Draw and label a complete laboratory set-up of acid-base titration using phenolphthalein as the indicator, using HCl as the analyte/sample, and using NaOH as the standard solution. Cite complete source/(s) if picture will be copied from the internet.
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- Using the table of pH indicators and their respective pKin. Match the best-suited indicator for the following titration scenarios. Note: You do not need to calculate the pH at the equivalence point, an estimation will be sufficient for this question. Indicator Pkin Thymol Blue 1.65 Methyl Red 5.00 Bromothymol 7.30 Blue Phenolphthalein 8.70 0.10 M acetic acid (pKa = 4.74) is titrated with 0.08 M NaOH [ Choose ] 0.10 M HCI is titrated with 0.0993 M NaOH [ Choose ] 0.10 M ammonia (pKb = 4.74) is titrated with 0.12 M HCI [ Choose ]Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH3CH₂CH₂COOH (K₁-1.54 x 10-5), with 0.1000 M NaOH solution after the following additions of titrant. (a) 15.00 mL: pH = (b) 20.60 mL: pH = (c) 26.00 mL: pH = GuiBy applying Gravimetry, Titration (Chemical indicator) and Potentiometry lessons which technique should be used in following situations. Explain your answer. In your explanation, state what is the advantage of the technique you chose over other technique and /or the barrier/difficulty of using the technique. Your choice should not be dependent on cost. Answer in less than 7 sentences. For chem students - Total Acid content per tablet of a newly developed drug that has yellow coating Target level is 1%.
- The following results were obtained in the titration of an unknown monoprotic acid (Use data from table). Students identified the acid as benzoic. Copy VNaOH (no first raw), then pH(all values) into your Lab Report template. Use the data you obtained to fill in the table below. Concentration of NaOH used, M 1.164 x 10-1 Mass of unknown aid used, g 0.3840 1) Find: a) Equivalence point, mL. b) Half equivalence point, mL. c) pKa d) Ka e) pKa from literature f) Percent Error g) Number of moles of NaOH, mol. h) Number of moles of acid titrated, mol. i) Molar mass of acid g/mol. j) Molar mass of acid, g/mol from the literature k) Percent errorConsider the following indicators: dinitrophenol (pKIn = 3.5), bromothymol blue (pKIn = 7), thymolphthalein (pKIn = 10). Match each titration below with its most-likely best indicator. (A specific indicator choice may be used more than once.) Group of answer choices titration of HF with NaOH [ Choose ] dinitrophenol bromothymol blue thymolphthalein titration of RbOH with HNO3 [ Choose ] dinitrophenol bromothymol blue thymolphthalein titration of HI with KOH [ Choose ] dinitrophenol bromothymol blue thymolphthalein titration of NH3 with HBr [ Choose ] dinitrophenol bromothymol blue thymolphthaleinQuestions 11-14 refer to the same strong base/strong acid (SB/SA) titration. A 15.00 mL solution of 0.100 M sodium hydroxide (NaOH) is being titrated with 0.250 M hydrobromic acid (HBr). What is the total solution volume (in mL) at the equivalence point? (Nearest whole number) Type your answer...
- Three-point calibration was not performed on the pH meter prior to titration. Is there a positive error, negative error, no effect, or error could not be determined In terms of the Computed pKa of the unknown weak acid?Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided TOPIC: Standardization of Titrant Question 7 Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX __ ET TOPIC: Determination of Molar Concentration of each component (Double Indicator Titration) Question 8 No blank correction Ex ___ ET Question 9 Bubbles trapped in the tip of burette: EX ___ ET Question 10 Measuring the sample volume using a volumetric pipet while looking downwards at the meniscus: EX ___ ETThank you! Data included in picture! No hand drawn graphs!! Determine the equivalence point of sudsy ammonia/citric acid reaction by graphing the titration data (pH vs volume citric acid) from Table 1: No Indicator Data Table. Draw a green arrow (use ‘Insert Shape’ feature to do this once you have copied your graph from Excel) on your graph indicating the data point that represents your equivalence point. Use a graphing software to create the x-y scatter plot showing the pH of the experimental solution as a function of the volume of citric acid (the titrant) added for the titration in Part 4. On your graph, the x-axis should be the volume of citric acid added (mL), and the y-axis should be the pH of the experimental solution at that volume. Do NOT connect your points; no trend line needed and make sure to: · Label the axes including the units in parentheses. · Include a figure legend (text below the graph) explaining the data in your graph that includes the arrow…
- During titration the following data were collected. A 25 mL poretion of an unknown acid soluation was titrated with 1.0 M NaOH. It required 65mL of the base to neutalize the sample. How many moles of acid are present in 3.0 liters of this unknown solution?I did an experiment called Potentiometric Analyses where we titrate NaOH with a solid unknown weak acid. Our group was told that our weak acid is diprotic. Mass of dry, solid acid = .155g Molar concentration of NaOH (mol/L)= 0.100 Buret reading of NaOH, initial (mL)= 50 mL Buret reading NaOH at stocichiometric point, final (mL)= 22.1 mL Volume of NaOH dispensed (mL) 27.9 mL Moles of NaOH to stoichiometric point (mol) : _____________ (I think the above answer would be 2.79 x 10-2? if yes then skip) Moles of acid (mol) _____________ Molar mass of acid (g/mol) __________ Note: In the book it says for a diprotic acid, 2 mol of OH-, neutralizes one mole of acid.Mr. Clean recently bought a laboratory-grade sodium carbonate from a chemical company known as Brand X. He was supposed to use it in the production of detergents. Unfortunately, he was scammed by the company. He suspected that he purchased a crude so- dium carbonate so he tasked the Quality Assurance Department to determine the components of the purchased chemical. The chem- ist assigned to analyze the sample used double indicator method. For the standardization of HCI titrant, 0.1025 g Na2CO3 of 99.5% purity (FW: 106.00) required 8.20 mL of the titrant to reach the phe- nolphthalein endpoint. FW: NaOH (40.00), NaHCO3 (84.01), Na2CO3 (106.00) a. What is the molarity of the titrant? (use significant figures) The chemist obtained a 3.150 g sample and dissolved it in distilled water to produce a 50.0 mL solution. An aliquot of 10.00 mL was obtained and diluted in a 100.0 mL volumetric flask. A 50.00-mL aliquot of the diluted sample was taken and it required 25.70 mL of titrant for the…