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- Tab Window Help age Learning X ATM HOMEWORK Module 9 X Submit Answer Mind Tap - Cengage Learning X loymentid=5735112480241329813180832311&eISBN=9781305862883&id=1707786068&snapshotid=33225... References Use the References to access important values if needed for this question. dation-Reduction Titrations: This is group attempt 1 of 10 tv Suppose a solution of the reducing agent Cut is titrated with a solution of the oxidizing agent permanganate. The balanced net ionic equation for the reaction is: MnO4 (aq) + 5Cu*(aq) +8H30*(aq) →Mn²+ (aq) + 5Cu²+ (aq)+12H₂O(l) What volume (in mL) of a 0.1258 M MnO4 solution would be required to consume the Cu* in a 20.00 mL sample of a solution containing 0.5548 M Cu*? mL Numeric input field Autosaved at 10:58 PM a 8 C G What volume (in mL) of a 0.125 A WPart 2 - Colorimetric Representation of Le Chatlier's Principle Mass needed to make 15.0 mL of 0.200 M CoCl₂ 6 H₂O (MW=237.93) • Starting solution (15.0 mL 0.200 M CoCl₂ 6 H₂O + 9.00 mL 12.0 M HC1) Try 1: ✔ 0.713 2 2 Info ID500 Try 1: ✔ Purple Correct Answer: ✔ Purple 0.750.75Profiles Tab Window Help p Cengage Learning XAM HOMEWORK Module 9 Back APR 17 html?deploymentid=5735112480241329813180832311&elSBN=9781305862883&id=1707786068&snapshotld-33225... X Submit Answer 18. Oxidation-Reduction Titrations: This is group attempt 1 of 10 MindTap - Cengage Learning X Use the References to access important values if needed for this question. The concentration of H₂C₂O4 in a solution is determined by titrating it with a 0.1796 M permanganate solution. The balanced net ionic equation for the reaction is: tv References 2MnO4 (aq) + 5H₂C₂O4(aq) + 6H30*(aq) → 2Mn²+ (aq) + 10CO₂(g) + 14H₂O(1) - In one experiment, 23.66 mL of the 0.1796 M permanganate solution is required to react completely with 30.00 mL of the H₂C2₂04 solution. Calculate the concentration of the H₂C₂O4 solution. N Autosaved at 10:58 PM I What volume of a 0.352 M hyd X ☎ Q 8 C M A W P U Mon Apr 17 * + Next ☐ X
- [References] A solution of a weak acid was tested with the indicators used in this experiment. The colors observed were as follows: Methyl violet: violet Thymol blue: yellow Methyl yellow: orange Congo red: violet Bromocresol green: yellow What is the approximate pH of the solution? Submit Answer Try Another Version 10 item attempts remainingCalculate pH of a salt solution. What is the pH of a 6.65x102 M aqueous solution of sodium hypochlorite, NACIO? (K, for HCIO = 3.5×10*) pH = Check & Submit Answer Show ApproachQuestion 27 please help
- Review the list of common titration errors. Determine whether each error would cause the calculation for moles of analyte to be too high, too low, or have no effect. ANSWER BANK: Too low, No effect OR Too high adding titrant past the color change of the analyte solutionrecording the molarity of titrant as 0.1 M rather than its actual value of 0.01 Mspilling some analyte out of the flask during the titrationstarting the titration with air bubbles in the buretfilling the buret above the 0.0 mL volume markonly SELECT correct respomses 1) Titrations of different forms are often employed to quantitate acids, bases, metal ions, and proteins. 2) To perform a titration, the experimenter must be familiar with the stoichiometry of the reaction taking place between the reagent and analyte. 3) Often in titrations, a visible color change will occur in the solution (due to an added indicator solution). 4) Gravimetric titrations directly measure the volume of reagent solution needed to react completely with an analyte. 5) For a monoprotic weak acid titration, the weak acid solution being titrated is the "sample" that is being quantitated. 6) For a monoprotic weak acid titration, the equivalence point is reached when the moles of added base equals the moles of weak acid originally present in the reaction vessel. 7) In a monoprotic weak acid titration, the weak acid is the analyte in solution, and a standardized base (for example, a solution of known concentration of NaOH) is the titrant. 8) A…Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29 1.41 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 50.37 49.39 49.84 Table 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29 1.41 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 50.37 49.39 49.84 Expected color at end point Volume of NaOH used (mL) 48.08 47.98 47.89 Compute for the ff: a. Average moles of acetic acid (mol)? b. Average molarity of acetic acid (M)? c. Average molarity of acetic acid (M)?
- Discussion 1.What the difference between primary and secondary standard substances? 2.Calculate the volume of conc. HCl(11M) required for preparing 250 ml 0.1 M? المرحلة الأولی 3. Calculate the weight of NazCO3 required for preparing 100 ml 0.1 M? قسم الهندسة الكيمياوية 4. Why is sodium carbonate primary solution? 5. Why standard solution should be colorless? 6. Why is HCl not primary solution?Water ionizes by the equation H2O(1) = H(ag) + OH (ag) The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between H+] and [OH]: Kw = [H+][OH) Keep in mind that, like all equilibrium constants, the value of Kw changes with temperature.A 2.00 graduated cylinder contains 1.40 of buffer solution. The density of the buffer solution is 1.02 g/mL. What is the mass in grams of the buffer in the cylinder? STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 0.001 2040 1000 1.40 1 2.00 1430 1.02 2.04 1.43 mL g/mL