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- A sample of pure sodium oxalate weighing 0.1050 g is ignited [Na2C2O4 (s) --> Na2CO3 (s) + CO (g)] and the resulting product requires 15.00 mL of a solution of H2SO4 for complete neutralization. What is the normality of the acid? MM of Na2CO3 = 106.0 g/molMM of Na2C2O4 = 134.0 g/molMM of CO = 28.01 g/molMM of H2SO4 = 98.08 g/mol50.0mL of 0.180 M sodium hydroxide solution is added to 50mL of .200 M lactic acid solution. The reaction goes to completion. It can be written CH3CHOH2H + OH ---> CH3CHOHCO2 + H2O What is the limiting reactant? How many moles of it were used?When a Vitamin C (ascorbic acid; MM = 176.12 g mol-1) tablet is crushed, dissolved and titrated with 0.0340 M KIO3(aq) to a purple/blue endpoint (given by a starch indicator), the volume of KIO3 used is 29.80 mL. If 60 mg of ascorbic acid is the recommended dietary allowance (i.e., 100% of the RDA), then what is the % RDA for the Vitamin C in the tablet? KIO3(aq) + 5 KI + 6 H+ → 3 I2(aq) + 3 H2O I2 (aq) + ascorbic acid → 2 I- + dehydroascorbic acid
- KHP (aq)+NaOH (aq)-->NaKHP (aq)+H2O(l) Trial Vi (mL) Vf (mL) 1 36.19 48.56 2 3 A student masses out 1.096 grams of KHP, which is dissolved in 25.00 mL of DI water. This KHP solution is titrated with NaOH, as shown in the equation above. Calculate the molarity of the NaOH solution.Marble, a material used in buildings and statues, has the chemical composition CaCO₃. CaCO₃ reacts with acid (H₃O⁺), dissolving the solid through the reaction: CaCO₃(s) + 2H₃O⁺(aq) → Ca²⁺(aq) + CO₂(g) + 3 H₂O(l) In 1985, rain water in central Pennsylvania had an approximate H₃O⁺ concentration of 8.0 × 10⁻² mM. What volume of rain would be needed to dissolve a small statue made of 4.50 kg of marble?In a titration, 15.5 g of oxalic acid was dissolved in a flask and neutralized with 31.2 mL of NaOH. Determine the molarity of the NaOH. Hint: Primary standards (like oxalic acid, here) incude water in their formula. As a result, they do not absorb atmospheric water. Oxalic acid has the chemcial formula: H2C2O4⋅2H2O (so be sure to include the 2 extra water molecules). a. 8.33 M b. 3.55 M c. 7.88 mol/L d. 0.333 mol/L
- Using the average molarity of the NaOH solution determined from your results in part A, calculate the molarity and percent by mass of the acetic acid in your vinegar sample and report their average values. H2C2O4•2H2O(s) + 2NaOH (aq)= Na2C2O4 + 4H2O(l) part A Mass of oxalic acid analyzed (g)- trial 1- 0.302 trial 2- 0.305 initial buret reading of NaOH (mL)- trial 1-0.31 trial 2- 23.42 final buret reading of NaOH (mL) trial 1- 23.42 trial 2 -46.73 Part B volume of vinegar analyzed (mL), trial 1- 5.00 , trial 2- 5.00 initial buret reading of NaOH (mL), trial 1 -0.00, trial 2 - 22.73 final buret reading of NaOH (mL) trial 1- 22.73, trial 2- 45.50 There is no molarity of oxalic acid that was used during the experiment givenSodium formate, NaCHO2, can be titrated in neutral solution according to the equation:CHO2- + MnO4- + H2O → MnO2 + CO2 + OH-.If 10.00 ml. of the KMnO4 are equivalent to 0.08161 gram of sodium formate by this method, what is the value of each milliliter in terms of millimoles of H2O2?naco3(aq) + cacl(aq) ----- 2nacl(aq) + caco3(s) calculate the volume (in mL) of 0.100M cacl needed to produce 1.00g of caco3(s) there is an excess of naco3 molar mass of calcium carbonate = 100.09 g/mol volume of calcium chloride = ? mL
- (1) Careless Carlie weighed her KHP sample, but forgot to bring her report sheet along, so she recorded the mass of KHP on a paper towel. During her titration, which required 18.46 mL of base, she spilled some base on her hands. She remembered to wash her hands, but forgot about the data on the towel, and used it to dry her hands. When she went to calculate the molarity of the base, Carlie discovered that she didn’t have the mass of her KHP. Her kindhearted instructor told Carlie that her base was 0.2987 M. Calculate the mass of Carlie’s KHP sample. Show calculations (2) What mass of solid NaOH would be needed to make 645 mL of Carlie’s NaOH solution? Show calculations.Tartaric acid, H2C4H4O6, is a diprotic acid that naturally occurs in the production of wine. Jose was tasked to find out the acid content in a 100.0 mL wine sample by titrating it with a standardized solution of NaOH. He was able to establish the working concentration of the NaOH solution by using 35.21 mL of it to titrate a primary standard of KHP that weighed 3.001 g. The grams and %w/w of Tartaric acid present in the 100.0 mL wine sample were then determined by titrating a 25.00 mL aliquot using 43.56 mL of the standardized NaOH solution. H2C4H4O6 (aq) + 2NaOH (aq) ↔ Na2C4H4O6 (aq) + 2H2O (l) Assume that the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of H2C4H4O6 = 150.087 g/mol What is the molar concentration of the prepared NaOH solution?…and Employees CH STATE GE 90 ENDULERSE IS FOREVER "ON-Tame Name Jodi Rayal Molarity = wt. x1000 3. Calculate the massof Potassium hydrogen phthalate (KHP) to prepare a 250.0 mL solution of 0.1000 M KHP solution. Mol ut. x Voluse the 2500×1000 204.22250 mass Initial Buret Reading Final Buret Reading Vol NaOH Added Moles of NaOH Moles of HCI Volume of unknown HCI solution Concentration of HCI Average concentration of HCI of KHP = 5.11g 4. Complete the table below for the following neutralization reaction of an unknown concentration of hydrochloric acid with 0.100 M sodium hydroxide: Mu spate solution Trial 1 0 11.15 го data and calculate the concentration 15 Trial 2 11.15 22.15 Trial 3 22.15 33.25 abyh 067 LANDINUKASHU TROWTHCENTISSATE ARAD Ma That par މއކނި REMURNAR MISAMARALISERDRY Tile