A solution contains a mixture of Na;CO3 and NaOH. Using phenolphthalein indicator 25 mL of mixture required 19.5 mL of 0.995 M HCI for the endpoint. With methyl orange, 25 mL of solution required 25 mL of the same HCI for the endpoint. Calculate grams per liter of NazCO3 in the mixture. (А) 23 (в) 11 78 D) 36
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- One Erlenmeyer contains 50 mL of 0.1 M Na2CO3 solution, the other Erlenmeyer contains 50 mL of 0.1 M NaHCO3 solution. Answer the following questions when both solutions are titrated with 0.1 M HCl (F=1) solution separately: a) How much mL will be consumed if the phenolphthalein indicator is used? b) How much mL will be consumed if the methyl orange indicator is used? please explain than solveSolution D: 20.0 mL of 1:1 buffer + 5.0 NaOH (Please type answer no write by hend)100ml of asample of water required 10 ml of N/10 acid for titrating using phenolphthalein indicator. A100 ml sample of water was again taken and methyl orange was used as indicator, when15ml of N/10 acid was required for neutralization. Interpret the results of alkalinities in ppm.
- Chemistry a malate buffer solution.Are any of the following true at the equivalance point? The analyte is present in excess, the titrant is present in excess, both the analyte and titrant are present in excess, neither the analyte or titrant is present in excess, the yield is 50%Exactly 50.00 mL of an HCl solution required 29.71 mL of 0.01963 M Ba(OH)2 to reach an end point with bromocreasol green indicator. What is the molarity of HCl?
- Moles of NaOH at the equivalence point? Mass of H2C2O4·2H2O= 1.32191 g Volume of the H2C2O4·2H2O solution= 250.0 mLWhy are the acidic and basic extracts cooled before neutralization?1. This should be displaced from tips of buret before titration 2. The chemical name of a weak monobasic acid which is soluble in a mixture of alcohol and water. 3. A solution whose concentration is known to a high degree of accuracy
- 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,…Consider the spectrophotometric pH measurement of seawater with the indicator thymol blue illustrated at the opening of this chapter. The blue form of the indicator In22 on page 202 has maximum absorbance at a wavelength of 596 nm (nanometers). The yellow form HIn2 has maximum absorbance at 435 nm. Measurements of absorbance at the two wavelengths allows us to find the ratio [In22]/[HIn2]. How would you use this measurement to find the pH?Please answer with complete solutions. Do not use spreadsheet. Thank you A series of solutions containing NaOH, Na2CO3, and NaHCO3, alone or in compatible combination, was titrated with 0.1202 M HCl. Tabulated below are the volumes of acid needed to titrate 25.00-mL portions of each solution to (1) a phenolphthalein and (2) a bromocresol green end point. Use this information to deduce the composition of the solutions. In addition, calculate them molar concentration. (1) Phenolphthalein End Point (2) Bromocresol Green End Point a 22.42 22.44 b 15.67 42.13 c 29.64 36.42 d 16.12 32.23 e 0.00 33.33