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- Part B Calculate the percerit lonization of 0.130 M lactic acid in a solution containing 0.0080 M sodium lactate. Express the percent lonization to two significant figures. View Available Hint(s) ΜΕ ΑΣΦΑ Submit ? %I made some titrations and the calculated molarity of HCI was 0.096, 0.097 and 0.098. The nomical concentrsrion of HCl is 0.1. How can I explain my results by comparing it to the nominal concentration if my confidence intervals don't include the nominal concentration?3. Complete neutralization of 10 ml of phosphoric acid solution by NaOH 0.I N in the presence of phenol phthalein until the appearance of purple color (pH, = 9) 11 ml. of NaOH is consumed. (a) What is the concentration of phosphoric acid? (b) Calculate the indicator error. pk2.1 pK. - 7.2 pK - 124
- 5- Instrumental methods of analysis example such 6- Acid equivalent weight can calculated by division of M.wt on the 7- Calculated the equivalent weight for CaC12 Ca-40, Cl-35 8- Calculated the equivalent weight for( KMno3) K=39, Mn-55, o-16 KMN0, + 8H* + 5eMn*2 + 4H20If K = 2.35 & K, 1.32 x 1010, Suppose 50ml of 0.010M aqueous amine is extracted with 100ml of benzene. What % will remain in aqueous sol" at (a) pH - 9 and (b) pH = 11.0 OA a. 51.1% b. 18.9% В. a. 29.2% b. 14.9% a. 48.6% b. 24.2% O D. a. 64.6%If K=2.25 & K,- 5.62 x 1010, Suppose 100 ml of 0.010M aqueous amine is extracted with 300ml of benzene. What will remain in aqueous sol" at (a) pH = 9 and (b) pH = 10.0 A. a. 48.6% b. 24.2% B. a. 29.2% b. 14.9% a. 28.9% b. 5.6% D. a64.6% b. 18.0% Beset Selection
- Ex. 13-5. A 50.00-mL of an HCl solution required 29.71 mL of 0.01963 M Ba(OH)2 to reach an end point with bromocresol green indicator. Calculate the molarity of the HCl. Ва(ОН)2 + 2HCІ- ВаCl, + 2H-0What conditions must be followed to perform complexometric titration?A 50.00 (±0.03) mL portion of an HCl solution required 29.71(±0.03) mL of 0.01963(±0.0030) M Ba(OH)2 to reach an end point with bromocresol green indicator. The molar concentration of the HCl is calculated using the equation below (attached image): a.) Calculate the uncertainty of the result (absolute error). M=0.02333(±?????) M b.) Calculate the coefficient of variation for the result. CV= (Sy/y) x 100%
- *which of the following are correct of the Procedural Steps: toit □ The PH meter be calibrated before use. 109, 9/ Used solutions, □ A 25.0 ml Sample of vinegar is diluted to 250ml □ Solutions of Known PH; called buffer are to calibrate the pH meter. □PH and volume measurements are collected approximately every 0.2 change in PH. of (spropst pak Ord noi tulo? Not od to smolou thy09 344 7) NO 1917, no 11 SHE 20 ENOT STEF bit OUSIN p 401 gonsloviope pr 5 10 triot Song Lovrops holo) 69 sub of bonp⁹7 2999912 70 70/4 TO6) Bu analyst in a solution uning two dierent indicators. lis results were an /lowes : meanired the con cen tration n aid Mean [HCI]+ Stand Dev. 002467テ 0.0045 Indi cator A: 18 12 Indicator B: 0-02407 チ0.0032 Is the difference between te tueo indican Ys figniticand at he 95%. confiden ce loue/?In the experiment, we used titration to determine the total acid content ofsamples, which we reported in terms of molarity. Reporting acidity through pHmeasurements is quite different, in that we can only measure the amount of theacid in its ionized form. You were tasked to investigate a clear aqueous solutionof an unknown monoprotic acid. You decided to use two methods togather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mLdistilled water. Two drops of phenolphthalein were added and then it was titrated3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip toestimate the pH, which turned out to be around 3.3. Another 1 mL of the samplewas diluted with 9 mL of water. The pH was taken again and is now around 3.8.a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict thepH of the sample.c) Using pH strip results,…