In this experiment, you will use phenolphthalein as an indicator. Why is it important to match the endpoint of a pH indicator to the equivalence point of the titration?
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- Why phenolphthalein is not a suitable indicator in the titration of a strong acid with a weak base?Could phenolphthalein be used as an indicator in the Kjeldahl titration?Assess the suitability of methyl orange to signal the equivalence point in weak acid and strong base of the experiment. Use the pH range over which the methyl orange changed colors to make this determination. If you conclude that methyl orange would not reliably indicate the equivalence point in this reaction, then suggest an alternative indicator which would be more appropriate.
- If water was used to rinse the conical flask used for the titration, how would this affect your final estimate of hydrochloric acid concentration? (More, less or unchanged?) Explain why, discussing the number of moles that you would actually have due to the rinsingList the observations of a manual titration experiment and explain your expectations. This should include color change and when the equivalence point (endpoint) might be reached. When do you stop and why.What factor affects the ‘strength’ of a buffer? Why was benzoic acid used as a solvent when making up the glucose stock standard solution?
- In the titration between potassium iodate and the sodium thiosulfate solution, if the titration is not performed immediately after the addition of the sulfuric acid, how would this likely affect the calculated concentration of your diluted sodium thiosulfate solution?How would the titration curves differ if the volume of the acid used was halved?Explain why the indicator cresol red changes color when the pH is lowered from 10 to 6. What colors will be observed at pH 10, 8, and 6? Why does the color transition require ,2 pH units for completion?
- What is the purpose of heating a sample prior to analysis (regarding potentiometric titration).What does a permanent faint pink color in the solution indicate in the Acid-Base Titration?Why do we use a solid acid as a primary standard? During the standardization of NaOH, Shane didn’t notice that there was an air bubble in the tip of the buret when they started their rough titration. The bubble went away during the rough titration and Shane continued with two fine titrations. Does this affect the calculated concentrations of NaOH? Why or why not?