In a different titration experiment, it took 23.96 mL of a 0.105 M solution of NaOH to titrate 20.00 mL of an unknown HCl solution. Calculate the molarity of the HCl solution. HCl(aq)+NaOH(aq)⟶NaCl(aq)+H2O(l)
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In a different titration experiment, it took 23.96 mL of a 0.105 M solution of NaOH to titrate 20.00 mL of an unknown HCl solution. Calculate the molarity of the HCl solution.
HCl(aq)+NaOH(aq)⟶NaCl(aq)+H2O(l)
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- A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?A 20.0 mL sample of vinegar is titrated with 0.108 M NaOH in the presence ofphenolphthalein indicator. If the vinegar requires 39.1 mL of NaOH solution for the completereaction, what is the concentration of acetic acid HC2H3O2 in the vinegar? The reaction is HC2H3O2(aq) + NaOH(aq) → NaC2H3O2(aq) + H2O(l)The endpoint of a titration is reached when 25.6 mL of a 0.100 M solution of Ca(OH)₂ is added to 50.0 mL of an HCl solution with an unknown concentration. The neutralization reaction is 2 HCl (aq) + Ca(OH)₂ (aq) → CaCl₂ (aq) + 2 H₂O (l) Calculate the Molarity of the HCl solution.
- A titration of 25.00 mL of an unknown HCl solution with 0.1550 M NaOH starts at a buret reading of NaOH of 0.33 mL. The phenolphthalein indicator turns light pink in the acid solution over 30 seconds at a buret reading of 24.19 mL. Write the balanced equation for the neutralization reaction. What is the molarity of the HCl solution?You perform an acid-base titration to standardize an HCl solution by placing 50.00 mL of HCl in a flask with a few drops of indicator solution. You put 0.1524 M NaOH into the buret, and the initial reading is 0.55 mL. At the end point, the buret read-ing is 33.87 mL. What is the concentration of the HCl solution?In a titration experiment, 0.27 M NaOH is added to 21.8 mL of a 0.35 M H3PO4 solution and reacts according to the equation: 3 NaOH (aq) + H3PO4 (aq)--------------> Na3PO4 (aq) + 3 H2O (aq) How many milliliters of sodium hydroxide solution have been added at the equivalence point (end point)?
- A solution of tartaric acid (H2C4H6O6) with a known concentration of 0.155 M H2C4H4O6 is titrated with a 0.425 M NaOH solution. How many mL of NaOH are required to reach the second equivalence point with a starting volume of 70.0 mL H2C4H4O6, according to the following balanced chemical equation : H2C4H4O6 + 2 NaOH --> Na2C4H4O6 + 2H2OIn a titration experiment, 0.84 M KOH is added to 34.6 mL of a 0.67 M H2SO4 solution and reacts according to the equation: 2 KOH (aq) + H2SO4 (aq)--------------> K2SO4 (aq) + 2 H2O (aq) How many milliliters of potassium hydroxide solution have been added at the equivalence point (end point)? 2. In a titration experiment, 0.27 M NaOH is added to 21.8 mL of a 0.35 M H3PO4 solution and reacts according to the equation: 3 NaOH (aq) + H3PO4 (aq)--------------> Na3PO4 (aq) + 3 H2O (aq) How many milliliters of sodium hydroxide solution have been added at the equivalence point (end point)?A student titrates a 35.00 mL sample of 0.0100 M sodium hypochlorite (NaClO), a salt containing the conjugate base of hypochlorous acid (HClO, Ka = 3.0 x 10-8), with 0.0125 M HCl.NaClO(aq)+ HCl(aq) → NaCl(aq)+ HClO(aq)Determine the pH of the solution after 30.00 mL of HCl has been added
- Benzoic acid, C6H5COOH, dissociates in water as shown in the equation below. A 40.0 mL sample of an aqueous solution of benzoic acid with a concentration of 0.50 M is titrated using standardized 0.25 M NaOH. C6H5COOH(s) ⇄ C6H5COO–(aq) + H+(aq) Ka = 6.46 x 10–5 a.Calculate the pH of the solution after the following amounts of NaOH have been added… 0 mL 10 mL 85 mL b. State whether the solution at the equivalence point of the titration is acidic, basic, or neutral. Explain your reasoning. c. How many mL of 0.25 M NaOH need to be added in order to make the ideal buffer solution?You perform the following titration. The concentrations and amounts of your reactants are listed below. What is the pH of the final solution?[hint: why did I give you the concentration and volume of BOTH reactants!]Ca(OH)2 (aq) + 2HNO3 (aq) → 2H2O (l) + Ca(NO3)2 (aq)50.00 mL 50.00 mL1.25 M 1.50 MYou are trying to determine the percentage of acetic acid in vinegar by titrating a sample of the vinegar with a standardized NaOH solution. Why is bromcresol green not a good choice for an indicator for this titration? If you do use bromcresol green as an indicator, will your result for the percentage of acetic acid in vinegar be too high or too low? What would be a better choice for an indicator for this titration? Why is your choice better?