alculate the Ksp of a Ca(OH)2 solution using the data below: Titrated with 0.103MHCl Initial syringe value: 9.71 Final Syringe value: 1.53 Volume of Ca(OH)2 titrated 24.39 mL
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alculate the Ksp of a Ca(OH)2 solution using the data below:
Titrated with 0.103MHCl
Initial syringe value: 9.71
Final Syringe value: 1.53
Volume of Ca(OH)2 titrated 24.39 mL
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- Calculate the mass of acetic acid in 100ml of both samples in vinegar. given: NaOH vs CH3COOH Burette solution is NaOH and the pipette solution is 5.0 mL of Vinegar Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate 0.0 mL 20.1 mL 20.1 mL 20.3 mL Titration 1 0.0 mL 20.9 mL 20.9 mL Titration 2 0.0 mL 20.0 mL 20.0 mL To find the average volume Average volume = 20.1 mL + 20.9 mL + 20.0 mL320.1 mL + 20.9 mL + 20.0 mL3 = 20.3 mL Concentration of Vinegar = Volume of NaOH * Concentration of NaOHVolume of vinegarVolume of NaOH * Concentration of NaOHVolume of vinegar = 20.3 mL * 0.0647 M5.0 mL20.3 mL * 0.0647 M5.0 mL = 0.2627 M Concentration of NaOH = Volume of H2SO4 * Concentration of H2SO4Volume of NaOHVolume of H2SO4 * Concentration of H2SO4Volume of NaOH = 10.0 mL…Titration of a 0.824 g of 99.99% KHP (204.23 g/mol) with phenolphthalein required 18.3 mL of NaOH (40.00 g/mol) solution to reach the end point. The same titrant was used to analyze an impure acetic acid (CH3COOH, 60.06 g/mol) solution. A 10.0 mL aliquot of the sample required 12.9 mL of the titrant. What substance served as the primary standard?Which served as the indicator in the titration?What is the color at the end point?What is the concentration of the titrant?What is the molar concentration of the acetic acid solution?Develop a titer for determining water hardness based on the following information: 6.240 mg/L Ca2+ calcium standard. It is titrated to the endpoint with 8.59, 8.34, and 8.47 mL of EDTA solution.
- A titrant solution of KMNO4 was standardized with 0.2g of Na2C2O4 amd consumed 27.75 mL to reach endpoint. What is the standardized normal concentration of the titrant?A 25.00 mL water sample required 14.00 mL of 0.021M EDTA to reach its endpoint. A blank titration required 2.13 mL. Calculate the hardness of the water sample in ppm CaCO3. Show the math setup.5g unknown sodium carbonate titrated with HCl. Two endpoints observed. TITRATION: 20mL of the diluted solution (5g sodium carbonate + 250 water) + 10mL of water were used for the titration (TOTAL VOLUME 30 mL) CO32- + H+ -> HCO3- HCO3- + H+ -> H2O + CO2 First endpoint 45.00mL HCl Second end point 65.00mL HCl FIND: alkalinity of CO32- & HCO3- wt% of CO32- & HCO3- PLEASE SHOW ALL WORK
- Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution.MnO4- + 5H2C2O4 + 6H+ → 2Mn2+ + 10CO2(g) + 8H2OCalculate the molar concentration of the KMnO4 solution.In how much volume of diluted sulfuric acid should you dissolve a multivitamin tablet of approximately 1700 mg of Vitamin C to back analyze 10.00 mL of that solution, with 25.00 mL of 0.01 M KIO3 and 0.04 M thiosulfate to use approximately 8-10 mL of titrant ? You have 25, 50, 150, 250 and 500 mL flasks.A dilute peroxide solution was prepared by quantitatively diluting 10 mL stock H2O2 (MW = 34.0147) to 250mL using a volumetric flask. 50 mL aliquot of the diluted peroxide solution was titrated using the previously standardized KMnO4 in problem 1. Titration of the sample required 29.00 mL titrant and the blank containing 50 mL 1:5 H2SO4 required 0.75 mL of the standard KMnO4. Calculate the concentration in %w/v of the stock H2O2. (Hint: H2O2 produces O2 under acidic condition). Follow sig. Fig
- Need solution to all parts if not answered I'll downvote solution Find the pH during the titration of 20.00 mL of 0.1910 M benzoic acid, C6H5COOH (Ka = 6.3 10-5), with 0.1910 M NaOH solution after the following additions of titrant. (a) 0 mL (b) 10.00 mL (c) 15.00 mL (d) 20.00 mL (e) 25.00 mLA sample is analyzed for chloride by the Volhard method. From the following data, calculate the percentage of chloride present:Weight of sample = 6.0000 g dissolved and diluted to 200 mLAliquot used = 25.00 mL AgNO3 added = 40.00ml of 0.1234MKSCN for back titration = 13.20ml of 0.0930MTitration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution. 2MnO4- + 5C2O4-2 +16H+ -> 2Mn2+ + 10CO2(g) + 8H2O Calculate the molar concentration of the KMnO4 solution What molecules would interfere with the titrimetric analysis?