Calculate the pH of 1.00 L of 0.195 M HC2H3O2 /0.125 M C2H3O2 - buffer system after the addition of 10.20 mL of 1.00 M HCl. [HC2H3O2: Ka = 1.8 x 10-5 ) (b) Compare the new pH with what you calculated from problem 1. Is the HC2H3O2 /C2H3O2 - mixture effective as a buffer? Explain. (c). Which buffer system is the best choice to create a buffer with pH = 7.20? Explain your choice. (HC2H3O2 Ka = 1.8 x 10-5 ; NH4 + Ka = 5.6 x 10-10; HClO2 Ka = 1.1 x 10-2 ; HClO Ka = 2.9 x 10-8 ) HC2H3O2/KC2H3O2 NH3/NH4Cl HClO2/KClO2 HClO/KClO.        Solution part a,b,c properly fast

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A: The answer for part (a) is given below. Kindly post the other sub parts as separate questions Given:…

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A: · Moles of H3PO4 = 5.46 mol· Moles NaOH = 2.97 mol· Volume of solution = 1.00 L· Ka1 = 7.5 × 10–3

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Q: A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500…

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Q: Pls help ASAP.

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Q: Question attached

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.