Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH3CH2CH2COOH (Ka = 1.54 x 10 5 ), with 0.1000 M NaOH solution after the following additions of titrant. (а) 10.00 mlL: pH (b) 20.10 mL: pH (c) 29.00 mL: pH = I.
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- You have performed an iodimetric titration using a commercial vitamin C tablet. Based on the following information below, calculate the %(w/w) of vitamin C(MM=176.16 g/mol) in the tablet: Mass of tablet dissolved in 250.0 mL: 5.422 g Aliquot volume of sample titrated: 25.00 mL Concentration of KIO3: 0.023 M Final burrette volume: 41.31 mL Initial burrette volume: 8.89 mL Blank volume: 0.14 mLWhat is the molarity of a commercial phosphoric acid solution, H3PO4 (MW= 98.0 g/mol) that is 85.0% (w/w) and has a specific gravity of 1.689? Also Make a graph of pH versus VHCl for the titration134 grams of potassium sorbate KCH3 (CH)4CO2 is fully dissolved in 100.00 mL of water, which is carefully transferred to a conical flask. Then 100.00 mL of 0.240 M HNO3 is added dropwise to this solution from a burette. Given: Ka (sorbic acid) = 1.7 × 1O^-5 Showing all your calculations and reasoning, determine the pH of the solution that results after the addition of all the acid mentioned above. Suppose that the titration continues. Determine the pH of the solution in the flask at theequivalence point
- 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?20.00mL of 6M HCl is taken from 500mL bottle containing the acid and is transferred to 250mL volumetric flask and diluted to volume with water. What is the molarity of the new solution? Do not enter units with your answer.In developing a method for the determination of formic acid by neutralization volumetry, an analyst calculated the pH as a function of the addition of NaOH for the titration of 30.00 mL of 0.1280 mol/L formic acid with standardized NaOH with concentration of 0.1570 mol/L. With respect to this titration curve, determine the pH of the solution after adding the following volumes of NaOH: 0.00 mL; 10.00 ml; 25 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two decimal places and show your calculations.
- Following titration analysis, a sample of a fruit juice was found to contain 8.9 mg cm-3 ascorbic acid. Given that the Mr value for ascorbic acid is 176.1 Da, calculate the value of the ascorbic acid concentration expressed in units of mmols dm-3 then enter itIf a 0.3 M solution of NaOH was used to titrate 100 mL of 0.3 M solution of CH3COOH (Ka =1.8 x 10 -5) and the following volumes of NaOH were recorded: 102, 97, 99, 98, 101, 106 mL. The pH Value is………………when added 99.0 mL of 0.3 M NaOH The pH of the solution at the equivalence point more than 7 Because................................... Calculate the 99% confidence limits of the mean? And use them to decide whether there is any evidence of systematic error? [ hints: For N=6 and the 99 % confidence interval, the value of t is 4.03].In a titration, 10.543 mL of a 1.112 M weak acid solution are placed in a 125 mL Erlenmeyer flask. A 1.249 M solution of NaOH (aq) is placed in the buret and filled to the 0.00 mL mark. NaOH solution is added to the flask and the buret reading is now 18.119. What is the pH of the solution? Enter your answer with at least 4 sig figs. The pKa of the weak acid is 4.954. (please type answer not write by hend)
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