The interaction between a basic analyte and the residual silanol groups of the stationary phase is minimized when the pH of the mobile phase used is equal to the pKa of silanol. True or False?
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The interaction between a basic analyte and the residual silanol groups of the stationary phase is minimized when the pH of the mobile phase used is equal to the pKa of silanol. True or False?
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- 25.0 cm3 of sodium hydroxide solution is tritrated against 0.2 mol dm–3 hydrochloric acid until the indicator just changes colour. 27.5 cm3 of the acid are required to reach the end point.Phenolphthalein is used as an indicator in the above experiment. What will be its colour change at the end point? From pink to yellow From pink to colourless From yellow to colourless From yellow to pink4. The molar absorptivities of the indicator weak acid HIn (K₁ = 1.42 x 105) and its conjugate base In at 570 were determined as ε(HIn) = 7120 and ɛ(In) = 961. The optical length b = 1.00 cm. (a) What is the absorbance of an unbuffered indicator solution having total indicator concentration 8.0 × 10%. (b) What is the absorbance of a buffered indicator solution having total indicator concentration 8.0 x 105 and pH = 6.5.A.) The value of Ka for hydrocyanic acid is 4.00×10-10.What is the value of Kb, for its conjugate base, CN-? B.) In the laboratory, a general chemistry student measured the pH of a 0.589 M aqueous solution of benzoic acid, C6H5COOH to be 2.199.Use the information she obtained to determine the Ka for this acid.Ka(experiment) =
- The standardization of same titrant during the determination of BOD5 of water sample was done separately for Day 1 and Day 5. Upon standardization, it turned out that the concentration of the titrant in Day 1 is higher than the concentration of the same batch of titrant in Day 5. How would you explain this discrepancy? (A) There were bubbles at the tip of the burette during titration. (B) Too much starch indicator was added in the conical flask. Sulfuric acid was added first before potassium iodide. (D) The water used to prepare the Na₂S₂O3 solution was not boiled resulting to proliferation of bacteria.What is the pH of a very dilute solution of a .5 x 10-7 M NaOH solution. Do not take into account Activity Coefficients1. Will a 5% preparation of caffeine citrate compounded in citrate buffer, pH 4.8 with no additional co-solvents be a solution – Yes or No? Explain. The MW of caffeine is 194.19 Da and that of caffeine citrate is 386.3 Da. The intrinsic solubility of caffeine is 2.17g/100 mL. please explain the answer.
- Show that the equivalence point N1V1=N2V2 where V1mL of analyte of strength N1 reacts with V2L of o titrant of strength N2?What would be the learning objective in an experiment of the determination of the Ksp of a slightly soluble compound?Calculate the pH of a buffer solution containing 10.0 cm3 of 0.100 mol dm–3 NaOH and 20.0 cm3 of 0.500 mol dm–3 ethanoic (acetic) acid made up to a total of 50.0 cm3 in a volumetric flask at 298 K. The pKa of ethanoic acid at 298 K is 4.77
- To perform a certain activity assay it is necessary to have 0.25 mL of an enzyme at a concentration of 0.2 mgmL-1 in the presence of 0.4 mM substrate and 200 mM NaCl in a suitable buffer. The stock solutions of enzyme, substrate and NaCl are 4 mgmL-1, 40 mM and 1 M, all in the same type of buffer. What volumes of the stock solutions and buffer are required for each assay?Sketch a plot of the fraction of species, f, vs pH for Tyr. Show your calculations for several points on the plot. You want to calculate the fraction of the species for more than 3 of the points. pKa’s for Tyr is 2.24, 9.04, and 10.10.Standard solution : 0.201 grams of acetylsalicylic acid was combined with 10 mL of 0.5 M NaOH, then transfered to a 100 mL flask and filled the rest of the way with water Then 0.500 mLs of the standard solution was transfered to a 10.00 mL flask and diluted to the 10 mL mark with 0.02 M of buffered iron chloride. Number of moles of NaOH = 0.005 moles Since the reaction between acetylsalicylic acid and NaOH is a 1:1 reaction, the number of moles of acetylsalicylic acid used in the reaction is also 0.005 moles. the concentration from analysis question 5: acetylsalicylic acid in the 100.00 mL volumetric flask is 0.050 M. From your plot, what is the value of εb? From the Beer- Lambert law For the aspirin sample, calculate the concentration of acetylsalicylic acid present using the value of εb that you found The concentration from analysis question 5 represents the concentration in the 10.00 mL sample that was prepared in the volumetric flask using an aliquot of the solution in the…