a. Calculate the solubility of PbI2 (Ksp = 1.5 × 108) in moles per liter. Ignore any acid-base properties.S =mol/Lb. Calculate the solubility of CdC03 (Ksp = 5.3 × 10-12) in moles per liter. Ignore any acid-base properties.S =mol/Lc. Calculate the solubility of Sr3 (PO4)2 (Ksp = 1.5 × 10¬8) in moles per liter. Ignore any acid-base properties.-31S =mol/L

Answered: Image /qna-images/answer/c5d0970e-cec0-4da5-9938-d23ca5d92b07.jpg

a. Calculate the solubility of PbI2 (Ksp = 1.5 × 10¬8) in moles per liter. Ignore any acid-base properties. S = mol/L b. Calculate the solubility of CdCO3 (Ksp = 5.3 × 10-12) in moles per liter. Ignore any acid-base properties. S = mol/L c. Calculate the solubility of Sr3 (PO4)2 (Ksp = 1.5 × 10-81) in moles per liter. Ignore any acid–base properties. S = mol/L

a. Calculate the solubility of PbI2 (Ksp = 1.5 × 10¬8) in moles per liter. Ignore any acid-base properties. S = mol/L b. Calculate the solubility of CdCO3 (Ksp = 5.3 × 10-12) in moles per liter. Ignore any acid-base properties. S = mol/L c. Calculate the solubility of Sr3 (PO4)2 (Ksp = 1.5 × 10-81) in moles per liter. Ignore any acid–base properties. S = mol/L

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter7: Solutions And Colloids

Section: Chapter Questions

Problem 7.39E

See similar textbooks

Similar questions

-The solubility of Ag3PO4 is measured and found to be 1.99×10-3 g/L. Use this information to calculate a Ksp value for silver phosphate.Ksp = -The solubility of Zn(CN)2 is measured and found to be 1.45×10-2 g/L. Use this information to calculate a Ksp value for zinc cyanide. Ksp = Please help. Thank you.
1. An acid solution is prepared by dissolving 19.264 grams of pure KHC2O4.H2C2O4.2H2O in water and diluting to exactly 900 ml. Fifty milliliters (50.00 mL) of this solution are neutralized by 35.00 ml. of KOH solution. What is the normality of each solution? 2. What mass of Ca(OH)2 is present in a sample if it is titrated to its equivalence point with 44.02 mL of 0.0885 M HNO3? The balanced chemical equation is as follows: 2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H2O ; Balanced.
One of your friends who likes gardening is attempting to make a solution that will increase some trace nutrients while also making the soil less acidic.* The planned solution will have the following concentrations: 0.03 M NaOH 0.008 M CaCl2 8 x 10-12 M Fe(NO3)2 You're going to help your friend out by checking to see if anything will precipitate out of this solution. Your friend is particularly worried about Ca(OH)2 [Ksp = 6.5 x 10-6] and Fe(OH)2 [Ksp = 7.9x10-16]. Your friend thinks they have done the math correctly so that no precipitates will form, but they don't know anything about ionic strength corrections.(NOTE: Assume molality = molarity. There's probably not much of a difference.) a) Calculate the ionic strength of the solution. b) Calculate the activity of hydroxide ions, aOH- c) Calculate the activity of Ca2+ ions. d) Calculate the activity of Fe2+ ions.
An unknown 36% v/v monohydroxide reagent has a density of 1.8 g/mL. Zeus wanted to determine the identity of this base, so he transferred a 90.916-mL aliquot of the base to a 1.0 L volumetric flask and diluted it up to mark. He then titrated the base solution and found out that its concentration is 1.0 M.a. What is the molarity of the base solution after dilution? b. If this 1.00M solution is used in the analysis of PLA (Polylactic Acid) plastics for lactic acid (H2Lactate) titration, what is its concentration in titer mg LA/mL titrant? (Lactic Acid: 90.08 g/mol)c. What is the molarity of the unknown monohydroxide reagent?d. What is the molar mass of the unknown monohydroxide reagent?(Density of H2O = 0.99707 g/mL)Hint: Mass of solution = mass of solvent + mass of solutee. What is the identity of the unknown monohydroxide reagent?
53.2 mL of 0.795 M hydroiodic acid is added to 46.2 mL of barium hydroxide, and the resulting solution is found to be acidic. 28.5 mL of 0.695 M sodium hydroxide is required to reach neutrality. What is the molarity of the original barium hydroxide simulation? ___ M
RESULTS AND CALCULATIONS: Standardization of NaOH solution 1.trial 2.trial 15.0 mL of 0.1015 M HCl + 15.3 mL NaOH 15.0 mL of 0.1015 M HCl + 15.2 mL NaOH Calculation of the average molarity of NaOH solution;
4,Titrate 0.5687g of solid KHP (KC8H5O4) requires 13.52 mL of an unknown NaOH solution to reach the equivalence point. What’s the molarity of this unknown NaOH solution? Show your work. Group of answer choices A, 0.254 B, 2.36 C, 0.126 D, 0.206 5,Titrate 35.00 mL of 0.156 M KHP solution requires 25.75 mL of an unknown NaOH solution to reach the equivalence point. What’s the molarity of this unknown NaOH solution? Group of answer choices A, 2.01 B, 0.235 C, 1.203 D, 0.212
A technician would like to standardize an unknown Ca(OH)2 solution. It takes 22.41 mL of a 0.155 M solution of HCl to titrate 25.00 mL the unknown Ca(OH)2 solution. Calculate the molarity of the Ca(OH)2 solution. Tip: Don't forget to consider the mole ratio between HCl and Ca(OH)2.
75 ml of 0.100M of thiosulfate, 100ml of distilled water mixed with 10ml 10% bleach, 6M OF HCl equation 2) I2 (aq) + 2 Na2S2O3 (aq) → 2 NaI (aq) + Na2S4O6 (aq) equation1) NaOCl (aq) + 2 Kl (aq) + 2 HCl (aq) → I2 (aq) + 2 KCl (aq) + NaCl (aq) + H2O (l)
Balanced eqation: 2 H3PO4 + 3 Ca(OH)2 → 6 HOH + Ca3(PO4)2 What is the molar concentration of 325.25 mL H3PO4 is needed to reach the equivalence point with 475.60 mL of 0.465 M Ca(OH)2?
How to prepare these solutions? 250.0 mL 0.125 M stock Na2S2O3 solution from Na2S2O3·5H2O crystals 250 mL 0.10 M NaOHNOTE: Use the 1.0 M NaOH prepared250.0 mL standard 2500 ppm Cu(II) stock solutiona. Weigh and dissolve appropriate amount of Cu(NO3)2·5H2O crystals in enough distilled water.
Dr. Donwonree tried to determine the vitamin C content in apple juice which he bought at CheMarket. He measured out 50.0 mL of the juice and added the HCl, KI, and starch. Then he started the titration by adding KIO3 solution into the juice. The concentration of the KIO3 solution was 0.200 M and it took only 1.50 mL of KIO3 to reach the endpoint. How much vitamin C (mg) is contained in 1.00 L of this apple juice?