Lab Data You have not titrated to the endpoint Initial volume of buret (mL) Mass of KHP (g) Observations turned purple Final volume of buret (mL) Volume of NaOH (mL) Concentration of NaOH (M) 1.90 1.300 How to calculate sodium hydroxide concentration ESET -29 -30 -31 -32 -33 MY NOTES A LAB DATA SHOW LABELS 1 Turn on stir plate PHASE 6: Titration 2 Start titration by adding sodium hydroxide to Erlenmeyer flask 4 Complete the following steps: 3 Record your observations in Lab Data 5 6 Stop titration t endpoint. Record final buret volume and volume of NaOH in Lab Data Turn off stir plate Calculate molarity of NaOH solution. Record concentration in Lab Data

Lab Data You have not titrated to the endpoint Initial volume of buret (mL) Mass of KHP (g) Observations turned purple Final volume of buret (mL) Volume of NaOH (mL) Concentration of NaOH (M) 1.90 1.300 How to calculate sodium hydroxide concentration ESET -29 -30 -31 -32 -33 MY NOTES A LAB DATA SHOW LABELS 1 Turn on stir plate PHASE 6: Titration 2 Start titration by adding sodium hydroxide to Erlenmeyer flask 4 Complete the following steps: 3 Record your observations in Lab Data 5 6 Stop titration t endpoint. Record final buret volume and volume of NaOH in Lab Data Turn off stir plate Calculate molarity of NaOH solution. Record concentration in Lab Data

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 51P

See similar textbooks

Similar questions

Calculate the pH during the titration of 50.00 mL of 0.100 M Sr(OH)2 with 0.100 M HNO3 after 0, 50.00, 100.00, and 150.00 mL nitric acid have been added. Graph the titration curve and compare with the titration curve obtained in Exercise 16.22.
Consider a 10.0% (by mass) solution of hypochlorous acid. Assume the density of the solution to be 1.00 g/mL. A 30.0-mL sample of the solution is titrated with 0.419 M KOH. Calculate the pH of the solution (a) before titration. (b) halfway to the equivalence point. (c) at the equivalence point.
Consider the following acids and bases: HCO2H Ka = 1.8 104 HOBr Ka = 2.0 109 (C2H5)2NH Kb = 1.3 103 HONH2 Kb = 1.1 108 Choose substances from the following list that would be the best choice to prepare a pH = 9.0 buffer solution. a. HCO2H b. HOBr c. KHCO2 d. HONH3NO3 e. (C2H5)2NH f. (C2H5)2NH2Cl g. HONH2 h. NaOBr
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.
A 30.0-mL sample of 0.05 M HClO is titrated by a 0.0250 M KOH solution Ka for HClO is 3.5 108. Calculate a the pH when no base has been added; b the pH when 30.00 mL of the base has been added; c the pH at the equivalence point; d the pH when an additional 4.00 mL of the KOH solution has been added beyond the equivalence point.