Referring to the figure below, what volume of the titrant was used to reach half-neutralization equivalence point? 14 •.. 12 10 8 4 10 20 30 40 50 60 Volume of 0.1000 M HC1, mL Figure 8-4 Curve for the titration of 25.00 mL of 0.1000 M Na,CO, with 0.1000M HC1. A) 25 mL 50 mL 56 mL Hd
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- Tony is showing a bacterium having high pH requirement for its growth. He then has to prepare a minimal medium at pH 9. Adding 0.5 ml of the pH indicator to 10 ml of the medium, the solution remained colorless. The pH of the medium was adjusted using 2.25 ml of the 0.05 N titrant. a. What was the pH indicator utilized? b. What is the amount of 1 N titrant needed to adjust 150 ml of minimal medium to pH 9? c.What was the titrant he used?Calculate the alkaline strength of pearl ash (impure potassium carbonate) in terms of percent K2O from the following data: Sample = 0.3500 g; HCl used = 48.03 mL; NaOH used for back titration = 2.02 mL; 1.000 mL HCl = 0.005300 g Na2CO3; 1.000 mL NaOH = 0.02192 g KHC2O4.H2O.A 50ml aliquot of 0.0500 M NaCN (Ka, HCN = 6.2x10^-10) is titrated with 0.1000 M HCl. Discuss which of the following indicators would be best used for the titration of 0.05000 M NaCN with 0.1000 M HCl: bromocresol green (transition range pH: 3.8-5.4), bromothymol blue (transition range pH: 6.2-7.6), or phenolphtalein (8.3-10.0)
- alculate the Ksp of a Ca(OH)2 solution using the data below: Titrated with 0.103MHCl Initial syringe value: 9.71 Final Syringe value: 1.53 Volume of Ca(OH)2 titrated 24.39 mLDouble indicator titration of 1.000g powdered sample containing either alone or any compatible mixture of NaOH/Na2CO3/NaHCO3 and the rest are inert components. The sample was dissolved in 20 ml water then titrated with 0.50 M HCl and reach phenolphthalein endpoint at burette volume of 25.55 ml. Continuing titration, it reached methyl orange endpoint at burette volume of 9.45 ml. Calculate the percentage mass of the possible alkaline component/s.Calculate the alkaline strength of pearl ash ( impure potassium carbonate) in terms of percent K2O from the following data: Sample=0.3500 g; HCl used=48.03 m; NaOH used for back titration=2.02 mL; 1.000 mL HCl = 0.005300 g Na2CO3; 1.000 mL NaOH = 0.02192 g KHC2O4·H2O
- Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution. 2MnO4- + 5C2O4-2 +16H+ -> 2Mn2+ + 10CO2(g) + 8H2O Calculate the molar concentration of the KMnO4 solution. Pls show step by step. What type of molecules will interfere in this analysis ?A 13.0 ml solution of weak base with Kb = 1.33×10-3 (at 25°C) with concentration of 0.086 mol L1 was titrated with 0.100 mol L* hydrochloric acid. What is the pH of the analyte solution at the equivalence point at 25°C? a. 8.79 b. 7.56 c. 9.48 d. 6.23 e. 2.841) Calculate the total hardness for the first sample (Sample Volume,V : 50 mL,Volume of EDTA titrant used for the sample, A:9.6 mL) 2)Calculate the calcium and magnesium concentrations for the first sample in the video in meq/L and mg CaCO3/L.(Sample Volume= 50 mL, Magnesium hardness titrant volume = 0 mL, Calcium hardness titrant volume:2,6 mL) 3)Assuming the pH and alkalinity of the first sample in the video are 7.5 and 100 mg CaCO3/L, respectively, calculate the temporary and permanent hardness values for this sample 4How much CaCL2 in meq/L should be added to the sample to equalize calcium and magnesium hardness? Which hardness level (soft, medium, hard, very hard) does the sample belong to after this addition?
- Calculate the alkaline strength of pearl ash (impure potassium carbonate) in terms of percent K2O from the following data: Sample = 0.3500 g; HCl used = 48.03 mL; NaOH used for back titration = 2.02 mL; 1.000 mL HCl = 0.005300 g Na2CO3; 1.000 mL NaOH = 0.02192 g KHC2O4.H2O. (Note: Use the least significant digits in your answer.)Give the proper scientific description of 50x TAE Buffer given the information below. 242 g Tris base 57.1 mL glacial acetic acid 18.61 g disodium EDTA Up to 1L with dI waterThe mass percent of Fe in an unknown salt sample was determined using both volumetric and gra vimetric titration. Ten determinations using both methods were performed. Volumetric(% of Fe): 24.22, 23.86, 24.07, 24.49, 24.69, 23.71, 24.28, 24.11, 24.26, 24.10 Gravimetric (% of Fe): 24.35, 24.26, 24.10,24.19, 24.18, 24.32, 24.11, 24.33, 24.17, 24.12 a. Do the two methods give similar standard deviations? b. Do the two methods give similar results for the mass percent of Fe at the 95% confidence level?