pH 12.0 10.0 8.0 6.0 4.0 2.0 10.0 Volume of 0.100 M NaOH, mL 5. If 20.0 mL of 0.100 M titrant in the graph above were required to reach the s equivalence point, how many moles of the acid were originally present? 5.0 (a) 0.00100 (b) 0.0100 (c) 0.00200 (d) 0.00050 15.0 20.0 25.0 30.0
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- 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 X3Part A: Standardization of a Sodium Hydroxide Solution Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH Molarity of NaOH Average Molarity of NaOH: _______________While preparing the samples for analysis, you forgot that you already added phenolphthalein indicator so you added some more. What will be its effect in the volume of the titrant needed to reach the endpoint? Select one: A. Increase B. Decrease C. No effect D. Cannot be determined Primary standards are used to determine the exact concentration of the titrant. Based on the criteria of primary standards, which of the following cannot be used as a primary standard? Select one: A.Oxalic acid B. Sodium hydroxide C. Sodium carbonate D. Potassium dichromate During titration, you notice that the retention of the faint pink color is longer than earlier. Your lab partner suggested that you add a “half-drop” to prevent over-titration of the analyte solution. Is it ethical to do the “half-drop” technique? Select one: A. NO. It will cause error in calculations if you forgot to record the volume reading before adding the half-drop. B. YES. No error in calculations will be encountered provided…
- Anachem Titration curved Calculate the pH of the solution for every 0.1 ml of the titrant (from 0 mL to 30 mL) and generate a titration curve using Excel. Highlight each stage in the titration and the equivalence point and obtain the first derivative of the curve (that is ΔpH / Δvolume). 1. A 25 mL solution of 0.2521 M HCl was titrated with 0.3133 M NaOH 2. A 25 mL solution of 0.4153 M NaOH was titrated with 0.5191 M HNO3 3. A 10 mL solution of 0.0543 M formic acid was titrated with 0.0332 M KOHLimestone consists mainly of the mineral calcite, CaCO3. The carbonate content of a 0.5972 g sample of powdered limestone was measured by suspending the powder in water, adding 25.00 mL of 0.508 molar hydrochloric acid, and heating to dissolve the solid and dispel carbon dioxide gas. The excess acid required 36.29 mL of 0.1064 molar sodium hydroxide for complete titration to a phenolphthalein end point. What is the weight percent of calcite in the limestone?a student was titrating a solutin of acitic acid with a sodium hydroxid solution. determin the ph at the equivilance point. do this by constructing a bca table, constructing and ice table, writing the equlibrium constant expresion and find the ph. the ka for ch3cooh is 1.8e-5. a 50ml solutin of 0.3 m of ch3cooh was titrated with 0.3 m of naoh.
- The data below is titration of Na2CO3 with HCl which is a diprotic titration curve. From the endpoint determinations, calculate the concentration of the carbonate solution if the [HCl] was 0.1036 M. use 10.00 mL of carbonate solution for the calculations PH Burett vol added 11.30 0.00 0.00 10.80 0.98 0.98 10.51 1.95 0.97 10.28 3.00 2.02 10.10 3.99 3.01 9.92 4.99 4.01 9.74 5.95 4.97 9.54 6.97 5.99 9.28 7.95 6.97 8.86 8.97 7.99 8.70 9.18 8.2 8.52 9.35 8.37 8.39 9.49 8.51 8.26 9.60 8.62 8.09 9.71 8.73 7.97 9.82 8.84 7.90 9.90 8.92 7.93 10.21 9.23 7.87 10.32 9.34 7.84 10.42 9.44 7.75 10.53 9.55 7.65 10.63 9.65 7.57 10.75 9.77 7.53 10.85 9.87 7.49 10.96 9.98 7.05 11.95 10.97 6.76 12.99 12.01 6.56 13.98 13 6.39 14.93 13.95 6.24 15.98 15 6.07 16.98 16 6.21 17.05 16.07 6.24 17.15 16.17 6.25 17.25 16.27 6.30 17.32 16.34 6.37 17.40 16.42 6.41 17.50 16.52 6.46 17.58 16.6 6.47 17.63 16.65 6.45 17.72 16.74 6.44…Molarity of titrant (NaOH): 0.4550 M HC2H3O2 (aq) + NaOH (aq) → NaC2H3O2 (aq) + H2O (l) Trial # First Second Third Fourth Initial buret reading 0.15 mL 2.43 mL 1.32 mL 0.58 mL Final buret reading 18.62 mL 20.87 mL 20.03 mL 19.14 mL Volume of titrant used 18.47 mL 18.44 mL 18.71 mL 18.56 mL 4) Calculate the molarity of the acetic acid in the vinegar solution (Show your work). use FW for moles-->grams acetic acid. Molarity acetic acid = _____________ M 5) Calculate the weight % of acetic acid in the vinegar. How does this compare with the % listed on the label (5.00%)? (For this calculation assume that density of vinegar is 1.03 g/mL and of course, show your work). Weight % = ___________ 6) If you didn’t get the same weight % of acetic acid as listed on the vinegar label (5.00 %), what are two things (be specific) that could’ve happened during the experiment that could explain the variation from the expected weight %? To do…Titration of 10.00 mL of a 0.444M solution of HCI with a solution of LiSH required 23.2 mL of the LiSH solution to reach the end point. What is the molar concentration of LiSH? HCL + LiSH -> LiCI+H2S a. 0.191M b. 0.223 C. 0.546 d. 0.229
- Titration of (4.890x10^-1) grams of monoprotic weak acid (dissolved in KCl) required (2.44000x10^1) mL of (2.12000x10^-1) molar NaOH solution to reach equivalence. Based on this information, how many moles of weak acid are present in this solution? Format your answer with correct number of sig figs. Use scientific notation.An automatic titration of Cola product was analyzed and the following results were produced: Volume of Standardized NaOH Titrant used to achieve the first equivalence point in titration: Trial #1: 1.300 mL Trial #2: 1.137 mL Trial #3: 1.140 mL May you explain why trial #1 was skewed; for example, if pipetting of the 25.00 mL was done incorrectly, how would the molarity change if the volume examined was supposed to be 24.50 mL?The potentiometric titration data of 2,422 mmol chloride ion with 0.1000 M AgNO3 are as follows. What should the x and y axis values be to find the turning point using the first derivative?