10.0 mL of a sulfuric acid (H2SO4) solution requires 24.39 mL of 0.1071 M NaOH to reach the end point of a titration. Write a molecular equation for this reaction.
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10.0 mL of a sulfuric acid (H2SO4) solution requires 24.39 mL of 0.1071 M NaOH to reach the end point of a titration. Write a molecular equation for this reaction.
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- A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.Does the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015-M oxalic acid? (b) Add solid ammonium chloride to 100. mL of 0.016-M HCl? (c) Add 20.0 g NaCl to 1.0 L of 0.012-M sodium acetate, NaCH3COO?A 50.00-mL sample of a white dinner wine required 24.57 mL of 0.03291 M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated).
- A 50.00-mL sample of white wine required 24.57 mL of 0.03291M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated.)Morphine, C17H19O3N, is a weak base (Kb = 7.4 X 10-7) . Consider its titration with hydrochloric acid. In the titration, 50.0 mL of a 0.1500 M solution of morphine is titrated with 0.1045 M HCl.(a) Write a balanced net ionic equation for the reaction that takes place during titration.(b) What are the species present at the equivalence point?(c) What volume of hydrochloric acid is required to reach the equivalence point?(d) What is the pH of the solution before any HCl is added?(e) What is the pH of the solution halfway to the equivalence point?(f) What is the pH of the solution at the equivalence point?You are titrating a 1.033 g sample of white vinegar solution (5.0% acetic acid) with a 1.00 M NaOH titrant. At the endpoint of titration, 0.89 mL of NaOH was used. What is the mass % of acetic acid based on your experimental results? CH3COOH = 60.052 g/mol
- The identity of an unknown monoprotic organic acid is determined by titration. A 0.455 g sample of the acid is titrated with 0.100 M NaOH. What is the molar mass of the compound if 25.3 mL of the NaOH solution is required to neutralize the sample? molar mass: The compound is 60.0% C, 4.48% H, and 35.5% O. What is the molecular formula of the organic acid? formula: g molThis 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…Part b and C What volume of 0.110 M HCI is required for the complete neutralization of 1.10 g of Na2 CO3 (sodium carbonate)? Express your answer to three significant figures and include the appropriate units. A sample of NaOH (sodium hydroxide) contains a small amount of Na2 CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.110 g of this sample requires 23.98 mL of 0.100 M HCI. Ar additional 0.700 mL of 0.100 M HCI is required to reach the methyl orange endpoint. What is the percentage of NaCO; by mass in the sample? Express your answer to three significant figures and include the appropriate units.
- 21 mL of NaOH is used to reach the endpoint in titrating 0.8001 g KHP (204.22 g/mol). How much of the said NaOH solution will be used in neutralizing 10.00 mL of 0.3245 M H₂SO₄? (Note the stoichiometry of your acid and base) CHOICES: 74.89 mL 37.45 mL 45.00 mL None of thesePetanoic (or valeric) acid is a weak organic acid with an unpleasant odour. Like other small carboxylic acids, it is used to make pleasant smelling esters that are used in perfumes, cosmetics, and food additives. Completed Part D In Part B, a 20.00 mL aliquot of a 0.195 mol L-1 pentanoic acid solution was titrated to its equivalence point with 19.7 mL of 0.198 mol L- 1 NaOH solution. At the equivalence point, all of the weak acid, pentanoic acid, is converted to its weak conjugate base, pentanoate. In part A, the Ka for pentanoic acid was determined to be 1.48×10-5. What is the pH at this equivalence point? 5.089 6.997 pentanoic acid 9.170 4.830 The pka of pentanoic acid is 4.830. 8.911An analytical chemist weighs out 0.045 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1800 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 4.2 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g x10 mol