For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pHat which you'd expect the highest solubility. You'll find Ke, data in the ALEKS Data tab.sp.Does solubilitychange withpH?highest solubilitycompoundpH = 2pH = 4pH = 5yesZnSnoyesMg Cl2noyesCaCl,noO OO OO O

Concept: Effect of pH on solubility: the effect of pH can be summarised as for ionic compounds…

Answered: For each of the following compounds,…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.26QAP

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For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find Ksp data in the ALEKS Data tab. compound Does solubility change with pH? highest solubility pH = 7 pH = 9 pH = 10 MgCl2 yes no BaOH2 yes no ZnS yes no huigp9ihb u
From the following data find the percentages of Na2CO3 and NaHCO3 in a mixture of these chemicals and inert constituents: a) A 0.5000 g sample required 45.50 mL 0.1050 N HCl to reach the methyl orange end point. b) 25.00 mL of 0.1000 N KOH is added to 0.2500 g of the sample; BaCl2 is added to precipitate the BaCO3 and 12.00 mL 0.1050 N HCl is required to reach the phenolphthalein end point.
How did diluting the buffer affect the pH of the buffer solution itself? ( pls explain it asap!) Thank you
Calculate the solubility of H2S in pure water. Ksp = 1x10-54 Ka1 = 6x10-8 Ka2 = 1,2x10-15
Compare the solubility of lead bromide in each of the following aqueous solutions: 0.10 M Pb(CH3COO)2 0.10 M NaBr 0.10 M KNO3 0.10 M NaCH3COO More soluble than in pure water. Similar solubility as in pure water. Less soluble than in pure water.
Predict the solubility and explain why: a) CdCO3 b) Na2S c) PbSO4 d) (NH4)3PO4 e) Hg2Cl2
Calculate the solubility at 25°C of CaF2 in pure water and in a 0.0060M NaF solution. You'll find Ksp data in the ALEKS Data tab. (CaF2 Ksp is 3.45×10−11 Round both of your answers to 2 significant digits. solubility in pure water: ? gL? solubility in 0.0060 M NaF solution:? gL?
51 mL of 0.060 M NaF is mixed with 17 mL of 0.15 M Sr(NO3)2. Calculate the concentration of F- in the final solution. Assume volumes can be added. (Ksp for SrF2 = 2.0×10-10) 0.038 M 0.0075 M 0.045 M 0.015 M 0.00012 M
Rank the solubilities (from least to most soluble) of BaCO3, CdS, NiCO3, AgCN, and SnS and explain specifically how this ranking was determined. Make sure to include details about the magnitude of Ksp (can be found in Appendix J of the OpenStax textbook) and what that indicates about solubility.
Q1.0 When 0.39 mol of solid CO2 is reacted with 0.23 mol of CH3MgBr in an ether solvent, the resulting product is isolated in aqueous solution (assuming 100% yield) and any excess CO2 is removed. Following this, 0.13 mol of HCl (aq) is added. What is the resulting solution's pH? Please note that you will need to research a pKa value for this query, and your answer should be reported to two decimal points.
2KMnO4 (aq) +5H2C2O4 (aq) + 3H2SO4 (aq) > 10CO2 (g) + K2SO4 (aq) +2MnSO4 (aq) + 8H2O (l) 90ml of 0.0150 M KMnO4 solution is mixed with 30 ml of 0.095 M H2C2O4 solution in a medium where there is excess sulfuric acid. Assume 100% yield Calculate the concentration of the following ions or molecules in the final solution a) Mn2+ b) K+ c) MnO4- d)H2C2O4
All three compounds are slightly soluble in water. For each compound determine the following: PbS Ksp = 8.4 x 10-28 | PbS04 Ksp = 1.8 x 10-8 Pb(103)2 Ksp = 2.6 x 10-13 a) Which compound would be the most (least) soluble and how do you know? b) Determine the solubility in moles/L for Pb(103)2. c) Calculate the number of grams of Pb(I03)2 dissolved in 1 L of solution? d) Is there a way to decrease the concentration of Pb2+(aq) ion in a solution containing PbS04? e) Calculate the concentration in moles/L of PbS04 in a saturated solution of the salt?

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