If the base (NaOH) is standardized to 0.12 M in Part A of this experiment, calculate the amount of oxalic acid dihydrate (H2C2O4•2 H2O, MW = 126.06 g/mol) required to neutralize 35 mL of this NaOH solution.
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If the base (NaOH) is standardized to 0.12 M in Part A of this experiment, calculate the amount of oxalic acid dihydrate (H2C2O4•2 H2O, MW = 126.06 g/mol) required to neutralize 35 mL of this NaOH solution.
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- This question is about acid base titration: Osama a student, performed an acid base titration involving a standard solution of Sodium hydroxide (NaOH) (RMM = 40) against unknown HCl solution and obtained the following results. Mass of Sodium hydroxide (NaOH) dissolved in 250 ml volumetric flask = 3.6 g 2.Volume of Sodium hydroxide used in the titration = 23 ml 3.The mean volume of HCl titrated with 25 ml Sodium…A sample of impure oxalic acid which weighs 0.4750 gram requires 35.6 mL of 0.20N NaOH. Calculate the percentage oxalic acid in the sample.A chemistry student weighs out 0.197 g of lactic acid (HC3H503) into a 250 mL. volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1600M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the equlvalence point. Round your answer to 3 significant dinits
- A student, performing the same experiment as you, recorded the following information. The original solution was diluted by a factor of 5.Calculate the volume of NaOH used to reach the equivalence point. Volume of diluted vinegar sample (mL) 25.00 Molarity of NaOH 0.0900 Initial buret reading (mL) 16.50 Final buret reading (mL) 38.00 Volume of NaOH1. An acid solution is prepared by dissolving 19.264 grams of pure KHC2O4.H2C2O4.2H2O in water and diluting to exactly 900 ml. Fifty milliliters (50.00 mL) of this solution are neutralized by 35.00 ml. of KOH solution. What is the normality of each solution? 2. What mass of Ca(OH)2 is present in a sample if it is titrated to its equivalence point with 44.02 mL of 0.0885 M HNO3? The balanced chemical equation is as follows: 2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H2O ; Balanced.A student trying to determine the Ksp for Calcium hydroxide used 10.15 mL of 0.050 M HCl to neutralize the initial volume of 15.00 mL Ca(OH)2 solution. If the accepted value of the Ksp for Ca(OH)2 is 6.5 x 10-6 calculate the percent error from this experiment.
- In Part A of this experiment, you will be standardizing a solution of sodium hydroxide (NaOH) against a sample of oxalic acid dihydrate (H2C2O4⋅2H2O, 126 g/mol). Calculate the number of grams of H2C2O4⋅2H2O required to completely neutralize 25.0 mL of 0.120M NaOH.Which of the following will result to an unlit light bulb when subjected to the conductivity test? a. 0.5 M NaCl b. 1.0 M citric acid c. Glacial acetic acid d. SeawaterWhich of the following will result to a dimly lit light bulb when subjected to the conductivity test? a. 1.0 M citric acid b. Glacial acetic acid c. Mixture of 10.0 mL 1.0 M Mg(OH)2 and 10.0 mL 1.0 M HNO3 d. 70% (v/v) ethanol
- Which of the following will result to a brightly lit light bulb when subjected to the conductivity test? a. Mixture of 10.0 mL 1.0 M Mg(OH)2 and 10.0 mL 1.0 M HNO3 b. 70% (v/v) ethanol c. 1.0 M citric acid d. Glacial acetic acid75 ml of 0.100M of thiosulfate, 100ml of distilled water mixed with 10ml 10% bleach, 6M OF HCl equation 2) I2 (aq) + 2 Na2S2O3 (aq) → 2 NaI (aq) + Na2S4O6 (aq) equation1) NaOCl (aq) + 2 Kl (aq) + 2 HCl (aq) → I2 (aq) + 2 KCl (aq) + NaCl (aq) + H2O (l)If 50.0 g Na2SO4 is dissolved in 750 mL of water what would be the sulfate ion concentration ? Show your work in a separate sheet. 0.939 M. 0.264 M. 0.469 M. 0.315 M