Determine the volume in mL of 0.652 M CSOH(aq) needed to reach the half-equivalence (stoichiometric) point in the titration of 49.6 mL of 0.873 M HBRO(ag). The Ka of HBro is 2.3 x 10-9. Enter your answer in exponential format using a capital "E" (example 1.23E-4) and no units (value + 2%).
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- Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was addedFor 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?
- 50 mL sample solution containing Na2CO3 and NaOH is titrated with 0.2 M HCl solution. In the presence of phenolphthalein indicator, the acid consumption is 15 mL. Then, the titration is continued by adding bromocresol green indicator, and in the presence of this indicator, the acid consumption is 10 mL. Accordingly, which of the following is the amount of Na2CO3 (in grams) in the sample? (NaOH: 40 g / mol; NazCO3: 106 g / mol)What is the best way to calculate the following titration: 100 ml water and 100 ml of solution with citric acid with pH2 is mixed togeather so the total volume is 200 ml. Then i titrate with NaHCO3 with the following grams. 0.62 gr , 1.82 gr , 2.40 gr What is the pH after each addition of NaHCO3. Please show details, along with the pKa and how it is used as I am very stuck on this and getting it wrongGive typed full explanation not a single word hand written otherwise leave it An experiment requires a pH 6.5 buffer. Solid sodium acetate and glacial acetic acid available. Glacial acetic acid is 99% acetic acid by mass and has a density of 1.05 g/mL. If the buffer is to be 0.20 M in acetic acid, how many grams of NaC2H3O2 and how many milliliters of glacial acetic acid must be used?
- Calculate the volume in milliliters of 0.368 M KOH necessary to titrate 0.0209 moles of acetic acid (HOAc, HC2H3O2) to a phenolphthalein end-point. Report the answer with a precision of two decimal places.Need solution urgently 125mL of an alkaline water sample containing 128 ppm carbonate and 40ppm hydroxide in terms of CaCO_(3) equivalent its titrated against 0.20NHCl using methyl orange as the indicator.What will be the titre value (in ml unit)?What mass of Ba(OH)2 is present in a sample if it is titrated to its equivalence point with 44.20 mL of 0.1000 N H2SO4? Note: Present complete solutions for the following problem. Express your final answers up to two (2) decimal places.
- A sample of 0.10 M CH3COOH(aq) of volume 25.0 cm3 is titrated with 0.10 M NaOH(aq). The Ka for CH3COOH is 1.8 x 10-5. (a) What is the pH of 0.10 M CH3COOH(aq)? (b) What is the pH after the addition of 10.0 cm3 of 0.10 MNaOH(aq)? (c) What volume of 0.10 M NaOH(aq) is required to reach halfway to the stoichiometric point? (d) Calculate the pH at that halfway point. (e) What volume of 0.10 M NaOH(aq) is required to reach the stoichiometric point? (f) Calculate the pH at the stoichiometric point.A 21.3 mL solution of HBr (a strong acid) of unknown concentration was titrated using 0.2735 mol L-1 NaOH using phenolphthalein as a pH indicator. At the moment when the solution turned a consistent light pink colour, the burette volume read 29.78 mL. The initial burette reading before the experiment was 7.15 mL. What was the concentration of HBr in the original HBr solution in mol L-1 ?A sample of 0.1687 g of an unknown monoprotic acid wasdissolved in 25.0 mL of water and titrated with 0.1150 MNaOH. The acid required 15.5 mL of base to reach theequivalence point. (a) What is the molar mass of the acid?(b) After 7.25 mL of base had been added in the titration,the pH was found to be 2.85. What is the Ka for the unknownacid?