4. Because of the small particle size of the CaC204•H2O precipitate, some of it passes through the filter and is not collected. How does this loss of precipitate affect the reported percentage of the limiting reactant in the salt mixture?
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- 1.1The Ksp of Ca3 (PO4 ) 2 is 1.3 × 10−26 . Estimate the solubility of this salt in units of g. L −1 . You must show any reaction equation(s) that you may think are necessary. 1.2 If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 1.1? Explain you answer in a short sentence.The compound lead(II) sulfate has a solubility of 4.824E-3 g/100mL at 25 degC.What is the molar solubility of this solution at saturation? 0.0002 mol/L What is the Ksp at 25 degC for lead(II) sulfate? What is the molar solubility of lead(II) sulfate in 0.28 M lead(II) nitrate ?Using an experimentally determined value (2.5×10−10) of Ksp, determine the value for the reaction quotient 'Q' if Ag2CrO4 will precipitate when 7.00 mL of 0.0040 M AgNO3 are added to 5.00 mL of 0.0024 M K2CrO4.
- A 0.8000-g sample of iron ore containing 21.00% Fe is analyzed gravimetrically. If the final precipitate (assumed to be Fe,03) contains 20.0 mg of Al,O3 by mistake, what percentage of Fe does the analyst find?Magnesium fluoride (MgF2, MW = 62.30 g/mol) is slightly soluble in water, with Ksp = 7.4 x 10^-11 at T= 25. C.a) Give the correctly balanced solubility reaction and expression for Ksp for MgF2.b) What mass of magnesium fluoride will dissolve in 1.000 L of pure water?1. The Ksp of Ca3(PO4)2 is 1.3 × 10−26. Estimate the solubility of this salt in units of g. L−12. If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence.
- What wt of magnetite should be taken for analysis in order that after converting to a precipitate of Fe2O3.xH2O, the percentage of Fe3O4 in the sample can be found by multiplying the wt in grams of the ignited precipitate (Fe2O3) by 100.a solution containing 6.25×10–3 M of S2– and 5.63×10–3 M of Cd2+ was prepared. CdS ⇌ Cd2+ + S2- Calculate the Qsp of the mixture (in 3 sig. figures) and In the given scenario, will a precipitate (Ksp = 3×10–28) form?1. When 22.0 mL of a 3.08 x 10-4 M potassium sulfide solution is combined with 25.0 mL of a 5.78 × 10-4 M zinc bromide solution does a precipitate form? (Ksp (ZnS) = 2.0 × 10-25) 2. For these conditions, what is the Reaction Quotient equal to?
- The solubility of Fe(OH)2 is measured and found to be 1.15×10-3 g/L. Use this information to calculate a Ksp value for iron(II) hydroxide.What is the maximum solid solubility of Mg in Al? At what temperature does it occur? e. An Al-Mg alloy (10 wt% Mg, 90 wt% Al) is heated slowly (to insure equilibrium) from a temperature of 200 C: i. At what temperature does the first liquid phase form? ii. What is the composition of the liquid phase at the temperature in part i.? iii. At what temperature does complete melting (no solid phase remaining) occur? iv. What is the composition of the last solid remaining prior to complete melting? f. Using the equilibrium phase diagram of Figure 1, identify the phases present, their compositions, and their relative mass fractions at equilibrium for a 70 wt% Mg – 30 wt% Al alloy held at 300 C.Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. Because solubility "rules" are generalizations, we don't use solubility rules when we have the specific Ksp data available. Instead, here, we can just use the Ksp value for CuCl which is 1.9 × 10–7, for AgCl is 1.6 × 10–10, and for AuCl is 2.0 × 10–13. Based on these specific Ksp values, which compound will precipitate first? All will precipitate at the same time. It cannot be determined. CuCl(s) AgCl(s) AuCl(s)