H₂S to 25.00 mL of acidified standard 0.010 44 M 15 to precip tate elemental sulfur. (If [H₂S]> 0.01 M. then precipitated sulf traps some I solution, which is not subsequently titrated.) T remaining I was titrated with 14.44 mL of 0.009 336 M Na₂S₂C Find the molarity of the H₂S solution. Should starch indicator added to this titration at the beginning or just before the en point?
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- A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCl, evaporated to incipient dryness and quantitatively transferred to a 250 mL volumetric flask, and diluted to mark. A 10 mL of aliquot was then transferred to an Erlenmeyer flask, together with 5mL buffer and 5 drops of EBT indicator, and was used to standardize the EDTA titrant. The solution turned blue after the addition of 24.10 mL of EDTA. A blank correction was performed and was determined to be 0.4 mL. What is the concentration of EDTA obtained (MW CaCO3 = 100.0869 g/mol)?A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCl, evaporated to incipient dryness, and quantitatively transferred to a 250 mL volumetric flask and diluted to mark. A 10 mL of aliquot was then transferred to an Erlenmeyer flask, together with 5mL buffer and 5 drops of EBT indicator, and was used to standardize the EDTA titrant. The solution turned blue after the addition of 24.10 mL of EDTA. A blank correction was made and was determined to be 0.4 mL. [Analysis] A 30 mL unknown water sample was treated with 37.6 mL of EDTA. A blank correction was made and was determined to be 0.4 mL. What is the concentration of Ca2+ (40.0780 g/mol) in ppm?The equilibrium constant for the conjugate acid-base pair HIn+H2OH3O++In is 8.00 10-5. From the additional information in the following table, (a) calculate the absorbance at 430 nmand 600 nm for the following indicator concentrations: 3.00 10-4M,2.00 10-4M, 1.00 10-4M, 0.500 10-4 M, and 0.250 10-4M. (b) plot absorbance as a function of indicator concentration.
- 10mL of a 10% by weight MgCl2 solution (density = 1.1 g / mL) is precipitated as magnesium ammonium phosphate after necessary processes, filtered and washed. The precipitate is dissolved in 50mL 1M HCl and excess acid is titrated with 2.0M NaOH solution in the presence of methyl orange. Find the NaOH consumption (Mg = 24,3g / mol, Cl = 35,5g / mol)Triplicate samples of NaOH was found to have concentrations of 0.1444 M (Trial 1), 0.1107 M (Trial 2), and 0.1160 M (Trial 3) upon standardization. a.) What is the appropriate primary standard and chemical indicator for this particular titration process? b.) If the volumes of NaOH used during the titration are 10.55 mL, 15.35 mL, and 14.50 mL for Trial 1, 2, and 3, respectively, what is the average weight ± SD of the primary standard?The concentration of ammonia in a cleaning product was determined by back titration.Firstly, 10.00 cm3 of the cleaning product was pipetted into a large conical flask,containing 250.00cm3 of 0.50 mol/l HCl to give Solution A.Following a period of reaction and shaking, 50.00cm3 of Solution A was removed anddiluted to 250 cm3 with water in a volumetric flask to give Solution B.20 cm3 samples of Solution B were titrated against 0.05 mol/l Na2CO3 solution, givingan average titre of 12.45 cm3. i) Write equations for the reactions that have taken place.ii) Determine the concentration of NH3 in the original cleaning product in mol/l,g/l, ppm, and % w/v.
- Compute the titration curve for Demonstration 16-1, in which 400.0 mL of 3.75 mM Fe21 are titrated with 20.0 mM MnO24 at a fixed pH of 0.00 in 1 M H2SO4. Calculate the cell voltage at titrant volumes of 1.0, 7.5, 14.0, 15.0, 16.0, and 30.0 mL and sketch the titration curve.A 20 ml aliquot of malonic acid solution was treated with 10.0 ml of 0.25M Ce4+ leading to the reaction CH2(COOH)2 + 6Ce4+ + 2H2O ® HCOOH + 2CO2 + 6Ce3+ + 6H+ After standing for 10 minutes at 60oC, the solution was cooled and the x’ss Ce4+ was titrated with 0.1M Fe2+, requiring 14.4 ml to reach the ferroin end point. Calculate the M of the malonic in the sample.The % (w/w) I- (MM = 126.9) in a 0.5812-g sample was determined by Volhard titration. After adding 50.00 mL of 0.06912 M AgNO3 and allowing the precipitate to form, the remaining silver was back-titrated with 0.07012 M KSCN, requiring 36.17 mL to reach the endpoint. Report the %(w/w) I- in the sample. 17.76 % 20.08 % 35.52 % 40.16%
- For Determining Carbonate in Soda Ash... Utilize primary Standard Na2CO3(FW = 105.99) and titrant 0.1 M HCl... with the reaction also use Bromocresol Green or Methyl Orange as indicators . What two other indicators can use aside from Bromocresol Green and Methyl Orange for the titration?A sample is analyzed for chloride by the Volhard method. Calculate the %KCl from the following data: Wt of sample = 0.5000g; Vol of AgNO3 added = 35.00ml; M of AgNO3 = 0.1157; Vol of SCN- used for back titration = 14.71ml; M of SCN- = 0.08598; Atomic wts: Ag = 107.87, N = 14.00, Cl = 35.5, O = 16.00An 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?