**Exercise:** Construct a titration curve by plotting \(pH\) vs. \(V_{\text{NaOH}}\) added.**Reaction:** \[\text{HCl}_{(aq)} + \text{NaOH}_{(aq)} \rightarrow \text{H}_2\text{O}_{(l)} + \text{NaCl}_{(aq)}\]---**Observations:**- **Volume of NaOH added (mL):** \(0.00, 5.00, 10.00, 15.00, 20.00, 25.00, 30.00, 35.00, 40.00, 45.00, 50.00\)- **[H⁺] Concentration:** Varies with each addition, starts at \(1 \times 10^{-1}\) M- **pH Values:** \(1.00, \ldots, \text{calculated}\)---**Diagram Description:**There is an illustration of a titration setup with:- A **buret** containing the titrant, \(0.1 \, \text{M NaOH}\).- A **flask** which holds the analyte, \(0.1 \, \text{M HCl}\), \(50 \, \text{mL}\).---**Hints:**The pH of the solution is calculated using:**(a) Initial Conditions:**- \(V_{\text{NaOH}} = 0\), \([\text{H}^+]\) = [HCl]**(b) After Initial Addition of NaOH (Before Equivalence Point):**\[ [\text{H}^+] = \frac{M \cdot V_{\text{HCl}} - M \cdot V_{\text{NaOH}}}{V_{\text{total}}} \]**At Equivalence Point (\(V_{\text{NaOH}} = 50 \, \text{mL}\)):**- All HCl is consumed, acidity from auto-ionization of water: \([\text{H}^+] = 1 \times 10^{-7}\)**(d) After Equivalence Point:**\[ [\text{H}^+] = \frac{1 \times 10^{-14}}{M \cdot V_{\text

The initial concentration of HCl = 0.1 M The initial concentration of NaOH = 0.1 M The initial…

Exercise Construct a titration curve by plotting pH vs. VNaOH added. HCl(aq) + NaOH(aq) H₂O(1) + NaCl(aq) Volume NaOH (mL) [H] pH 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 40.00 45.00 48.00 50.00 52.00 55.00 60.00 65.00 70.00 75.00 80.00 95 00 1×10-² Hints: The pH of the solution is calculated using the following equations: (a) Initial conditions (VNaOH = 0), [H'] = [HCI] (b) After initial addition of NaOH and before the end point: MVC-M NOVNO V LV (e) At the end point (Vsaou 50 mL), all the HC1 is being consumed and the acidi of the solution comes from auto ionization of water which is: [H]=1*10 (d) After the end point: [H"]= 1x10-¹4 M XV W V. +K

Exercise Construct a titration curve by plotting pH vs. VNaOH added. HCl(aq) + NaOH(aq) H₂O(1) + NaCl(aq) Volume NaOH (mL) [H] pH 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 40.00 45.00 48.00 50.00 52.00 55.00 60.00 65.00 70.00 75.00 80.00 95 00 1×10-² Hints: The pH of the solution is calculated using the following equations: (a) Initial conditions (VNaOH = 0), [H'] = [HCI] (b) After initial addition of NaOH and before the end point: MVC-M NOVNO V LV (e) At the end point (Vsaou 50 mL), all the HC1 is being consumed and the acidi of the solution comes from auto ionization of water which is: [H]=1*10 (d) After the end point: [H"]= 1x10-¹4 M XV W V. +K

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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Exam review question 2
How would you prepare 1.40 L of a buffer with a pH of 9.07 from 0.170 M Na CO, and 0.240 M HCl7 For the carbonic acid. Ka (H₂CO3) = 4.45 x 10 and Ka (H₂CO₂) = 4.69 × 10 Mix mL of 0,170 M Nag COs with mL of 0.240 M HCI Submit Answer Try Another Version S tem attempts remaining
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Review I Constants I Periodic Table A 130.0-mL buffer solution is 0.100 M in NH3 and 0.135 M in NH, Br. You may want to reference (Pages 781-791) Section 17.2 while completing this problem. Part A What mass of HCI can this buffer neutralize before the pH falls below 9.00? Express the mass in grams to three significant figures. m= .0023 Submit ΨΕ ΑΣΦΑ X Incorrect; Try Again 772= Previous Answers Request Answer Submit Part B If the same volume of the buffer were 0.270 M in NH3 and 0.390 M in NH, Br. what mass of HCI could be handled before the pH falls below 9.00? Express the mass in grams to three significant figures. VG ΑΣΦ FOX ? Request Answer ? 8 8
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Question 3 3 Consider exactly one litre of a hydrofluoric acid buffer solution, containing 0.800 M HF and 0.528 M F. 3.1 Determine the pH of the buffer solution. - You may use "HA" to denote the formula of the acid. - You may make certain assumptions to simplify your calculations - Ka for hydrofluoric acid is 6.6 x 10-. 3.2 Determine by means of a full calculation the change in pH of the buffer solution that will result when 100. ml. of a 1.00 x 10-2 M HCt solution is added to it. You must indicate all the relevant reaction equations in your working.
Exercise Construct a titration curve by plotting pH vs. VNaOH added. HCl(aq) + NaOH(aq) H₂O(1) + NaCl(aq) Volume NaOH (mL) [H*] pH 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 40.00 45.00 48.00 50.00 52.00 55.00 60.00 65.00 70.00 75.00 80.00 85.00 90 95 100 1x10¹ Hints: The pH of the solution is calculated using the following equations: (a) Initial conditions (VNaOH = 0), [H] = [HCI] (b) After initial addition of NaOH and before the end point: [H]=MCVMNam *V N₂ V LV (c) At the end point (Vsou 50 mL), all the HCI is being consumed and the acidity of the solution comes from auto ionization of water which is: [H]-1×10 (d) After the end point: [H"]= 1x10-14 xV VO+VY M NOW ɔ CLOTHING titrant: NaOH, 0.1M Question 1) What is the pH when the solution volume in the flask reaches 95 ml? a. 12.79 b. 12.82 c. 1.95 d. 12. 75e. 2.28 Question2) What is the maximum pH reached at the end of titration? a. 12.77b. 12.79 c. 12.81 d. 12.78 e. 12.82 analyte: HC1, 0.1 M, 50 ml.
Letter: D, E, F
titration of 35.0 mL of 0.150 mol/L benzoic acid (?? = ?. ? × ?? −? ) with 0.110 mol/L NaOH. a) what is initial pH of benzoic acid b) what is pH after addition of 30ml of NaOH c) what is pH after addition of 60ml of NaOH d) make a sketch of graph
Letter: G, H, I