calculate the pH of the equivalence point N2OH soluhon Concentrahun.of n =0.lmol/L Mean titre (MOOH solution)= 18,95 mL Amount of NanH = 0.00199 moles Molar raho of Naot: aspirin=1:1 inn31:1 Aspirin= 0.0o189 moles Lintitration) Amount of 0.00189 Moles Mass of aspirin = 0,341 4 Mass /9 of Aspinin (per tablet) =0,34

calculate the pH of the equivalence point N2OH soluhon Concentrahun.of n =0.lmol/L Mean titre (MOOH solution)= 18,95 mL Amount of NanH = 0.00199 moles Molar raho of Naot: aspirin=1:1 inn31:1 Aspirin= 0.0o189 moles Lintitration) Amount of 0.00189 Moles Mass of aspirin = 0,341 4 Mass /9 of Aspinin (per tablet) =0,34

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What do you call the stage of the titration in which the number of moles of the titrant is stoichiometrically less than the number of moles of the analyte? (A post-equivalence (B pre-equivalence end stage (D equivalence
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 Enter
lonfiguration. How many milliteters (mL) of 1.0M NaOH would be needed to neutralize and precipitate 20.0L th B.0150 M Hs PO ?
The pH at 10, 100, and 110% titration (% of the equivalence point volume) for the titration of 50.0mL of 0.100 M HCI with 0.10OM NaOH at 10=1.09 , at 100= 11.00 O at 10=1.09 , at 100= 10.68 at 10=1.09 , at 100= 12.68
Consider 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 No
Qy A 50ml 0.1IM CeH:COOH( K= 10-)is diluted to 100 m! and titrated with 0.2 M KOH 1- Find the PH before any base is added 2- Find the PH when 15 ml of base has been added. 3. Find the PH at the equivalence point 4. Find the PH when 30 ml of base has been added 5- Draw the approximate titration curve, and discuss the feasibility of the titration.
Only first 3 parts please A ,B,C
Determine the pH change when 0.060 mol HI is added to 1.00Lof a buffer solution that is 0.417 Min HF and O.260 M in F. pH after addition - pH before addition pH change - Bub Anwer Ratry tie Grep mn p tempt remaling Determine the pH change when 0.090 mol NaOH is added to 1.00 L of a buffer solution that is 0.336 Min HCN and 0.224 M in CN. pH after addition - pH before addition - pH change Retry Entn Greup A mers grup attemat remaining Sumit Anwer
Please give me correct solution.
@ 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 pH
es) 1. Calculate the volume of the salt to be used in the preparation of 200 ml of the following buffer solutions. BUFFER DESIRED NUMBER pH 1 2 3 4 7.18 9.45 8.25 6.90 0.1M SOLUTIONS NaH2PO4/Na2HPO4 NH4CI/NH3 NH4CI/NH3 NaH2PO4/Na2HPO4 pka wwwwww 6.80 9.30 9.30 6.80 VOLUME OF ACID (ml) VOLUME OF SALT (ml)
What is the pH of the solution when Caitlin has added 30.00 mL of the 0.25 M LIOH to the 25.00 mL of 0.40 M formic acid? K₂ = 1.8 x 10-4 pH = [?] pH of Solution Enter