7. A formula calls for 0.6 mL of a coloring solution. Using a 10-mL graduate calibrated from 2 to 10 mL in 1-mL units, how could you obtain the desired quantity of the coloring solution by the aliquot method? Use water as the diluent.
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7. A formula calls for 0.6 mL of a coloring solution. Using a 10-mL graduate calibrated from 2 to 10 mL in 1-mL units, how could you obtain the desired quantity of the coloring solution by the aliquot method? Use water as the diluent.
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- 148. Addition of 50.00 mL of 2.238 m H2SO4 (solution density = 1.1243 g/mL) to 50.00 mL of 2.238 M BaCl2 gives a white precipitate. (a) What is the mass of the precipitate in grams? (b) If you filter the mixture and add more H2SO4 solution to the filtrate, would you obtain more precipitate? Explain.The Kjeldahl method was used to determine the nitrogen content of a soil sample. 25 g soil sample was digested and the liberated ammonia distilled into 10 mL of 0.05 M HCl, which was used in the subsequent back titration. The unreacted HCl required 13.25 ml of 0.025 M NaOH for complete titration. Calculate the Total Kjeldahl Nitrogen (TKN) in mgkg¹¹ N.Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. Ni(NO3)2From the stock solution (1.0 M), determine the volume needed to prepare 0.00, 0.04, 0.08, 0.12 and 0.16 M Ni(NO3)2 solution in 50 mL volumetric flask. Obtain the calculated amounts, place in corresponding volumetric flasks and dilute to mark.
- 3. A 0.1093-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the end point. Report the purity of the Na2CO3 sample.If you prepared a solution of KOH by weighing out 4.750 g of solid KOH that had a purity of 84.6 % and then diluted this to a final volume of 1 L in a volumetric flask, what would be the % mass of KHP in an unknown sample with 0.555 g of mass if it required 20.34 mL of KOH titrant to reach the endpoint? PLEASE show your1. If the concentration of a stock solution is 0.152 M, what is the concentration of 10.0 mL of thestock solution diluted into a 100-mL volumetric flask? Show your work.2. If you were to have a stock solution with a concentration of 1.475 M and performed a serialdilution as shown in Fig. 5.1, what would the concentrations be in flasks A, B, C, and D?3. If you wished to study the molecule below by measuring absorbance, what wavelength shouldyou set your spectrophotometer to?
- 1. A group of students from the instrumental analysis laboratory of the course analyzed the sodium content in a serum sample using ICP-OES. They used 5 flasks with 25 mL of sample serum in each and added different amounts of a standard 2.640MNaCl solution to a total volume of 50 mL . Calculate: a. Equation for calibration b. Serum sodium concentrationShow your complete solution and round-off your answers to four decimal places. A 0.1093-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.06911 N AgNO3, the sample was back titrated with 0.05781 N KSCN, requiring 27.36 mL to reach the end point. Calculate the % purity of the Na2CO3 sample. Answer = _% Na2CO3The thiourea in a 1.455 g sample of organic material was extracted into a dilute sulfuric acid solution and titrated with 37.31 mL of 0.009372 M Hg2+ via reaction: 4(NH2)2CS + Hg2+ →[(NH2)2CS]4 Hg2+ Is this an example of total analysis technique or concentration technique? Explain. Calculate the percent (NH2)2CS ( 76.12 g/mol) in the sample. What is classification of the analysis based on the amount of sample and amount of analytes present? Explain.
- I add 0.1011 g of a primary standard FAS into a volumetric flask and diluted it to the line with water. We then add 2 mL of that solution into another 100 mL volumetric flask and diluted to the line with water. What would be the concentration of the diluted solution in g/mL?A 25.00 cm3 solution containing Ni2+ was treated with an excess of an ammoniacal solution of dimethylglyoxime (dmgH2) and 0.7223 g of Ni(dmgH)2 was precipitated. What is the molarity of Ni2+ in the solution in mol dm–3? [Mr / g mol–1: Ni(dmgH)2 = 288.9149] a. 1.000 × 10–3 mol dm–3 b. 1.00 × 10–1 mol dm–3 c. 1.0 × 10–1 mol dm–3 d. 1.000 × 10–1 mol dm–3 e. 1.0 × 10–3 mol dm–3When standardizing two liters of a potassium permanganate solution, approximately 0.0100 M, with a primary standard solution of sodium oxalate, it was planned to use between 30.00 and 45.00 ml of the titrated reagent. In which mass range (in grams) the primary standard should be weighed?