate solution. Round your answer to 2 significant digits.
A chemist prepares a solution of iron(III) bromide (FeBr,) by weighing out 45.48 g of iron(III) bromide into a 350. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in g/dL of the chemist's iron(III) bromide solution. Round your answer to 3 significant digits. alo x10 dL Ar ?