Identify each type of titration curve. Note that the analyte is stated first, followed by the titrant. Drag each graph to the appropriate bin. • View Available Hint(s) Reset Help 14 14 14 14 12- 12 12 12 10 10 10 10 4 4 2- 2 2 ml of titrant mL of titrant mL of titrant ml of titrant Strong acid-strong base Weak acid-strong base Weak base-strong acid Polyprotic acid-strong base Hd Hd Hd Hd

Identify each type of titration curve. Note that the analyte is stated first, followed by the titrant. Drag each graph to the appropriate bin. • View Available Hint(s) Reset Help 14 14 14 14 12- 12 12 12 10 10 10 10 4 4 2- 2 2 ml of titrant mL of titrant mL of titrant ml of titrant Strong acid-strong base Weak acid-strong base Weak base-strong acid Polyprotic acid-strong base Hd Hd Hd Hd

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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Over much of the titration curve, the pH lies within 1 pH unit of the pka. In this range, the change in pH with moles of base added is minimal. 13 12 11 10 9 8 7 6 TO 4 3 2 1 0 NH HCOOH NH3 pk of NH4 HCOO pk of HCOOH .5 25 .75 Moles base added per mole acid Titration curves of weak acids. 1.0 At the midpoint of the titration where half the acid is neutralized, pH=pKa Part A Calculate the pH of a 1.0 M NH4Cl solution. (Ką for NH4+ is 5.62 × 10-10) Express your answer to two decimal places. pH = Submit Part B pH = Submit VO ΑΣΦ Calculate the pH of the solution that results following addition of 10 mL of 1.0 M NaOH to 50 mL of 1.0 M NH₂ Cl. Express your answer to two decimal places. Part C Request Answer 5 ΑΣΦ ? Request Answer ? Calculate the pH of the solution that results following addition of 21 mL of 1.0 M NaOH to 50 mL of 1.0 M NH₂ Cl. Express your answer to two decimal places.
Can you help me find both equivalence points and pKa1 and pKa2 so I can label it on my graph?
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.
Please answer this question with steps thanks.
please see attached image. Im trying to calulate moles of HCl the volume I drew was 5.0 the volume titrated bas 8.15.
Titration of a weak acid Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. First what is the initial pH (before any NaOH is added)? The K₂ for HOCI is 3.0 x 10-8 M. Need help? Hint, given in general feedback. Answer: 3.96 How many mL of NaOH are added to reach the equivalence point? Answer: 8 What is the pH after 3.40 mL of NaOH are added? Hint given in general feedback. Answer:
can you help with question 4, thank you.
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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
What is the mmole of NaOH?
a) Compare between equivalence point and endpoint. Distinguish which point comes first. b) James performed an acid base titration experiment. A 25 mL sample containing HCl was transferred to Erlenmeyer flask using volumetric pipette. HCl sample was titrated against standardized 0.5010 M NaOH. An average titre volume of 24.35 mL was reported. Suggest a suitable pH indicator for James to be used in this experiment. Predict the initial concentration of the HCl. c) Alan and friends wish to sketch a weak acid strong base titration curve. Before they can do so, they need some data points. In a case where 50 mL of 0.20 M CH3COOH (Ka = 1.80 x 10-5 ) was titrated with 0.05 M NaOH, deduce the pH after addition of different volumes of NaOH. (i) 0 mL NAOH (ii) 100 mL NaOH (iii) 200 mL NaOH
Solve correctly please.