30. Acid HP and acid HQ are titrated with standardized NaOH, and their titration curves are shown in Fig.3. Both acids have the same concentration and solution volume initially. Based on these titration curves, answer the following questions. Titration of 40 mL 0.1MAcid 14 12 10 Part 1. Which of the above two acids does have a greater value of acid ionization constant K,? 8 6. Acid HP a) HP; b) HQ: c) same for both acids; d) cannot be judged Acid HQ 2 Part 2. The pK, of acid HP is most close to 10 20 30 40 50 60 70 20 a) 3.0 b) 5.0 c) 9.0 d) 9.5 e) insufficient information. mL 0.1M NaOH titrant Fig. 3 the concentration of the Part 3. The hydroxide ion concentration at the equivalence point (endpoint) of acid HP is hydroxide ion concentration at the equivalence point (endpoint) of acid HQ. a) less than b) equal to c) greater than d) none of the above

30. Acid HP and acid HQ are titrated with standardized NaOH, and their titration curves are shown in Fig.3. Both acids have the same concentration and solution volume initially. Based on these titration curves, answer the following questions. Titration of 40 mL 0.1MAcid 14 12 10 Part 1. Which of the above two acids does have a greater value of acid ionization constant K,? 8 6. Acid HP a) HP; b) HQ: c) same for both acids; d) cannot be judged Acid HQ 2 Part 2. The pK, of acid HP is most close to 10 20 30 40 50 60 70 20 a) 3.0 b) 5.0 c) 9.0 d) 9.5 e) insufficient information. mL 0.1M NaOH titrant Fig. 3 the concentration of the Part 3. The hydroxide ion concentration at the equivalence point (endpoint) of acid HP is hydroxide ion concentration at the equivalence point (endpoint) of acid HQ. a) less than b) equal to c) greater than d) none of the above

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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1. Label your graph "Strong Acid-Strong Base Titration." Create a line graph using the data below, which shows titration of 40.00 mL of 0.100M HCl with 0.100M NaOH. Once you have created the graph and connected the points with a smooth curve, use a colored pencil to label the equivalence point on your graph. Volume NaOH added (mL) 0.00 10.00 20.00 30.00 35.00 39.50 39.99 40.00 40.01 40.25 41.00 45.00 50.00 60.00 70,00 80.00 PH 1 1.22 1.48 1.85 1.85 3.20 4.90 7.00 9.40 10.50 11.09 11.76 12.05 12.30 12.43 12.52
a) In a NaOH and HCl titration lab: Suppose you add 40 ml of water instead of the 45 mL. How will this affect the calculations for the molarity of the HCI? (In this case, the molarity of HCl turned out to be 0.559 mol/L). While being specific. Explain why it will not matter or it will make the molarity high or it will make the molarity low. b) if you disregard the instructions to titrate until a persistent blue endpoint is reached and instead conclude the titration at the initial appearance of blue, describe the impact on the reported molarity of the CoC12 solution. Provide specific details and specify whether the reported molarity will be higher, lower, or remain unaffected.
7. The pH titration curve of a weak acid, HA, is shown me below. As the titration progresses, HA is converted into its conjugate base, A-. 12 10 8 (a) What is the volume of NaOH at the equivalence point? 2 25 30 35 15 20 volume of NaOH added (mL) 5 10 (b) At what volume (or volumes) is all of the acid present in the protonated (HA) form? (c) At what volume (or volumes) is all of the acid present in the conjugate base (A') form? (d) At what point along the titration will half the original amount of HA have been converted to A-?
Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 100.0 mL of the strong acid has been added. The value of Kb for H,NNH, is 3.0 × 10-6. ( PREV 1 Based on the result of the acid-base reaction, determine the pH of the solution. pH RESET 6.21 7.79 11.3 2.70 1.85 1.70 3.91 10.1 12.3 3.70 17.7
Match each term with its definition or description. 0000000 The point in a titration when the added amount of standard reagent is equal to the amount of analyte being titrated. A volumetric analysis technique used to determine the unknown concentration of a solution by using the known concentration of another. A solution of unknown concentration. The standard reagent of known concentration that is added from a buret to the analyte solution. A common concentration unit - moles per liter. The point in a titration when a change in the analyte solution is observed, indicating equivalency. It is added to the analyte solution and aids in the observation of the completion of the reaction. molarity equivalence point Answer Bank end point titration titrant analyte indicator
Which plot accurately represents the titration between 50.0 mL unknown HNO2 concentration and 0.15 M NaOH? А. В. Base (mL) Base (mL) C. D. Base (mL) Base (mL) Graph A Graph B Graph D Graph C Hd
4. A student titrates 20.0 ml of an acid solution with 0.500 M NaOH and gets the graph shown below. Determine the concentration of the acid. 2 14.0 13.0 12.0 1.0 5.0 3.0 2.0 00 Titration: pH vs. Volume of Strong Base 2.0 SO Volume of Base Added (ml) 8.0 5. From the graph given in the previous question, determine the pKa of the acid used in the titration. Which of the following acids (hypobromous-HBrO, Formic-HCHO2, Hypochlorus-HCIO, or Periodic-HIO4, or Hydroiodic-HI) is the acid used? Explain how you know. 1.0.0 703
Titration Curve Using the table of indicators identify which of the given 13 12 indicators would be appropriate for the titration 11 10 represented in the titration curve. 9 thymol blue 8 pH 7 6 alizarin yellow R 5 O quinaldine red 4 3 O clayton yellow 2 1 metacresol purple 4 6 8 10 12 14 16 18 20 Volume of Titrant (mL) O methyl green 2.
A 50.0-ml sample of 0.20 M hydrochloric acid (HCI) is titrated with 0.5 M LIOH. Determine the pH of the solution after the following volumes of LIOH titrant are added. Express your answers to two decimal places. a) pH after 10 mL of LIOH added: b) pH after 20 mL of LIOH added: c) pH after 30 mL of LIOH added: Check
Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 10.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. 1 2 4 NEXT Use the table below to determine the moles of reactant and product after the reaction of the acid and base. H2NNH2(aq) H*(aq) H2NNH;*(aq) + Before (mol) Change (mol) After (mol) 5 RESET 0.200 0.100 +x 0.200 + x 0.200 - x -x 0.100 + x 0.100 - x 1.00 x 103 -1.00 x 10-3 2.00 x 10-3 -2.00 x 10-3 6.00 x 103 -6.00 x 10-3 7.00 x 10-3 -7.00 x 103 8.00 x 103 -8.00 x 103
7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?
5 6 7 8 Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The K, of hypobromous acid is 2.8 x 10¹⁹. A 30.00 mL solution of 0.300 M hypobromous acid (HBrO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LiOH). What is the initial solution pH (i.e., when 0.00 mL of titrant have been added)? (Two decimal places) Type your answer... Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The K, of hypobromous acid is 2.8 x 10¹⁹. A 30.00 mL solution of 0.300 M hypobromous acid (HBrO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LiOH). What volume (in mL) of titrant will have been added at the half-equivalence point? (One decimal place) Type your answer... Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The K₂ of hypobromous acid is 2.8 x 10.⁹. A 30.00 mL solution of 0.300 M hypobromous acid (HBrO) is being titrated with a solution that is 0.600 M in lithium hydroxide…