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write a lab report with reference on salicylic acid titration (1500 words)
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- Thank 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…how we can implement acid base titration in pharmaceutical industries?Match each term with its definition or description. 0000000 The point in a titration when the added amount of standard reagent is equal to the amount of analyte being titrated. A volumetric analysis technique used to determine the unknown concentration of a solution by using the known concentration of another. A solution of unknown concentration. The standard reagent of known concentration that is added from a buret to the analyte solution. A common concentration unit - moles per liter. The point in a titration when a change in the analyte solution is observed, indicating equivalency. It is added to the analyte solution and aids in the observation of the completion of the reaction. molarity equivalence point Answer Bank end point titration titrant analyte indicator
- Suppose a student performed a similar standardization titration experiment. Below is the calculated concentration of NaOH from each of their titrations. Titration #1 Titration #2 Titration #3 Concentration of NaOH (M) 0.9554 0.9540 0.9551 Using the 3 concentrations, calculate the average concentration of the student's NaOH solution and calculate the ± error in parts per thousand (ppt). Show the complete calculation. Express your final answer in the form of average (with units) ± error in ppt. use the right significant figuresSuppose a student performed a similar standardization titration experiment. Below is the calculated concentration of NaOH from each of their titrations. Titration #1 Titration #2 Titration #3 The concentration of NaOH (M) 0.9554 0.9540 0.9551 Using the 3 concentrations, calculate the average concentration of the student's NaOH solution and calculate the ± error in parts per thousand (ppt). Show the complete calculation. Express your final answer in the form of average (with units) ± error in ppt.Shown below is data from a titration experiment that was performed using HCI, CH3 COOH and C6 H8O7 and H2SO4 of unknown concentration. Different dilutions of H2SO4 were made prior to the titration experiment: a 1:2 dilution, a 1:5 dilution and a 1:10 dilution. Table 1. Titration Data HCI Acetic Acid Citric Acid 1:2 1:5 1:10 monoprotic. triprotic diprotic diprotic diprotie pH of diluted acid solution Volume of acid titrated (mL) 1 0. 20 20 20 30 0.65 5.20 30 5.20 10.05 30 0.55 15.15 1.75 6.65 0.10 2.45 4.95 Initial volume of NaOH (mL) Final volume of NaOH (mL) 12.2 Volume NaOH (mL) Amount of 0.20M NAOH added (mmol) Amount of acid (mmol) Concentration of acid titrated (M) Concentration of acid before dilution (M)* 2. 3.
- Part A What is the pH of a buffer system that contains 0.170 M hydrocyanic acid (HCN) and 0.100 M sodium cyanide (NaCN)? The pKa of hydrocyanic acid is 9.31. Express your answer using two decimal places. pH = %3D Submit Request Answer < Return to Assignment Provide Feedback Previous MacBook Air DII DD F4 F5 F6 F7 F8 F9 F10 F11 & 4 6. 7 11 * CO %24Chemistry write introduction Experiment Acid-Base Titration Using a pH Meter and Phenolphthalein Strong acid vs Strong base should state the purpose of the investigation and must include appropriate citations of relevant, precedent work but should not include an extensive review of marginally related literature. If the manuscript describes a new method, indicate why it is preferable to older methods. If the manuscript describes an improved analysis of a substance, the competing methods must be referenced and compared. use Hydrochloric acidC. Titration of acid by a base Standardization of NaOH Volume of NaOH Mass of KHP Initial buret Final buret Trial used Molarity of NaOH (g) reading (mL) reading (mL) (mL) (1) (2) (3) (4) (5) 1.2075 0.7 25 24.3 0.243 (6) (7) (8) (9) (10) 1.2062 16.4 40.9 24.49 0.2412
- Phenolphthalein is an indicator which turns a pink color at a pH of 8.3. In this experiment, phenolphthalein is added to the antacid solution to indicate the equivalence point of the back titration. Phenolphthalein solution by itself is weakly acidic. If instead of adding one drop, a student adds several milliliters of the phenolphthalein solution, will this cause the student to under-estimate or over-estimate the neutralizing power of the antacid? Explain your answer.if the bubble in the tip of the buret is not removed prior to performing HCl titration will the reported concentration of the HCl be greater than, less than, or equal to the true concentration of the HCl if the bubble is pushed from the buret during the titration? (in respect to volumetric analysis)1. At what point (how many milliters of added acid) was the solution in beaker “B” neutralized? Neutralization of Acids and Bases Test Data: Table 2: Initial pH Test Results Container Substance in Container pH using the pH meter A distilled water 6.8 B 0.5 g sodium bicarbonate with distilled water 7.5 C vinegar 2.3 Table 3: Neutralization Amount of Acid Added (mL) pH using the pH Meter 1 mL 7.5 2 mL 7.3 3 mL 7.2 4 mL 7.2 5 mL 7.2
