Having trouble working through these questions 14.(17 Points)Iron (III) hydroxide, Fe(OH)3 (Ksp = 2.6x10-39 M³) is an insoluble compound.a) (4 Points) Write the equation for the solubility equilibrium of Fe(OH)3.Fe(OH), () = Fe+ (aq) +30 (aq)S35b) (3 Points) Write out the Ksp expression for the solubility equilibrium of Fe(OH)3.ksp = [5] [35]KSP [275]"c) (5 Points) Calculate the solubility of Fe(OH)32.6x16 (275342.3410M = 2758.4 x 10 = S-12d) (5 Points) Calculate the molar solubility of Fe(OH)3 in a solution of 0.0125 M NaOH.2.611039Fe(OH)2|PageIL

considering the solubility of Fe(OH)3 and the effect of NaOH on its solubility:a) Solubility…

Answered: 14. (17 Points) Iron (III) hydroxide,…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter7: Statistical Data Treatment And Evaluation

Section: Chapter Questions

Problem 7.26QAP

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Which of the following compounds will be the MOST soluble in pure water at 25 ˚C? A. Lead (II) carbonate, PbCO3 Ksp = 7.4×10–14 B. Cobalt (II) carbonate, CoCO3 Ksp = 1.4×10–13 C. Manganese (II) carbonate, MnCO3 Ksp = 1.8×10–11 D. Cadmium carbonate, CdCO3 Ksp = 5.2×10–12 E. Barium carbonate, BaCO3 Ksp = 5.1×10–9
Lactic acid (CH3 - CH(OH) - COOH) is a weak acid and therefore a weak electrolyte.found in "cut milk". The freezing point of an aqueous solution 0.01 m of lactic acid is 0.0206 ºC. Knowing that in aqueous solution the following equilibrium occurs:CH3 -CH(OH) -COOH(ac) = CH3 -CH(OH) -COO(-)(ac) + H(+)(ac)and that, therefore, there are three species (solutes) in solution, calculate their percentage of ionization.
Lactic acid (CH3 - CH(OH) - COOH) is a weak acid and therefore a weak electrolyte. found in "cut milk". The freezing point of an aqueous solution 0.01 m of lactic acid is 0.0206 ºC. Knowing that in aqueous solution the following equilibrium occurs: CH3 -CH(OH) -COOH(ac) = CH3 -CH(OH) -COO(-)(ac) + H(+)(ac) and that, therefore, there are three species (solutes) in solution, calculate their percentage of ionization.
The Ksp of Barium Carbonate, BaCO3, is 2.58x10^-9. Calculate the solubility of this compound in g/L.
The following data table indicates the solubility of a substance. By examining the data presented, predict the solubility of the substance at 50 oC. Temperature (oC) Solubility (mM) 5 5.00 15 4.35 25 3.70 35 3.05 45 2.40
The following data table indicates the solubility of a substance. By examining the data presented, predict the solubility of the substance at 50 oC. Temperature (oC) Solubility (mM) 5 5.00 15 4.35 25 3.70 35 3.05 45 2.40 2.00 mM 1.40 mM 1.00 mM 2.10 mM 1.75 mM
Table 1: Temp vs. solubility data of ammonium chloride. Test tube g NH4Cl/10 mL H2O Crystallization temp. (ºC) 1 1.0 g/10 mL H2O 10 oC 2 1.8 g/10 mL H2O 20 oC 3 2.9 g/10 mL H2O 40 oC 4 3.8 g/10 mL H2O 65 oC 5 4.4 g/10 mL H2O 95 oC Use the table to plot a solubility curve for ammonium chloride on the graph provided below. For the best fit line, use a smooth curve. "Mass of Solute per 100 mL of H2O," should be written on the y-axis (use increments of 2g for every box). "Temperature (°C)" should be written on the x-axis (use increments of 10 °C for every 2 boxes).
Like all equilibrium constants, the value of KwKw depends on temperature. At body temperature (37 ∘C∘C), Kw=2.4×10−14Kw=2.4×10−14. What is [H3O+][H3O+] in pure water at body temperature?
Is Ksp for Mg3(PO4)2 is 5.2 x 10^-24 at 25 degree Celsius. What is the molar solubility of Mg3(PO4)2 in 0.25 NaPO4? -> 2.1 x 10^-10M -> 1.5 x 10^-8 M -> 1.5x10^-3M -> 4.1x 10^-1M -> 2.0 M
2.3 - At temperature of 18°C was 4,7 g of silver molybdate (M = 376 g mol–1) mixed with 500 cm3 of a) distilled water b) solution of AgNO3 with concentration of 0,02 mol dm–3 c) solution of Na2MoO4 with concentration of 0,02 mol dm–3 Determine, how many percent of Ag2MoO4 will dissolve in each case. Solubility equilibrium of Ag2MoO4 is 3,1.10-11.
For Cu (OH)2, Ksp = 2.6x10-19. What is the molar solubility of Cu (OH)2?
Estimate the aqueous gram-solubility in g/L of mercury(I) chloride: Hg2Cl2(s) ↔ 2Hg+ (aq) + 2Cl– (aq), Ksp = 1.43×10–18 The molar mass of Hg2Cl2 is 472.06 g/mol.

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