I got the second part of the question wrong, need help. Suppose there is look of an aqueous buffer containing600.0 moral & acetic acid (pk. - 4.76) and 40.0 mmol ofacetate. Calculate the pt of this buffer.pH = pka + log [#]acid[HA]- acetic acid = 60 mmol[A-] acetate = 40 mmalpka = 4.76PH² 4.76 log (128)-14.58B What volume of 3.50 M NaOH would be required to increase.the pH to 4.93?Required ph= 4.93IeE0.17 =10Substitute into Henderson pH = pka + log [CH₂COO][CH3COOL+]4.93 = 4.76 + log (40+ 3.-4.76-4.7660-1.47TOCH3COOH + OH → CH ₂ COO + H₂O3.50x401-3.50x(60-3.50x) D40-3.50x0.1740+3.50x60-2xX = 20.35+3.50X40+ 8.50x160-2xPH40+ 3.50 x40-2x)-3.50 x+3.50x/(40+3,50xکو

NaOH is a base and when it is added to the buffer , it gets add up to the base concentration and…

suppose there is 1.00L of an aqueous buffer containing 600.0 moral & acetic acid (pk. 4.76) and 40.0 ml of acetate. Calculate the pott of this buffer. pH = pka + log [#] and [HA]- acetic acid 60 moal [A-] acetate = 40 mmal pka = 4.76 PH= 4.76 log (488) = 4,58² # PH What volume of 3.50 M NaOH would be required to increase the PH to 4.93?

suppose there is 1.00L of an aqueous buffer containing 600.0 moral & acetic acid (pk. 4.76) and 40.0 ml of acetate. Calculate the pott of this buffer. pH = pka + log [#] and [HA]- acetic acid 60 moal [A-] acetate = 40 mmal pka = 4.76 PH= 4.76 log (488) = 4,58² # PH What volume of 3.50 M NaOH would be required to increase the PH to 4.93?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 15.BCP

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