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- 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?Would the indicator bromocresol green, with a transition range of pH 3.8–5.4, ever be useful in the titration of a weak acid with a strong base? Why?What volume in mL of 0.2572 M NaOH must be added to 500.0 mL of 0.1000 M chlorous acid (HClO2, Ka = 1.10 x 10–2) to produce a buffer solution with a pH of 2.25?
- A solution containing Mg2+ was buffered to pH 9.99 and titrated with EDTA. Eriochrome black T, with p?a1 = 6.3 and p?a2 = 11.6 was used as the indicator. It is a diprotic acid, H2E What is the fraction of the predominant form of eriochrome black T in solution at this pH? (To answer this, report the alpha fraction of the indicator’s most prevalent species at this pH)Calculate the mass of sldium thiosulfate necessary to prepare .5L of the .10M Na2S2O3 titrant.In the titration of 20 mL CH3COOH (Ka = 1.76 x 10-5) 0.4 M with a solution of NaOH 0.4 M, calculate the pH of the resulting solution after addition of: 30 mL NaOH
- Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 247 mL 0.0581 M 3‑(N‑Morpholino) propanesulfonic acid (MOPS) to give the solution a pH of 7.55. The pKa of MOPS is 7.18.If a 3g sample of zinc oxide, 95% ZnO, were treated with 50ml of 1.1230N sulfuric acid in the usual way, what volume of 0.9765N sodium Hydroxide would be required in the residual titration?I was just wondering how you got the 4.0 x 10-4 for the acidionzation constant.
- An alkaline sample of sodium compounds weighing 1.196 g was dissolved in water, cooled at 15 deg C, treated with 2 drops of phenolphthalein indicator and titrated with 1.058 N H2SO4 requiring 6.8 mL to render the solution colorless. Upon adding 2 drops of methyl orange and continuing the titration 16.5 mL more of the acid was needed to complete analysis. What is the quantitative composition of the sample?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 mLb. A student has a sea water sample which contains Ca2+ ions . Describe briefly how he willdetermine the concentration of Ca2+ ion in the sample using a simple titration. Explain the colourchanges at the endpoint. Which medium is suitable for performing the titration, acidic or basic medium and why?