5.4.Consider the following precipitation reaction:Part A2Na3PO4 (aq) + 3CUC12 (aq) → Cu3(PO4)2 (s) + 6NAC1(aq)What volume of 0.173 M Na3PO4 solution is necessary to completely react with 89.5 mL of 0.103 M CuCl2 ?Express your answer in milliliters.• View Available Hint(s)ΑΣφ?V = 0.035mLSubmitPrevious Answers

Given Concentration of Na3PO4 = 0.173 M Concentration of CuCl2 = 0.103 M Volume of CuCl2 = 89.5 ml =…

Consider the following precipitation reaction: Part A 2NazPO4 (aq) + 3CuCl2(aq) → Cu3(PO4)2(s) + 6NaCl(aq) What volume of 0.173 M NazPO4 solution is necessary to completely react with 89.5 mL of 0.103 M CuCl2? Express your answer in milliliters. • View Available Hint(s) Π ΑΣφ ? V = 0.035 mL Submit Previous Answers

Consider the following precipitation reaction: Part A 2NazPO4 (aq) + 3CuCl2(aq) → Cu3(PO4)2(s) + 6NaCl(aq) What volume of 0.173 M NazPO4 solution is necessary to completely react with 89.5 mL of 0.103 M CuCl2? Express your answer in milliliters. • View Available Hint(s) Π ΑΣφ ? V = 0.035 mL Submit Previous Answers

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter1: Basic Concepts Of Chemistry

Section: Chapter Questions

Problem 49RGQ: Fluoridation of city water supplies has been practiced in the United States for several decades. It...

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Use the appropriate tables to calculate H for (a) the reaction between MgC03(s) and a strong acid to give Mg2+(aq), CO2(g), and water. (b) the precipitation of iron(III) hydroxide from the reaction between iron(III) and hydroxide ions.
A solution was prepared by dissolving 435 mg of K3Fe(CN)6 in enough water to give 945 mL of solution. (a) Calculate the molar concentration of K+(aq) and Fe(CN)63-(aq). (b) The normality of K+(aq) and Fe(CN)63-(aq). c) Calculate the weight/volume percentage of K3Fe(CN)6. d) The concentration of K+(aq) and Fe(CN)63-(aq) in ppm.
(3) 11. In a titration it is found that 97.7 mL of 0.154 M NaOH(aq) is needed to neutralize 25.0 mL of a solution of HCl(aq). Calculate the concentration of the HCl solution. Show your work. [Hint: Write a balanced equation for the reaction first.]
Although other solvents are available, dichloromethane(CH₂Cl₂) is still often used to “decaffeinate” drinks because thesolubility of caffeine in CH₂Cl₂ is 8.35 times that in water.(a) A 100.0-mL sample of cola containing 10.0 mg of caffeine is extracted with 60.0 mL of CH₂Cl₂. What mass of caffeine re-mains in the aqueous phase? (b) A second identical cola sampleis extracted with two successive 30.0-mL portions of CH₂Cl₂.What mass of caffeine remains in the aqueous phase after each extraction? (c) Which approach extracts more caffeine?
If 20.0 g of NaOH is added to 0.750 L of 1.00 M Cd(NO:)2, how many grams of Cd(OH)2 will be formed in the following precipitation reaction? 2 NaOH(aq) + Cd(NO:)>(aq) → Cd(OH)2 (s) + 2 NaNO:(aq) | g 1 2 3 4 5 6. 7 8 9. +/- х 100
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5.) Calculate the volume, in liters, of NaOH required to titrate the KHP in flask #2. (A7) – (A6) Volume of NaOH = 1000 mL/L 16.36 O.80 (A14) 1000 mL/L ||
6. (I) HCOj(aq)+ H2O(0) = co(ag)+H3O*(g) (II) HCO3(aq) + H₂O(1) H₂CO3(aq) +OH(aq) In which of the following reactions, H₂O acts as an acid? (III) HPO (aq) + H₂O(l) H₂PO4 (aq) + OH¯(aq) PO (aq)+ H3O*(aq) (IV) HPO (aq) + H₂O(l) (A) I and II (B) None (C) II and III (D) I and IV (E) III and IV
The following reactions (note that the arrows are pointingonly one direction) can be used to prepare an activity seriesfor the halogens:Br2(aq) + 2 NaI(aq)----->2 NaBr(aq) + I2(aq)Cl2(aq) + 2 NaBr(aq)----->2 NaCl(aq) + Br2(aq)(a) Which elemental halogen would you predict is the moststable, upon mixing with other halides? (b) Predict whethera reaction will occur when elemental chlorine and potassiumiodide are mixed. (c) Predict whether a reaction will occurwhen elemental bromine and lithium chloride are mixed.
5) The solubility of BaCO3 is 24 mg/L at room temperature. a. What is the molar solubility and the Ksp of barium carbonate? b. The carbonate ion can react with water as follows: CO3² (aq) + H₂O (1) HCO3 (aq) + OH- (aq) Kb = 2.1 x 10-4 Write the reaction out from part a, add the two reactions together, and calculate the new K of the combined reaction. C. Using your K from part b, find the solubility of BaCO3 when the reaction in part b is also considered. Did the solubility increase or decrease from part a? Explain using Le Chatelier's Principle.
1. Calcium in a sample solution is determined by atomic absorption spectroscopy (AAS). A stock solution of calcium is prepared by dissolving 1.834 g CaCl, 2H,0 in water and diluting to 1 litre. From this stock solution, the second stock solution is prepared by the dilution factor of 10. Three standard solutions of calcium are prepared from the second stock solution with the following dilution factor: 20 (first standard solution), 10 (second standard solution) and 5 (third standard solution). A blank solution is prepared as well. Absorbance signals of AAS are as follows: 1.5 (blank solution), 10.6 (first standard solution), 20.1 (second standard solution), 38.5 (third standard solution), 29.6 (sample solution). (Molar mass; Ca = 40.00 g mol-, CI = 35.45 g mol-, 0 = 16.00 g mol-', H = 1.00 g mol-1) a. Construct ONE (1) plot that could be used to represent the calibration curve. b. From the plot of Q1a, determine the amount of calcium in parts per million.
Sodium carbonate is a reagent that may be used to standardize acids in the same way that you have used KHP in this experiment. In such a standardization it was found that a 0.498-g sample of sodium carbonate required 24.8 mLmL mL of a sulfuric acid solution to reach the end point for the reaction. Na2CO3(aq)+H2SO4(aq)→H2O(l)+CO2(g)+Na2SO4(aq)Na2CO3(aq)+H2SO4(aq)→H2O(l)+CO2(g)+Na2SO4(aq) What is the molarity of the H2SO4H2SO4?