After preparing 500 mL of 0.1019 M NaOH solution, the cap is left open and it absorbs 0.652 g CO2. With this solution, Calculate the relative carbonate error in acetic acid titration besides the phenol phthalate indicator.
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Q: Calculate the relative carbonate error made in acetic acid titration
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After preparing 500 mL of 0.1019 M NaOH solution, the cap is left open and it absorbs 0.652 g CO2. With this solution, Calculate the relative carbonate error in acetic acid titration besides the phenol phthalate indicator.
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- Write two features of Erichrome black- T which makes it a suitable indicator in complexometric titration. In which medium does it undergo complex formation?In which cases are the wet Electorstatic Precipitators used?What is the importance of having a titration of about pH 10 in compleximetric 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?Discuss the theory behind potentiometric pH determinations. Then compare the advantages and disadvantages of potentiometric titration with classical indicator-based titration.500 mL of 0.1019 M NaOH solution is preparedIt is immediately forgotten with the cap open and absorbs 0, 652 g of CO2. Calculate the relative carbonate error made in acetic acid titration with this solution with phenol-phthalate indicator.
- Titration of 0.1 M HCl against a 25mL liquor mixture of NaOH and Na2CO3 using phenolphthalein indicator requires 17.5mL of the acid for the endpoint. After this, methyl orange was added and 3.5mL of HCl was again required for the next endpoint. A. Write separate equations for reactions for the two endpoints B. Calculate the amount in milligrams of NaOH and Na2CO3 in the mixtureAn indicator with an acid dissociation constant of 2.19 x 10‑5 could typically be used for a solution with pH 3.66 True or False?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.
- What would be an appropriate indicator to use to measure the endpoint volume for a titration with a pH of 4.32 at the equivalence point?A 25.0-mL volume of 0.040 0 M phosphoric acid was titrated with 0.050 0 M tetramethylammonium hydroxide. Write the series of titration reactions and find the pH at the following volumes of added base: Vb 0, 10.0, 20.0, 30.0, 40.0, and 42.0 mL. Sketch the titration curve and predict what the shape will be beyond 42.0 mL.In the titration of 50.00mL of 0.2980M HCl, 71.93mL of 0.2173M NaOH was required to reach the phenolphthalien endpoint. Calculate the percent error between the predicted amount and the experimental amount