08 %24 2. 10 Hd 3 The following plot shows a titration curve for the titration of 1.00 L of 1.00M diprotic acid H 2A with NaOH. 12 9. a. 0. 0. 2.50 00 Moles of OH added 0.50 Which point a-d represents the first equivalence point? point a point b point c point d Click Save and Submit to save and submit. Click- Save All Answers to save all answers. MacBook Air DD 000 F4 F5 F2 F3 %23 #3 L 4.

08 %24 2. 10 Hd 3 The following plot shows a titration curve for the titration of 1.00 L of 1.00M diprotic acid H 2A with NaOH. 12 9. a. 0. 0. 2.50 00 Moles of OH added 0.50 Which point a-d represents the first equivalence point? point a point b point c point d Click Save and Submit to save and submit. Click- Save All Answers to save all answers. MacBook Air DD 000 F4 F5 F2 F3 %23 #3 L 4.

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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Q7
2. For each titration, predict whether the equivalence point is less than, equal to, or greater than pH = 7. (Circle) a) Pyridine (CSH5N) titrated with nitric acid b) Acetic acid titrated with calcium hydroxide pH 7 > pH 7 > pH 7 = pH 7 = pH 7 c) Hydrobromic acid titrated with strontium hydroxide = pH 7 3. Calculate the pH at 25°C of a solution that results from mixing equal volumes of a 0.050 M solution of ammonia and a 0.025 M solution of hydrochloric acid? pKa(NH4*) is 9.25.
can someone determine the equivalence points of these graphs and explain how you got those values? thank you
Need help with the Pre lab calculations
Not Secure - gmc.mrooms3.net English - United States (en_us) When titrating acetic acid with sodium hydroxide at 25°C, the Select one: O a. pH will be less than 7 at the equivalence point. O b. pH will be equal to 7 at the equivalence point. O c. pH will be greater than 7 at the equivalence point. O d. titration will require more moles of base than acid to reach the equivalence point. O e. titration will require more moles of acid than base to reach the equivalence point.
The following titration data was collected by a students in CH1031. Based on the results, determine the concentration of the aqueous hydrochloric acid. Concentration of NaOH used: 0.25 M Volume of NaOH used: 25.0 mL Indicator: phenolphthalein Colorless to pale pink Endpoint color change: Table 1 Volume of hydrochloric acid Required Burette reading (mL) Trial 1 Trial 2 Trial 3 29.28 1.78 Final reading Initial reading Volume HCI used (mL) 36.62 43.98 9.28 16.62
Describe the shape of the titration curve shown, describe why it has this shape.
Titration Curves: Weak acid with strong base 14.0 The equivalence-point pH is NOT 7.00 here. Why not?? Excess base results in high pH 12.0 Equivalence point 10.0 Cole „nange piienolphthalein Bromphenol blue was ok for the strong acid/strong base titration, but it changes color far too early 8.0 6.0 pH = pka to be useful here. 4.0 Color change | bromphenol blue Excess acid results in low pH 2.0 0.0 0.0 5.0 10.0 15.0 20.0 25.0 30.0 Volume of 0.500 M NaOH, mL CH;COOH + NaOH → Na CH,CO0 + H,0 Hd
A 24.7 mL sample of 0.345 M formic acid (HCHO₂) is titrated with 0.345 M NaOH. Calculate the pH after the addition of 24.7 mL of NaOH. (For HCHO2; Ka = 1.76 × 10-4) Hint: Determine the equivalence point so you know where you are in the titration. Report your answer with 2 places past the decimal point. २
Ee.82.
If an unknown organic acid is titrated with 0.200 M NaOH and it takes 34.50 mL to reach the equivalence point. Show how to calculate the # moles of H3O+at the equivalence point? Answer: Moles of H30+= 0.0069 moles Suppose 0.345g of an unknown acid (with one ionizable H+ion) is titrated using the information in question above. Show how to calculate the Equivalent Mass of this acid.