The following results of alkalinity determination for 100 ml sample titrated with 0.02N H,SO. (Answer 8-9) Sample pH- 11 Phenolphthalein end point 10ml Methyl orange end point= 15.5ml 8 Caustig alkalinity in mg/l asCaCO. 17.0 0.001 50 200 9) Total alkalinity in mg/l asCaCO, 230 105 300 155
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- Molarity of titrant (NaOH): 0.4550 M HC2H3O2 (aq) + NaOH (aq) → NaC2H3O2 (aq) + H2O (l) Trial # First Second Third Fourth Initial buret reading 0.15 mL 2.43 mL 1.32 mL 0.58 mL Final buret reading 18.62 mL 20.87 mL 20.03 mL 19.14 mL Volume of titrant used 18.47 mL 18.44 mL 18.71 mL 18.56 mL 4) Calculate the molarity of the acetic acid in the vinegar solution (Show your work). use FW for moles-->grams acetic acid. Molarity acetic acid = _____________ M 5) Calculate the weight % of acetic acid in the vinegar. How does this compare with the % listed on the label (5.00%)? (For this calculation assume that density of vinegar is 1.03 g/mL and of course, show your work). Weight % = ___________ 6) If you didn’t get the same weight % of acetic acid as listed on the vinegar label (5.00 %), what are two things (be specific) that could’ve happened during the experiment that could explain the variation from the expected weight %? To do…Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3A RbOH solution is titrated four (4) times against potassium hydrogen phthalate (KHP; FW=204.224) samples to the Phenolphthalein endpoint. Using the data below, determine the concentration of the RbOH solution? g of KHP Volume of Base Required 0.5373 g 42.49 mL 0.5856 g 43.88 mL 0.5790 g 48.56 mL 0.5856 g 44.60 mL (Report your answer as "mean +/- std dev") M What is the percent relative standard deviation? % What is the 99% Confidence Interval for the concentration of the solution (population mean)?
- Part A: Standardization of a Sodium Hydroxide Solution Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH Molarity of NaOH Average Molarity of NaOH: _______________1 ) The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is 2) Calculate the pAg^ + at the equivalence point in the titration of 25.0ml of 0.0823 M Kl with 0.051M AgNO 3 . Ksp Agl=8.3*10^ -16 3) Commercial concentrated aqueous nitric acid is 70.4% HNO3(63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is 4) Consider the titration of 25ml of 0.0823M KI with 0.051M AGNO3, Kspagi =8.3x10-16 Calculate pAg* after adding 39.0 ml I03 Ag* + 103 ====AglO3 5) Commercial concentrated aqueous nitric acid is 70.4 1\%HNO 3 (63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is: 6) What mass in g of Na 2 CO 3 [106 g/mol] is required to prepare 250 ml of 0.3M aqueous solution in Na^ + [23.g/mol] ? 7) Calculate pAg^ + after adding 42.30ml AgNO 3 In the titration of of 0.0823M Kl with 0.051M AgNO 3 . KspAgl = 8.3 * 10 ^ - 16 8) The milliliters of concentrated HClO 4 (100.5 g/mol),6 60% by mass,…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.
- A 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 0.0930MQ: The solubility product of Zn(OH)2 at 25oC is 3.0 x 10-6 M3. Calculate the solubility of Zn(OH)2 in water in gdm-3. [Ar: Zn = 65.5; O = 16; H = 1] The Mr for Zn(OH)2 is 99.5. When I multiply it with Ksp, I didn't get the same answer as the given answer which is 0.904 gdm-3.Find out the molarity of an old KOH solutionYou measure 1.456 g of KHP (MW=204.22 g/mole) dissolve it in 50.0 of H20 add an indicator and begin to titrate with the old KOH KHP (aq) +KOH (aq) =K2P (aq) +H2O (l) the initial and volume burette readings are 1.35 mL & 24.3 mL then what is the concentration of KOH ?
- A 25.0mL mixture solution contains NaNO3 and KIO4, titrated against 0.02M Na2S2O3. The volume of titrants is 18.2 mL, the concentration of KIO4 is:a) 3.64 × 10-4 b) 9.1 × 10-5c) 1.82 × 10-3 d) 2.35e) 3.64 × 10-4a primary standard of (COOK)2.H2O was prepared up to 0.05M. This primary standard was then titred against an unknown concentration of 50cm3 of KMnO4. An average titre value of 13 was obtained. The balanced equation is as follows: 5(COOK)2.H2O + 2KMnO4 + 8H2SO4 = 6K2SO4 +2MnSO4 + 10CO2 +18H2O. Find the concentration of the KMnO4.Use acid-base titration to determine theconcentration of:– A strong acid: HCl 0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOH Phenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10