### Influence of Precipitate Loss on Limiting Reactant Percentage**Question 4:**Because of the small particle size of the CaC₂O₄·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?### Detailed Explanation:When conducting a chemical experiment where the precipitation and filtration processes are used to determine the amount of a product (in this case, Calcium Oxalate Monohydrate - CaC₂O₄·H₂O), the particle size of the precipitate can significantly impact the accuracy of the results. If the precipitate particles are too small, they may pass through the filter, leading to an incomplete collection of the solid product.This incomplete collection means that the actual mass of the precipitate recovered will be less than the theoretical amount that should be formed based on stoichiometric calculations. The reported percentage of the limiting reactant, which is calculated using the mass of the collected precipitate, will consequently be lower than the actual percentage. This is because the lower mass of the recovered precipitate will suggest that a smaller amount of the limiting reactant was used in the reaction than actually was. In other words, the perceived efficiency of the limiting reactant will be underestimated, which can lead to incorrect conclusions about the reactant quantities and the reaction yield.**Key Points:**- Small particle size of CaC₂O₄·H₂O precipitate may cause it to pass through the filter.- Loss of precipitate results in a lower reported mass of the collected product.- The reported percentage of the limiting reactant will be inaccurately low.- This underestimation impacts the perceived efficiency and yield of the reaction.This methodological nuance highlights the importance of considering particle size and filtration efficiency in experimental design to ensure accurate measurement and analysis.

Answer is explained below. In the question it is given that, because of the small particle size of…

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?

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?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

5. Calculate the solubility (g/L) for silver sulfate, Ag2SO4 in 0.250 M AgBr. Ksp = 1.5 x 10s %3D
10. For the following solid Ca3(PO4)2|| a. From the balanced equation for the dissolution reaction b. From the expression of the solubility product (Ksp)
128 Identity of Oxalate Salt Solubility: •) macias CF C204" Solubility Product Constant 240 Sr C₂04-H₂0 0.00433g Sr C₂O4 - H₂0 toog H₂O Kp from Solubility (Show your calculations below) Calculate the molarity of KMnO4 solution needed to titrate 50.00 mL of a saturated solution of this oxalate salt. It should take 7.50 mL of KMnO4 solution to titrate the saturated oxalate solution. m - 000904 ROG GA oval
Calculate the solubility at 25 °C of PbCO3 in pure water and in a 0.0070M Pb(NO3)2 solution. You'll find K sp Round both of your answers to 2 significant digits. solubility in pure water: x10 solubility in 0.0070 M Pb(NO3)2 solution: 20 170 L Ox 00 믐 ? data in the ALEKS Data tab.
1. Calculate the Ksp for MgF, if it has a solubility of 5.3 x 103.
One mixes aqueous NaCl with aqueous AgNO3. NaCl. AgNO3and NaNO3all have appreciable solubility in water. AgCl has a solubility product constant Ksp of 1.6 x 10-10. If one mixes the NaCl solution with the AgNO3solution, one would suspect: a) no precipitate will form b) AgCl precipitate will form c) NaNO3 precipitate will form d) both AgCl and NaNO3 precipitates will form
4. In a gravimetric determination of sulfur as BaSO4, 0.8863 g of the ignited precipitate is found to contain 7.71 mg of coprecipitated Na,SO4. Calculate the percentage error of the determination resulting from the presence of the Na,SO4-
To determine the solubility product constant of Al(OH)3 at a specific temperature, a saturated solution of Al(OH)3 at the required temperature was titrated with 0.2M HCl via the reaction: 3HCl + Al(OH)3 → AlCl3 + 3H2O. Based on the following data, determine the Ksp of Al(OH)3 at the specified temperature: Volume of Al(OH)3 titrated: Volume of 0.2M HCl required: 9.5 mL 3.44 mL Your answer should follow the format: a) mols of HCl added b) mols of Al(OH)3 c) Molarity of Al(OH)3 d) Ksp of Al(OH)3
4.0 mL of 0.20 M HCI is added to 4.0 mL of 0.30 M Pb(NO3)2 to produce a precipitate of PbCl21s)- Water in the amount of 9.0 mL is added to dissolve the precipitate. Based on this data, what is the Ksp of PBCI2(s}? Express answer as a decimal value.
Determine the molar solubility for Cd₂(PO) by constructing an ICE table, writing the solubility constant expression, and solving for molar solubility. The value of Ksp for Cd₂(PO) is 2.5 × 10:³³. Complete Parts 1-3 before submitting your answer. Initial (M) Change (M) Equilibrium (M) +x 1.000 + 3x Assume the solution already contains 0.500 M NPO. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. 0 1 +2x 1.500 + x Cd (PO),(s) 0.500 +3x 1.500 + 2x -0.500 0.500 + x 2 1.500 + 3x 1.000 0.500 + 2x 3 Cd²+ (aq) -1.000 3 0.500 + 3x + 1.500 1.000 + x 2 PO³(aq) RESET NEXT -1.500 1.000 + 2x
If a student combines specific amount CaCl2. 9H2O and Na2CO3 and obtained a solid precipitate. The student dissolve 1.37 gram of CaCl2. 9H2O in 25.0 mL of water and 0.984 g of Na2CO3 in 25.0 mL of water. The student is then combining the two solutions and observed the formation of a solid precipitate. The student filter the solution and recovered the precipitate. The following data were obtained for the experiment. Initial Mass of CaCl2. 9H2O 1.37 g Initial Mass of Na2CO3 0.984 g % yield of this experiment 87.4% 1. What is the balanced equation for this experiment?
Construct the expression for Ksp for solid Ba³(PO4)2 in aqueous solution. Ba3(PO4)2(S) = 3 Ba²+(aq) + 2 PO4³-(aq) 1 Based on your knowledge of how the solid will dissociate in aqueous solution, construct the expression for the solubility constant, Ksp. Each reaction participant must be represented by one tile.. [Bas(PO4)2] [Ba²+] [PO4³-1² 2[Bas(PO4)2] 3[Ba²+] 3[PO4³] Ksp 3[Bas(PO4)2] [Ba²+]³ [PO4³-1³ = [Bas(PO4)2]² [PO4²-] [Bas(PO4)2]³ 2[PO4²-] [Bat] [PO4²-]² 3[Bat] [PO4³-] RESET [Ba+]³ 2[PO4³]