Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- 30.0 mL of the 1.0 M LIOH is added to 50.0 mL of 0.20 M H2SO4. What is the pH at this point in the titration? H₂SO4 + 2LIOH → Li₂SO4 + 2H₂O pH = [?] Hint: How many moles of H+ and OH- are present? pH at 30 mL base Enterarrow_forwardConsider the following infermation about sulfurous acid, a diprotic acid (11,S0,L LSO3=HSO, +1I* pK=1.81 HSO, S0,+H pK2-691 The titration curve for sodism sulfite, Na SO, with standard HCl is shown below PH VI V2 ml, HO added What are the major species present al point 3? O Noarrow_forwardPlease give me correct solution.arrow_forward
- @ Prepare a "pH curve" as follows: a) Find the pH of the acid solution just before the end point when 0.1 ml of base less than the end point voiume has been added. potnt, therefore at the end of the titration ph - 7. We are assuming that end point equals equivalence b) Repeat calculation 'a' for a volume 1 ml less and 5 ml less then end point and before any base is added. That is Oml base added.) Before end point, we assume that all the base is used up by the acid. c) Assuming you had continued the titration past the end point, calculate the pH when 0.1 ml of base beyond end point had been added. d) Repeat calculation 'c' for 1 ml, S ml and 10 ml of base beyond end point. Show all calculations and record your results in a table similar ta the one shown below: excess H+ excess OH 0 -5 -1 END PT -.1 +.1 +1 +5 +10 (ML) BASE VOLUME 20 24 24-9 25 25.1|26 30 35 pHarrow_forwardWrite the reaction that occurs and calculate the pH after... 15.0 mL of 0.100 M NaOH is added to 5.00 mL of 0.150 M HCl 25.0mLof0.10MNaOHisaddedto40.0mLof0.20MHF. (Ka 3.5x10-4) 80.0mLof0.10MNaOHisaddedto40.0mLof0.20MHF. (Ka 3.5x10-4)arrow_forward
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