The KHP titer of NaOH is 40.84mg/mL. Determine total acidity if 18.00mL of NaOH is required to titrate 5.00mL vinegar sample. Give the chemical reactions involved.
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Q: Question 28
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The KHP titer of NaOH is 40.84mg/mL. Determine total acidity if 18.00mL of NaOH is required to titrate 5.00mL vinegar sample. Give the
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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.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.)
- 4. Complete neutralization of 10 mL of hydrochloric acid solution by NaOH 0.1 N in the presence of phenol phthalein until the appearance of purple color (pHf= 9) 15 mL of NaOH is consumed. (a) What is the concentration of hydrochloric acid? (b) Calculate the indicator error.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/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…
- Maleic acid (H2C4H2O4, represented by H2M) is the precursor of malic acid widely used in industry. food as an acidulant and in the pharmaceutical industry it is used in the treatment of wounds. This acid can be determined by neutralization titration. Answer the items below about this determination. Considering a 15.0 mL sample of maleic acid-based product used in industry, determine the maleic acid concentration, in mol/L, in the sample knowing that 21.7 mL of a solution of 0.1120 mol/L NaOH for complete neutralization of this acid. How many grams of maleic acid were in the sample analyzed and what is its percentage (%, m/v) in the sample? [Answer; m=0.1405 mol L-1; percentage = 0.9365%] NaOH(aq) + H2M(aq) Na2M (aq) + H2O(l) Suggest an appropriate indicator for the titration of this acid by looking at the titration curve profile below (IMAGE)Chem. 1A: Acid-Base titration : to determine molar mass of a diprotic ACID : H2A Put a weighing paper on the pan of balance and tare it. Then add 0.1482 g of an unknown diprotic acid. Transfer the acid to a Erlenmeyer flask add 35.0 mL. water and 4 drops phenophethaleine. The color of solution is colorless. Set up a 50.00 mL. buret: wash the buret with tap water twice, with deionized water twice and and the 0.1029 M NAOH(aq). Fill the buret with 0.1029 M NaOH(aq), remove the air bubble and adjust the initial buret reading to 0.00 mL. Put the Erlenmeyer flask containing the acid and the phenolphethaleine below the buret with 0.1029 M NAOH(aq). Add NaOH(aq) from buret to the Erlenmeyer flask containing the diprotic acid and phenolphethaleine , until the color of the solution turn to pink by adding one or two drops of NaOH(aq). Then stop adding NaOH(aq) from buret and read the final volume of NaOH(aq). Acid-base titration: buret base of known concentration + stopcock acid of unknown…1. ) What weight of 98.5% KHC,HO, is equivalent to (a) 35 ml of 0.01 N NaOH, 2.) A 50.00-ml sample of calcium hydroxide solution required 19.50 ml of 0.1050 N hydrochloric acid in a titration. Calculate (a) the amount of Ca(OH), in the 50.00-ml sample and (b) the Ca(OH) a concentration in % w/v. 3.) If 25.00 ml of a hydrochloric acid solution were required in titration of a 0.6500-g sample of pure sodium carbonate, what weight of each of the following pure reagents would be required to neutralize 25 ml of the hydrochloric acid solution? (a) NaHCO3. (b) KOH, (c) Ba(OH)2• (d) Cao. 4.) If 25.00 ml of a sodium hydroxide solution required 40.00 ml of a sulfuric acid solution in a titration, and 25.00 ml of the sulfuric acid solution were required in the titration of 0.3060 g of pure sodium carbonate, what was the normality of the sodium hydroxide solution? 5.) If 25.00 ml of a sulfuric acid solution were found to be equivalent to 20.50 ml of a sodium hydroxide solution, and 35.00 ml of the…
- How many milliliters of 0.0850 M NaOH are required to titrate each of the following solutions to the equivalence point: (a) 40.0 mL of 0.0900 M HNO3, (b) 35.0 mL of 0.0850 M HC2H3O2, (c) 50.0 mL of a solution that contains 1.85 g of HCl per liter. Be sure to write the balanced titration reaction for each.Which statement about acid-base indicators is not correct? * A- A weak acid can be used as an acid-base indicator provided that the chemical structures of the weak acid and its conjugate base differ slightly. B- The end point of the titration is not a specific colour but the point where one drop of acid or base from the burette changes the colour of the solution in the conical flask. C- Phenolphthalein can be used to detect the end point of the titration of a strong base with a weak acid. D- All these statements are correct. E- None of these statements are correct.You are studying a clear solution and you added the pH indicator methyl violet. The colour range of the indicator methyl violet in a clear solution when changing from acidic to basic is yellow (pH 0) to blue purple (pH 1) to violet (pH 2). You initial pH of the solution when tested with a pH meter is O.2. You are going to add 250 drops of 0.1 M HCI. Please select the most appropriate answers to the following two questions. What is the initial colour of the solution at pH 0.2? What is the colour of the solution and what will the pH be after the addition of the HCI? Select 2 correct answer(s) The colour of the solution after the addition of HCI will be clear and the pH will be less than 0.2. The colour of the solution after the addition of HCI will be violet and the pH will be higher than 0.2.