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- Which of the following steps MUST be done prior to titration of an analyte? I. Prepare a standardized solution II. Wash the burette with a standardized solution III. Fill the burette to the 50-mL mark IV. Prepare a contrast paper to determine burette volume and titration endpointIn the case of over-titration, what should be done to the sample? Select one: a. Dilute the sample with water b. Discard and prepare another sample c. Add acid to revert the color back to faint pink or colorless d. Add more phenolphthalein indicatorChoose all options that will lead to an unsuccessful titration. a. Before filling the burette with the titrant, Chemist A used distilled water to rinse it. b. Chemist B used again the same flask for the second titration without cleaning it. c. Chemsit C chose to add 100mL of distilled water to the soda sample instead of 50 mL. d. Chemist D duplicated titration trials of the vinegar sample with an interval of 30 minutes.
- A person forgets to calibrate his burette before a titration experiment. This will cause his results to be: A. Accurate and imprecise B. Accurate and precise C. Inaccurate and precise D. Inaccurate and impreciseUsing table 3, answer the following questions. Concentration of HCl (M) 1.0M Volume HCl (mL) 5.01ml Concentration of NaOH (M) 1.0M Initial NaOH Volume (mL) 9.7mlml Final NaOH Volume (mL) 7.00 Total Volume of NaOH Used (mL) 2.7ml Moles of NaOH needed to neutralize 5.0 mL of 1.0M HCl (mol): Grams of HCl neutralized (g): NaOH volume difference between back titration and control (mL): Grams of HCl neutralized by NaOH volume difference (g):1. A student failed to carry out all of the procedural steps when doing the experiment. Would the following procedural variations result in an experimentally determined molarity of NaOH that is too high or too low? Briefly Explain. (a) The student didnt clean the buret before the beginning the titration. After completeing the titration, the student noticed that droplets of the titrant were clinging to the inside surface of the barel. (b) The buret tip was not completely filled with NaOH solution when the titration was begun. (c) The student forgot to add phenolphthalein indicator solution to the KHP solution before doing the titration
- What happens when a non-standard titrant is used in the titration of an unknown sample?a - The volume of the acid used will not be accurate.b - The normality of the acid used will not be accurate.c - The weight of the analyte will not be accurate.d - It will not matter.You have a solution of a standardized titrant of 0.01254 M and a sample that approximately has a molarity of 0.48 M. What dilution do you have to do to spend approximately 15 mL of titrant if you have 25 mL and 10 mL pipettes to take the diluted sample and value it?A 30.00 ml sample of carbonic acid is titrated to the endpoint with a 0.1000 M potassium hydroxide solution. The initial buret reading was 13.04 mL; the final reading was 56.61 mL. What is the molarity of the acid solution? 0.0759 0.0472 0.0726 0.283 0.0353
- Why you can't always use M1V1 = M2V2 in all titration problems?In titration, what solution is placed inside the burette? Group of answer choices stock solution analyte diluted solution titrantIn a titration experiment what would having a drop on the tip of the buret do for the accuracy of the end point? Is it a problem to have a drop on the end of your belt? Why or why not?