By titration, it is found that 70.1 mL of 0.161 M NaOH(aq) is needed to neutralize 25.0 mL of HCI(aq). Calculate the concentration of the HCl solution. [HC1] = M
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![By titration, it is found that 70.1 mL of 0.161 M NAOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the
concentration of the HCl solution.
[HCI] =
M
Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry | Publisher: University Science Books](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4cbada35-3122-4a6c-a25c-246bca0ae236%2Fa12d316e-c9cb-439b-bfc3-98a9d5c4afa1%2F34h7pme_processed.png&w=3840&q=75)
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- Calculate the volume in mL of 0.311 M KOH necessary to titrate 23.38mL of 0.342 M diprotic sulfuric acid, H2SO4 to a phenolphthalein end-point. Report your answer to a precision of 2 decimal places.A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was addedA substance contains 0.5 g of magnesium hydroxide as the only basic ingredient . The sunstamce is analysed by dissolving it and titrating with a standard hydrochloric acid solution .The hydrochloric acid solution used in this titration is made by diluting 200 ml of 2M standardised solution to 500 ml 1.Calculate the volume of the HCl solution required to neutralize two of these indigestion substaces dissolved in water to make 35ml solution and calculate the concentration of Cl- in the final solution in mol.dm-3
- A sample of vinegar weighing 10.52 g is titrated with NaOH. The end point is overstepped, and the solution is titrated back with HCl. From the following data, calculate the acidity of the vinegar in terms of percentage of acetic acid, CH3COOH Standardization Data:1.050 mL HCl ≡ 1.000 mL NaOH1.000 mL NaOH ≡ 0.06050 g benzoic acid, C6H5COOH (122.12 g/mol) Analysis Data:Volume NaOH used = 19.03 mLVolume HCl used for back titration = 1.50 mLCalculate the volume in milliliters of 0.368 M KOH necessary to titrate 0.0209 moles of acetic acid (HOAc, HC2H3O2) to a phenolphthalein end-point. Report the answer with a precision of two decimal places.A 23mL sample of HCl is titration to phenolphthalein end point with 26.43 mL of a 0.09181 M NaOH standard solution. Calculate the molar concentration of the HCl solution.
- Normality is same as Molarity for sodium hydroxide and normal = molar (for NaOH) Normality of sodium hydroxide = 0.10395N (normal) or Molarity of NaOH = 0.10395M (molar) Volume of NaOH consumed during the titration = 21.87 mL Mol wt of Naproxen = 230.26 g/mol Weight of Naproxen ds (i.e., sample) = 0.534g Calculate the % Purity (dried-basis) of Naproxen ds, given that the LOD results for Naproxen = 1.0% a 97.0 b 98.0 c 98.5 d 99.0 e 99.5 f none of the other answers.For an acid-base titration, the moles of the acid should be equal the moles of the base. 30 mL of aliquot of a 0.23N HCl is placed in an Erlenmeyer flask and 2 drops of phenolphthalein was added. It was titrated and had an intial reading of 15.8 The normality of the solution is found to be 0.52N. (a) How much of the NaOH solution is used for the titration? (b) What is the final reading on the buret?For the adjustment of 0.1 M HCl standard solution, 0.1345 g Na2CO3 in primary standard purity was weighed, dissolved in 50 mL of distilled water and titrated with HCl solution. As a result of the titration, 14 mL of acid solution was consumed. Accordingly, what is the true concentration of the HCl solution?
- An approximately 0.1-molar solution of NaOH is to be standardized by titration. Assume that the following materials are available. Clean, dry 50 mL buret •Analytical balance 250 mL Erlenmeyer flask •Wash bottle filled with distilled water Phenolphthalein indicator solution Potassium hydrogen phthalate, KHP, a solid monoprotic acid (to be used as the primary standard) Briefly describe the steps you would take, using the materials listed above, to standardize the NaOH solution. Describe (the set up) the calculations necessary to determine the concentration of the NaOH solution.A tablet contains 0.5 g of magnesium hydroxide as the only basic ingredient . The tablet is analysed by dissolving it and titrating with a standard hydrochloric acid solution .The hydrochloric acid solution used in this titration is made by diluting 200 ml of 2M standardised solution to 500 ml 1.Calculate the volume of the HCl solution required to neutralize two of these indigestion tablets dissolved in water to make 35ml solution and calculate the concentration of Cl- in the final solution in mol.dm-3Benzoic 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 Calculate the pH of the solution after the following amounts of NaOH have been added… A. 0 mL B. 10 mL C. 85 mL
