A 50.0 ml of acidic solute (Ka = 1.20 x 10-2) is titrated with a %3D 2.50 mL of 1.00 x 10-5 M NAOH solution. Which of the following indicators would be best for this titration? Indicator pKa methyl orange methyl red bromocresol purple 6.12 bromthymol blue thymol blue phenolpthalein 3.46 5.00 7.10 8.90 9.10 Methyl red
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Q: A 50.0 ml of acidic solute (Ka = 1.20 x 10 2) is titrated with a 2.50 mL of %3D 1.00 x 10-5 M NaOH…
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A: the answer is as follows:
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- 5. How would you prepare a liter of “carbonate buffer” at a pH of 10.10? H2CO3 ↔ H+ + HCO3- Ka = 4.2 x 10-7 HCO3-↔ H+ + CO3-2 Ka = 4.8 x 10-11 a 1stbuffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solution b 2ndbuffer is preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution c 1stbuffer preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution d 2nd buffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solutionA 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)A 10.00cm3 portion of the 100.00cm3 HCl solut was taken from the volumetric flask and was titrated with KOH (aq). It was neeutralized by 24.35cm3 of potassium hydroxide od concentration 0.0500moldm-3. Calculate the concentrat of the original concentrated hydrochloric acid in moldm-3.
- 2. A 0.5131-g sample containing KBr is dissolved in 50 mL of distilled water. Titrating with 0.04614 M AgNO3 requires 25.13 mL to reach the Mohr end point. A blank titration requires 0.65 mL to reach the same endpoint. Report the %w/w KBr in the sample.A biochemist needs 750 mL of an acetic acid–sodiumacetate buffer with pH 4.50. Solid sodium acetate(CH3COONa) and glacial acetic acid (CH3COOH) areavailable. Glacial acetic acid is 99% CH3COOH by massand has a density of 1.05 g/mL. If the buffer is to be 0.15 Min CH3COOH, how many grams of CH3COONa and howmany milliliters of glacial acetic acid must be used?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 X3
- 10.00 mL of 0.2099 M iodic acid {Ka = 1.70 xx 10^(-1)} is titrated with 0.1057 M NaOH. a) What is the pH after 14.61 mL of NaOH are added to the solution?A sufficient quantity of each of the following aqueous solutions has been made available to you: (i) 0.2M NaH2PO4; (ii) 0.1M Na2HPO4 (a) How many ml of each of these two solutions would you require to mix together in order to prepare one litre of a 0.01M phosphate buffer pH 7.2? [For H3PO4: pKa1 = 2.15; pKa2 = 6.82; pKa3 = 12.38]. (Ans. = 14.7 ml 0.2M NaH2PO4; and 70.6 ml Na2HPO4). (b) Having calculated these volumes (of 0.2 M NaH2PO4 and 0.1M Na2HPO4) required, what further steps would you take to prepare the 0.01M phosphate buffer solution of pH 7.2?Acetic acid has a Ka of 1.8 x 10-5. Calculate the pH at the point when 30.00 mL of 0.150 M NaC2H3O2 is has been mixed with 37.2mL of 0.125 M HBr.
- Phenolphthalein indicator is a weak acid with Ka = 10-9 mol/dm-3. It is colourless while its conjugate base is pink in solution. Calculate the ratio of the number of pink particles to the number of colourless particles of this indicator in a solution of pH = 9Q.1: Determination of % composition of mixture of KI & KNO3 using Eoscein as indicator.Calculate the pH at the following points in a titration of 40. mL (0.040 L) of 0.145 M 4-chlorobenzoic acid (Ka = 1.0 ✕ 10−4) with 0.145 M KOH. (Assume Kw = 1.01 ✕ 10−14.) When 40. mL of KOH solution added?