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- Solution A: 1.7 x 10-5 M HCI Solution B: 3.40 8 of CH3C0ONa.3H20 in 250 mL of 0.1 M CH3COOH (Buffer solution) 0.IM NaOH and methyl red indicator pH solution steps obseration Solution A Addition of a few drops the colour changes from clear to pink 4.68 of methylred (HCL) Addition of 10 drops of The colour change from clear to pink 4.73 0.1 M NAOH Soluion B Addition of a few drops The colour change from pink to clear of methyl red (buffer solution) Addition of 10 drops of The colour stays the same 4.73 0.1 M NaOH a) Calculate the pH of a buffer system made up of 0.25 M C6H5C0OH and 0.35 M C6H5COONa. b)What is the pH after the addition of 20 mL of 0.I M HCI to 500 ml of the above buffer solution? c)Describe how you would prepare a IL solution of 0.1 M sodium acetate (CH3CO0Na)/0.I M acetic acid (CH3C0OH) buffer system with a pH of about 5.Chemistry A 20 mL solution containing both Ca2+ and Mg2+ cations is diluted in to 100 mL. When 10 mL of this solution is taken and titrated with 0.05 M EDTA at pH = 10 in the presence of Erio – T indicator, the consumption is found as 12 mL. A new 10 mL was taken from the same solution and (NH4)2C2O4 is added on it and then formed the precipitate is filtered. The filtered solution is titrated with the same EDTA solution and the consumption is found as 3 mL. So find the Ca2+ and Mg2+ amounts in the main sample solution in terms of mg/L.OpenVellumHMAC=defce5f03204e95efa2fcf11b1ecff98#10001 I Review | Constants | Periodic Table [base] pH = pK, + log Tacid 3.5 x 10 2 -log(1.8 x 10-5)+ log 0.1025 4.74 – 0.467 4.28 Part C For 500.0 mL of a buffer solution that is 0.185 M in CH,CH,NH, and 0.135 M in CH3CH,NH CI, calculate the initial pH and the final pH after adding 2.0x10-2 mol of HCl (K,(CH CH,NH,) = 5.6 x 10 4) Express your answers using two decimal places separated by a comma. pHinitial. pHrinal 10.89, 11.12 Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Provide Feedback Next > P Pearson at © 2022 Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy | Permissions Contact Us 11:57 PM 4/16/2022 lyp DDI C dele %3D backspace 00
- A professor prepares a buffer solution that they need for the purification of protein from human cell lysates. They did mix weak acid and conjugate base and obtained the initial solution, which is characterised by these parameters. Final volume: 200mltotal buffer compound concentration: 150mMIntitial concentration weak acid: 0.03MInitial concentration conjugate base: 0.12MInitial pH 6.9buffer compound pka 6.3If the standard solutions had unknowingly been made up to be 0.0024 M AgNO3 and 0.0040 1 MK2CrO4, what would be the value of Ksp? The value of Ksp would be larger. The value of Ksp would be smaller. The value of Ksp would be the same. O More information is needed to answer this question.pH of solution made by mixing 200 mL of 0.2 M CH3COONa and 400 mL 0.1 M CH3COOH is [pKa(CH3COOH) = 4.7] %3D 3.2 4.7 5.2 6.8
- 50mL aliquotof 0.0500M NaCN istitrated with 0.100M HCl.The reaction is: CN- +H3O+ ↔HCN+H2O Calculate the pH after the addition of: a) 0.00mL b) 10.00mL c) 25.00mL d) 26.00mL of acidA 250.0 mL 0.100 M buffer solution at pH 7.0 is to be prepared. The following reagents are available in the laboratory: 1.0 M H3PO4, 1.0 M NaH2PO4, solid Na2HPO4 (MM = 141.96), and solid Na3PO4 (MM = 163.94). Constants: pKa1 = 2.30, pKa2 = 7.21, pKa3 = 12.10 A. What are the amounts (in M) of the acidic and basic components in the buffer? B. What are the amounts (in g or mL) of the reagents needed to prepare the buffer?In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one to be used? (pK, of the weak base B is 10.50). Indicator 2: Methyl red: pH transition = 4.8-6.0 Indicator 1: Cresol purple: pH transition = 1.2-2.8 Indicator 4: Thymolthalein: pH transition = 8.5-10.5 O Indicator 5: Indigo Carmine: pH transition= 11.6- 14.0 O Indicator 3: Cresol red: pH transition = 7.2-8.8
- bn the lab vou titrated 40 ml of 0.006 M Ca with 0.008 M EDTA at pH 10. What was the pCa in that titration at the following points r4 B 16. After adding 1I5 ml of titrant, the pCa is (a) 2.35 (b) 2.66 (c) 2.92 (d) 3.22 C17. At equivalence point, the pCa is (a) 6.36 (b) 6.81 (c) 7.45 (d) 7.98 C18. Alter adding 45 ml of titrant, the pCa is (a) 8.75 (b) 9.32 (c) 9.95 (d) 10.37Compare the 2 quantities based on the given condition. Choose A If quantity in Column 1 is greater B If quantity in Column 2 is greater C If the two are equal D If relationship cannot be determined Titration of 25.0-mL 0.0150 M Fe2+ solution I. Volume at EP using 0.0100 M Ce4+ as titrant II. Volume at EP using 0.0100 M Mn04- as titrant2. Measurement of the pK, of Acetic Acid by the Half-Neutralization Method 1.00 Concentration of standardized NaOH titrant mole/L Trial 1 Trial 2 Trial 3 Mass of acetic acid solution 20.0 20.0 Volume of NaOH added to half-neutralize the acetic acid 0.40 mL 0.40 mL mL Measured pH of half-neutralized solution 4.68 4.66 28-7 Average pH value pk - K, = Calculate the [H,0*) and the concentrations of A- and HA, in the half-neutralized solution (Note: In this solution, [H,O*] # [A-].)
