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- Paragraph BIEE Table 1: pH readings after addition of NaOH to a buffer solution and water Tabel 1: pH metings na byvoeging van NaOH tot die buffer oplossing en water Volume NaOH added Total Volume NaOH added to Volume NaOH bygevoeg Totale Volume NaOH bygevoeg tot pH measurement/ lesing (mL) (mL) Water Buffer Buffer Water 0. 0. 4.6 6.2 5. 5. 4.8 11.4 10 10 4.9 11.7 15 15 4.9 11.9 10 25 25 5.1 12.0 10 35 35 5.4 12.1 20 55 55 6.2 12.2 Path: p » span » strong O555 WIN= Syl.... A solution initial components B Gr... O ACIDS AND BASES Making qualitative estimates of pH change C Each row of the table below describes an aqueous solution at 25 °C. > The second column of the table shows the initial components of the solution. . Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. D H₂O, HNO3 Explanation H₂O H,Ο, ΗΝΟ, We... H₂O Check 14.... initial type (check all that apply) acidic basic neutral acidic basic neutral acidic basic neutral acidic basic neutral Olo o Ol0 0 0000 change add NaNO3 add K Cl add NaOH 14..... add HCl A ALEKS-... effect of change on pH (check one) X Ο ΟΙΟ Ο pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same OpH higher OpH lower OpH the same ♫ tv MacBook AirUse the following atomic masses (in g/mol): Mg = 24.31; O = 16; Ca = 40.08; C = 12.01; Na = 23; H = 1; N = 14.01; S = 32.06; Cl = 35.45; 4.) Sulfamic Acid (H3NSO3) is a monoprotic acid that can be used to standardize NaOH. Compute for the M of NaOH if 34.26mL is equivalent to 0.3337g sulfamic acid.
- E University Librarie. E UNIVERSITY POR. Student Detail Sc. Part A The table shows respective color change when a universal indicator is added to the clear solutions. Rank the samples based on increasing order of acid strength. Solutions Color change 0.001 M lactic Light red 0.01 M phenol Light yellow 0.01 M nitrous acid Light orange 0.001 M hydrogen peroxide Light green Rank the solutions by Increasing order of their acid strength. To rank items as equivalent, overlap them. > View Available Hint(s) Reset Help 0.01 Mnitrous acid 0.001 Mlactic acid 0.001 M hydrogen peroxide 0.01 Mphenol Least acidic Most acidic P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy | Permissions | Contact Us | MacBook Air 80 888 DII DD F3 F4 F5 F6 F7 F8 F9 F10 F11 $ & 3 4 7 8. 9. { R Y U 一 F J K く C V B N M + I| .. .- エ トAn analytical chemist is titrating 118.6 mL of a 0.6400M solution of aniline (C,H,NH,) with a 0.8500M solution of HIO,. The pK, of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 95.6 mL of the HIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places. pH =|| Explanation Check 2021 McGrawH EC 19 MacBook Air 888 F4 F5 esc F2 % & @ 9 6 7 3 4 P Ywhat is the balance equation wirh physical sates of butanoic acid and potassium butanoate as buffer solution.
- 1 2. 3) 6. 10 11 12 13 14 An analytical chemist is titrating 171.3 mL of a 0.5600M solution of propylamine (C,H,NH,) with a 0.8900M solution of HNO2. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 71.3 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = | %3D Submit Assignment Continue MacBook Air F1 F9 F10 F7 F8 80 F3 esc O00 F4 F5 F2An analytical chemist is titrating 186.4 ml of a 0.7700M solution of anilline (C,H₂NH₂) with a 0.7300M solution of HNO,. The pK, of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 51.8 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = 0 X 2How can we answer these questions? 1) What other methods could you have used to identify the unknown chemical? 2). What is/are the dominant species in solution at pH = 4.4? 3) Does the solution at pH = 4.9 constitute a buffer? What about at pH- 5.9? Explain
- 40.00 mL of 0.0900 M NaOH is diluted to 100mL and titrated with 0.1000M HCI. Calculate the pH after the addition of the following volumes of titrant (mL); (d) 30.00 ; (e) 35.95 ; (f) 36.00 (g) 36.05 ; (h) 40.00.6. 10 An analytical chemist is titrating 220.7 mL of a 0.3400M solution of trimethylamine ((CH,) Nv Nwith a 0.6600M solution of HNO, The p K, of trimethylamine is 4.19 Calculate the pH of the base solution after the chemist has added 120.1 mL of the HNO, solution to it. 3. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = Subm Continue Terms of Use Privacy Cente O 2022 McGraw Hill LLC. All Rights Reserved.Data: Provided with the following bottles: Bottle A: NaOH solution Bottle B: HCI solution Bottle C: 0.05 M NH, solution Bottle D: 0.01 M CH,COOH solution Bottle E: Buffer solution Part (1): pH measurements with pH meter: pH 12.67 Solution Bottle (A): NaOH Bottle (B): HCI Bottle (C): NH, solution (0.05 M)10.97 Bottle (D): CH,COOH (0.01 M) 3.39 Distilled water 1.25 6.5 Tap water Boiled distilled water 7.86 Calculations for part (1): 1. Calculate the molarity of NaOH solution. 2. Calculate the molarity of HCl solution. 3. Calculate K, for the weak base NH, cam) solution.