3.1) as a buffer for your You are interested in using lactic acid (pka biochemical experiment. a) Would it be most useful for creating a buffered solution at pH 2, 4 or 6? Explain. b) You decide to use lactic acid to make 1.5 L of 50.0 mM buffer at the pH you selected in part a. Determine the concentrations of lactic acid and its conjugate base that are required. =

Solve correctly please. (Gpt/Ai wrong answer not allowed)

Part A B and C

need explanation y other options are in correct too

Buffer C: 100.0 mL at pH= 12.000, [conj.base] = 0.500 M conjugate acid: HPO4 ^2- conjugate base: PO4 ^3- require concentration (in M) =1.05 mass of solid necessary as source of conjugate acid: 14.9 g

This question has multiple parts. Work all the parts to get the most points. a Identify the buffer system(s) - the conjugate acid - base pair(s) - present in a solution that contains equal molar amounts of the following: (Select all that apply.) HC1 KCN | HNO2 KNO2 b (Select all that apply.) OK,CO3 H,CO3 KF HF

Learning Goal: To calculate the pH at the equivalence point for various types of titrations. The equivalence point in an acid-base titration is the point at which stoichiometrically equivalent quantities of acid and base have been mixed together. At this point the reaction is complete because all analyte has been consumed by titrant. On a titration curve, the equivalence point is represented by the point of inflection (where the curve changes concavity). The figure (Figure 1) shows the titration of 40.0 mL of 0.100 M HCl with 0.100 M NaOH. When 40.0 mL of the NaOH solution is added, the acid-base neutralization reaction is complete. When analyzing titrations involving weak acids or bases, consider how the neutralization reaction will impact the pH of the system. For example, when titrating a weak acid with a strong base, at the equivalence point all the base has been used to neutralize the acid forming its conjugate weak base Figure E 14 12 10 8 6 4 2 0 0 Equivalence point 20.0 40.0 mL…

(Correct!) When 0.300 g of a diprotic acid was titrated with 0.100 M LIOH, 40.0 mL of the LiOH solution was needed to reach the second equivalence point. Identify the formula of the diprotic acid. H₂C4H4O6 (Your correct answer) H₂C204 H₂Se H₂S H₂ Te

ortant values if needed for this question. Design a buffer that has a pH of 4.66 using one of the weak base/conjugate acid systems shown below. Ka pka 2.4x10-11 10.62 1.7x10-8 7.77 6.7x10-6 5.17 Weak Base Kb Conjugate Acid 4.2x 10-4 CH3NH3+ CH3NH₂ C6H1503N 5.9x107 C6H1503NH+ C5H5N 1.5x109 C5H5NH+ How many grams of the chloride salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams chloride salt of conjugate acid = grams weak base =