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 K,, data in the ALEKS Data tab.spcompoundDoes solubilitychange withpH?highest solubilitypH = 9pH = 8pH = 6yesBaCO3O no○ yesPbF₂O○ no○ yesCuBr○ noOX0G

To determine whether the solubility of a compound changes with pH, we need to consider the effect of…

Answered: For each of the following compounds,…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter12: Gravimetric Methods Of Analysis

Section: Chapter Questions

Problem 12.33QAP

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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
you want to separate Ni2+ and Mn2+ by precipitating the corresponding sulphidesfrom each other. What pH value must you set so that one of the twometals is precipitated quantitatively (concentration in the solution less than/equal to 10/-5 mol/l)is precipitated while the other is still in solution? Ksp (NiS): 10^-21, Kps (MnS): 10~15; Ks (H2S): 10 ~- 20,Saturation concentration of H2S in water: 0.1 mol/l
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
Calculate the Molar Solubility and Ksp of Borax. I have included the data and some calculation that can help with solving, but I am unsure if the calculation I have provided are accurate Data: 1. Concentration of standardized HCl Solution (mol/L) = 0.1563M 2. volume of saturated borax (mL) = 5 mL 3. Buret reading, initial (mL) = 24.60 mL 4. Buret reading, final (mL) = 29.53 mL 5. Volume of HCl added (mL) = 4.93mL Calculations: 6. Amount of HCl added (mol) = 0.00077mol 7. Amount of OH- in saturated solution (mol) = 8. [OH-] equillirium (mol/L) = Molar solubility of borax=? Ksp of borax=?
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.
Compare the solubility of silver chloride in each of the following aqueous solutions: Match to soubility levels that goes with each. 0.10 M NH4NO3 0.10 M KCH3COO 0.10 M NH4Cl 0.10 M AgNO3 More soluble than in pure water. Similar solubility as in pure water. Less soluble than in pure water.
Solid potassium hydroxide is slowly added to 175 mL of a 0.318 M nickel(II) acetate solution until the concentration of hydroxide ion is 0.0568 M. The percent of nickel ion remaining in solution is __ % Solubility Product Constants (Ksp at 25 oC) Type Formula Ksp Bromides PbBr2 6.3 × 10-6 AgBr 3.3 × 10-13 Carbonates BaCO3 8.1 × 10-9 CaCO3 3.8 × 10-9 CoCO3 8.0 × 10-13 CuCO3 2.5 × 10-10 FeCO3 3.5 × 10-11 PbCO3 1.5 × 10-13 MgCO3 4.0 × 10-5 MnCO3 1.8 × 10-11 NiCO3 6.6 × 10-9 Ag2CO3 8.1 × 10-12 ZnCO3 1.5 × 10-11 Chlorides PbCl2 1.7 × 10-5 AgCl 1.8 × 10-10 Chromates BaCrO4 2.0 × 10-10 CaCrO4 7.1 × 10-4 PbCrO4 1.8 × 10-14 Ag2CrO4 9.0 × 10-12 Cyanides Ni(CN)2 3.0 × 10-23 AgCN 1.2 × 10-16 Zn(CN)2 8.0 × 10-12 Fluorides BaF2 1.7 × 10-6 CaF2 3.9 × 10-11 PbF2 3.7 × 10-8 MgF2 6.4 × 10-9 Hydroxides AgOH 2.0 × 10-8 Al(OH)3 1.9 × 10-33 Ca(OH)2 7.9 × 10-6 Cr(OH)3 6.7 × 10-31 Co(OH)2 2.5 ×…
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.
TypeFormulaKsp Solubility Product Constants (Ksp at 25 oC) TypeFormulaKspBromidesPbBr26.3 × 10-6AgBr3.3 × 10-13CarbonatesBaCO38.1 × 10-9CaCO33.8 × 10-9CoCO38.0 × 10-13CuCO32.5 × 10-10FeCO33.5 × 10-11PbCO31.5 × 10-13MgCO34.0 × 10-5MnCO31.8 × 10-11NiCO36.6 × 10-9Ag2CO38.1 × 10-12ZnCO31.5 × 10-11ChloridesPbCl21.7 × 10-5AgCl1.8 × 10-10ChromatesBaCrO42.0 × 10-10CaCrO47.1 × 10-4PbCrO41.8 × 10-14Ag2CrO49.0 × 10-12CyanidesNi(CN)23.0 × 10-23AgCN1.2 × 10-16Zn(CN)28.0 × 10-12FluoridesBaF21.7 × 10-6CaF23.9 × 10-11PbF23.7 × 10-8MgF26.4 × 10-9HydroxidesAgOH2.0 × 10-8Al(OH)31.9 × 10-33Ca(OH)27.9 × 10-6Cr(OH)36.7 × 10-31Co(OH)22.5 × 10-16Cu(OH)21.6 × 10-19Fe(OH)27.9 × 10-15Fe(OH)36.3 × 10-38Pb(OH)22.8 × 10-16Mg(OH)21.5 × 10-11Mn(OH)24.6 × 10-14Ni(OH)22.8 × 10-16Zn(OH)24.5 × 10-17IodidesPbI28.7 × 10-9AgI1.5 × 10-16OxalatesBaC2O41.1 × 10-7CaC2O42.3 × 10-9MgC2O48.6 × 10-5PhosphatesAlPO41.3 × 10-20Ba3(PO4)21.3 × 10-29Ca3(PO4)21.0 × 10-25CrPO42.4 × 10-23Pb3(PO4)23.0 × 10-44Ag3PO41.3 × 10-20Zn3(PO4)29.1 ×…
Professor Acetico Acido has assigned the analysis of unknown organic compound samples to Al Coholbased on their solubility behavior. The summary of the solubility profile are tabulated below along with thepossible structures of the samples. Identify each unknown sample by matching the respective solubility profilewith the given structures. Briefly explain the reason for your answer.
Copper is regulated in drinking water to protect public health. The relevant reaction is below. The solubility product (equilibrium constant) for the reaction is pK = 19.3. Cu(OH)2 (s) = Cu+2 + 2 OH- The regulatory “action limit” (concentration at which a drinking water utility must take action to reduce levels) is 1.3 mg/L dissolved copper. If the water is at a pH of 7.2, is the level of dissolved copper above, at, or below the action limit? To reduce the concentration of dissolved copper, would you raise or lower the pH? Why? SHOW ALL WORK
CdF2(s)⇄Cd2+(aq)+2F−(aq) A saturated aqueous solution of is prepared. The equilibrium in the solution is represented above. In the solution, [Cd2+]eq=0.0585M and [F−]eq=0.117M. Some 0.90MNaF is added to the saturated solution. Which of the following identifies the molar solubility of CdF2 in pure water and explains the effect that the addition of NaF has on this solubility?

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