38. (a) How many grams of NaOAc must be added to 300 ml 0.01 MHOAC to produce a buffer of pH 6.50?(b) 2.00 mM NAOH is added to the buffer above. What is the pH afterthe addition of the base?(c) What would happen to the buffer if 2.00 mM NAOH additional wereintroduced?Ans. (a) 14 g.; (b) 7; (c) pH becomes 11.53. 30. The base (CH2)3N has an ionization constant of 7 x 10-5. If 50 ml0.1 N (CH3)3N is titrated with 0.1 N HCl:(a) Find the pH before any acid is added.(b) Find the pH at the equivalence point.(c) Find the pH when the base is two-fifths neutralized.(d) Draw the approximate titration curve.(e) What indicator should be used?31. Repeat the calculations of problem 29 for the neutralization of 50 ml0.001 N HA by 0.001 N NaOH, assuming an initial volume of 200 ml.

38. (a) A buffer solution is a solution that resists the change in its pH on the addition of a small…

38. (a) How many grams of NaOAc must be added to 300 ml 0.01 M HOAC to produce a buffer of pH 6.50? (b) 2.00 mM NAOH is added to the buffer above. What is the pH after the addition of the base? (c) What would happen to the buffer if 2.00 mM NAOH additional were introduced? Ans. (a) 14 g.; (b) 7; (c) pH becomes 11.53.

38. (a) How many grams of NaOAc must be added to 300 ml 0.01 M HOAC to produce a buffer of pH 6.50? (b) 2.00 mM NAOH is added to the buffer above. What is the pH after the addition of the base? (c) What would happen to the buffer if 2.00 mM NAOH additional were introduced? Ans. (a) 14 g.; (b) 7; (c) pH becomes 11.53.

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...

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5:51 1 .ll LTE Search Question 16 of 20 Submit Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH, with 0.100 M HNO3 after 80.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. 1 2 4 Based on the result of the acid-base reaction, set up the unknown. ICE table in order to determine the H2NNH3*(at H2O(1) =H;O*(aq) H2NNH2(aq + Initial (M) Change (M) Equilibrium (M) RESET 0.100 0.200 0.0333 0.0667 +x -X 0.100 + x 0.100 - x 0.200 + x 0.200 - x 0.0333 + x 0.0333 - x 0.0667 + x 0.0667 - x www
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18) What is the pH of a 100ml solution formed by adding 0.1mole NaOH to a buffer solution that contains 0.25 mole HF and 0.15 mole NaF? (K, = 6.8 x 10* for HF)
10a.
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9a.
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