Using the diagram below, explain how you would prepare serial dilutions of 10-3, 10-5 and 10-6 of a milk sample. Please include all the details below in your answer. Tube 1: volume of diluent, volume of sample added ==> dilution achieved Tube 2: volume of diluent, volume of sample added ==> dilution achieved
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- 2.0x10^-4bmoles of s4o8^2- in 50ml of solution is consumed in 188 seconds , what is the rate of consumption of s2o4.50.00 cm3 of a 1.5784 mol.dm-3 solution of potassium hydroxide is transferred to an empty 700.00 cm3 volumetric flask. This flask is made up to the mark with distilled water and then shaken well. The concentration of the potassium hydroxide in this second flask is:Beaker 0.00200 M Fe(NO3)3, mL 0.00200 M NaSCN, mL total volume, mL 1 3.000 2.000 10.00 2 3.000 3.000 10.00 3 3.000 4.000 10.00 4 3.000 5.000 10.00 5 (blank) 3.000 0.000 10.00 In Solutions 1-4 you are adding successively larger volumes of 0.00200M SCN- to the Fe3+ solution and diluting to 10.00 ml. Calculate the final diluted molarity of SCN- in solution #1 Your answer should have 3 sig figs =
- A student performs a crystallization on an impure sample of biphenyl. The sample weighs 0.5 g and contains about 5% impurity. Based on his knowledge of solubility, the student decides to use benzene as the solvent. After crystallization, the crystals are dried and the nal weight is found to be 0.02 g. Assume that all steps in the crystallization are performed correctly, there are no spills, and the student lost very little solid on any glassware or in any of the transfers. Why is the recovery so low?A 1 mL sample of glycogen was calculated to contain 21 µmol (micromole) glucose. To 1 mL of this sample was added 2 mL of 2 M HCl. It was then hydrolysed by boiling the solution for 15 minutes. After boiling the hydrolysate was cooled and made up with H2O to a final volume of exactly 10 mL. The glucose was measured in this solution and found to have a concentration of 340 µg/mL (microgram/milliliter). i) Calculate the mass (mg) of glucose in the 10 mL of hydrolysate. As the 1 mL of glycogen sample was made up to a final volume of 10 mL, this mass of glucose was produced by the hydrolysis of the original 1 mL glycogen sample. ii) Calculate the amount (µmol) of glucose produced by the hydrolysis of the glycogen sample. iii) Calculate the purity of the glycogen used in the sample as % Purity = (moles of measured glucose/ moles of calculated glucose in glycogen) *100 iv) state your answer in a complete sentence. Show your working out such that the marker can easily understand it.…How would each of the following errors affect the determination of the molar mass of the unknown (Increase/Decrease/No effect)? a. Thermometer reads 2.0o higher than the true temperature. b. Some of the t-butanol was unknowingly spilled after it had been weighed but before the solute was added. 3. A student accidentally added acetylsalicylic acid (MW = 180.157 g/mol) rather than salicylic acid (MW = 138.121 g/mol), if no other mistakes were made, how would this error affect the determined molal freezing point depression constant for t-butyl alcohol (Kf)? 4. Based on the Tf and Kf you determined for t-butyl alcohol, predict the freezing point of a t-butyl alcohol solution containing 0.530 m NaCl. Assume 1.9 is the van’t Hoff factor for NaCl in t-butyl alcohol. Show your work.
- A 1 mL sample of glycogen was calculated to contain 35 µmol (micromole) glucose. To 1 mL of this sample was added 2 mL of 2 M HCL. It was then hydrolysed by boiling the solution for 15 minutes. After boiling the hydrolysate was cooled and made up with H2O to a final volume of exactly 10 mL. The glucose was measured in this solution and found to have a concentration of 570 µg/mL (microgram/milliliter). i) Calculate the mass (mg) of glucose in the 10 mL of hydrolysate. As the 1mL of glycogen sample was made up to a final volume of 10 mL, this mass of glucose was produced by the hydrolysis of the original 1 mL glycogen sample. ii) Calculate the amount (µmol) of glucose produced by the hydrolysis of the glycogen sample. iii) Calculate the purity of the glycogen used in the sample as % Purity = (moles of measured glucose/ moles of calculated glucose in glycogen) *100 iv) state your answer in a complete sentence.Method of separation/chemical reaction (with brief process) of raw materials of the assign drug below, please put a detailed explain Assign drug product is: Seignette salt (active ingredient) Raw materials: 1.5 kgs cream of tartar and 2.5 kg sodium carbonate monohydrate Actual yield: 1.20 kgs Seignette salt Formulation: 1.20 kgs Seignette salt Dosage Form: Syrup Packaging: 100 mL per bottleAcetaminophen or paracetamol, the active ingredient in many pain killers absorbs in the UV range with a λmax at 250 nm in neutral solutions (methanol usually). Its extinction coefficient is 14 mM-1cm-1. Each commercially available tablet (Tylenol, Panadol or Herron) contains 500 mg paracetamol. Its molecular weight is 151.1. Using this information, calculate the dilution required to analyse the concentration of paracetamol in a commercially available paracetamol tablet. Start by dissolving the tablet in 100 mL methanol. Show working out.
- To calculate the unknown concentration of a chemical in a solid sample, 4 different calibrationcurves were plot using 4 different methods. Which of the following method is considered asacceptable? a. Method 4, R? = 0.998b. Method 1, R2 = 0.650c. Method 2. R' = 0.890d. Method 3, R' = 0.169could you please explain theses datas and graph for the synthesis and spectrophotemetric analysis of aspirin and also I got 84.3% for my percent aspirin and 8.43% for my percent yield could you include that in the expiation too thank you!!Concentration of AR Stock Solution (ppmppm) 21.22 Unrounded Rounded Concentration of AR Stock Solution (μMμM) 42.7461 42.7