Exp #14: Titration 1) Standardization of NaOH with HCL. Molarity of HCI_I. DI 3 L. Volume HCI Used Volume HCI Used 25.00 Moles HCI Used M ml mol Initial Vol of NaOH_0.00 ml. Final Vol NaOH 21.5 ml Volume NaOH Used Molarity of NaOH Standard_{. 178 M Show Calculations for Molarity of NAOH: 2) Determination of Acetic Acid Concentration mly or Volume Vinegar Used 20.00 L 0.02000 L Molarity of NaOH_ 0.50 M Initial Vol of NaOH_ 0.60 mL Final Vol NaOH 35.45 mL Volume NaOH Used Moles NaOH Used mol Moles of CH,COOH mol Molarity of Vinegar M Chow Calculations for moles of NaOH and molarity of vinegar:

Exp #14: Titration 1) Standardization of NaOH with HCL. Molarity of HCI_I. DI 3 L. Volume HCI Used Volume HCI Used 25.00 Moles HCI Used M ml mol Initial Vol of NaOH_0.00 ml. Final Vol NaOH 21.5 ml Volume NaOH Used Molarity of NaOH Standard_{. 178 M Show Calculations for Molarity of NAOH: 2) Determination of Acetic Acid Concentration mly or Volume Vinegar Used 20.00 L 0.02000 L Molarity of NaOH_ 0.50 M Initial Vol of NaOH_ 0.60 mL Final Vol NaOH 35.45 mL Volume NaOH Used Moles NaOH Used mol Moles of CH,COOH mol Molarity of Vinegar M Chow Calculations for moles of NaOH and molarity of vinegar:

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 118CP: Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH,...

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In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 0.01 pH unit of each other? Explain.
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.)
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
Data Table: (include units!) Unknown Acid # Your NaOH concentration 0.10 Trial 1 Trial 2 Volume of Acid (in mL) 17ml 15ml Initial Buret reading for 15.00ml 0.00ml your NaOH Final Buret reading for 39.06ml 21.23ml your NaOH Total volume of NaOH 0.024L 0.021L used in titration
71tIN31Mrr15eZ41AWW-Ty2kfKY-gdiBaAX2wU/edit=slide%=Did gc31407e235 0_39 SS.. Typing Spanish Ac.. D Prese Is Add-ons Help Last edit was seconds ago 田 Background Layout- Theme Transition 1 2 3 I 4 5 6. 7 T 8 9. Drawing Conclusions How are 0.010 M solutions of HCI, CHOOH, and CH COOH similar to one another besides their concentration/molarity (M)? (Look at the ions present) 1. 2. How are they different besides what they are made up of? (Looks at the ions present)
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O Thank you - Zoom B Readin Question 8 of 10 Subr In a titration of 52.0 mL of a 0.350 M solution of a diprotic acid H,SO, with 0.600 M Ba(OH),, how many mL of base are required to reach the second equivalence point? mL 1 3 4 6. C 7 8 9. +/- x 100 G Search or type URL 5
. A 4.59 mL sample of HCl, specific gravity 1.3, required 50.5 mL of 0.9544N NaOH in a titration. Calculate the % w/w HCl.
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