For eac.ne 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.spDoes solubilitychange withpH?highest solubilitycompoundpH = 5pH = 7pH = 8%3DyesCal,O noO yesBa (OH)2O noO yesKClO no

Answered: For eac. ne following compounds, decide…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.28QAP

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A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
(a) I f t he molar solubilit y o f CaF2 at 35 °C i s1.24 x 10-3 mol/L, what is Ksp at this temperature? (b) It isfound that 1.1 x 10-2 g SrF2 dissolves per 100 mL of aqueoussolution at 25 °C. Calculate the solubility product forSrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 x 10-10. What isthe molar solubility of Ba(IO3)2?
Suppose 100 mL of 2.0 × 10–4 M Fe(NO3)3is added to 100 mL of 2.0 ×10–5 M KIO3. What is Qsp value? Will it precipitate?
The solubility of strontium carbonate (SrCO3) is 0.0011 g/100 mL at 20ºC. Calculate the Kspvalue for this compound.
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
The arsenic in a 1.22-g sample of a pesticide was converted toAsO43- by suitable chemical treatment. It was then titratedusing Ag+ to form Ag3AsO4 as a precipitate. (a) What is theoxidation state of As in AsO43-? (b) Name Ag3AsO4 by analogyto the corresponding compound containing phosphorusin place of arsenic. (c) If it took 25.0 mL of 0.102 M Ag+to reach the equivalence point in this titration, what is themass percentage of arsenic in the pesticide?
(a) If the molar solubility of Cd3(AsO4)2 at 25 oC is 1.15e-07 mol/L, what is the Ksp at this temperature?Ksp = __________(b) It is found that 8.90e-06 g of Y2(CO3)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Y2(CO3)3.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3? solubility = ________mol/L
In order to prepare for a qualitative analysis experiment, Felix is predicting whether small samples of several pairs of 0.10 M control solutions will form a precipitate when mixed. He uses the table of solubility values provided as well as the general solubility guidelines in the chempendix. Solubilities of Alkaline Earth Salts (g/100 g H2O, at 20−25∘C) OH− CO2−3 SO2−4 CrO2−4 C2O2−4 Mg2+ 0.00069 0.18 35.7 54.8 0.038Ca2+ 0.16 0.00066 0.205 13.2 0.00061Sr2+ 2.25 0.00034 0.135 0.106 0.005Ba2+ 4.91 0.0014 0.00031 0.00026 0.0075For each pair of compounds, predict the formula for the precipitate that Felix will see when he mixes the solutions in lab. If no precipitate forms, enter NP for no precipitate.
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
A solution of 0.079 M CoBr2 is saturated with H2S. ([H2S] = 0.087 M. Assume saturation is maintained by bubbling H2S through the solution for the duration of the experiment.) CoS(s) Co2+(aq) + S2−(aq) Ksp = 4.0 ✕ 10−21 H2S(aq) + 2 H2O(l) 2 H3O+(aq) + S2−(aq) K = 8.9 ✕ 10−27 What is the minimum pH at which CoS begins to precipitate?
The solubility product for an insoluble salt with the formula M2X3 is written as __________, where s is the molar solubility. A. Ksp= 108s5 B. Ksp= 6s5 C. Ksp= 18s5 D. Ksp= s5 E. Ksp= 56s5
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 ×…

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