Current Attempt in Progress Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a b

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Current Attempt in Progress Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer solution containing 23 g of NH₂Cl dissolved in 1.00 L of 0.919 MNH₂? pH- (b) How many moles of acid are required to change the pH of this solution by 0.05 pH units? (c) Suppose 5.8 mL of 12.6 MHCI solution is added to 467 mL of the solution of Part (a). Calculate the new pH. pH- eTextbook and Media mol Save for Later
Question 9 of 16 < View Policies Current Attempt in Progress The pH of an acetic acid-acetate buffer is 4.58. What is the [A VIHA] concentration ratio? eTextbook and Media Hint D Save for Later -/8 E Attempts: 0 of 3 used Submit Answer
Question 10 of 16 < View Policies Current Attempt in Progress One of the most common buffers used in protein chemistry is a weak base called TRIS (the nitrogen atom of the amino group is the basic portion of the molecule): pH= HO. HO eTextbook and Media -NH₂ OH A biochemist prepares a buffer solution by adding enough TRIS and 12 M HCI to give 1.0 L of a buffer solution that has concentrations [TRIS] 0.28 M and [TRISH*] -0.65 M. (pK, of TRIS is 5.91.) (a) Calculate the pH of the buffer solution. (HOCH₂)CNH, TRIS (b) Suppose that 6.6 mL of 12 M HCI is added to 12 L of the buffer solution; calculate the new pH of the solution. PH Save f Last saved 44 minutes ago. Saved work will be auto-submitted on the due date. Auto- submission can take up to 10 minutes -/6 ! Attempts: 0 of 3 used Submit Answer
Question 12 of 16 Calculate the ratio [HCOO (aa)]/[HCOOH(aq)] in the buffered solution required to achieve a pH of 3.33. [HCOO{ag)]/[HCOOH{ag)| = | eTextbook and Media Hint < We want to prepare a buffered solution having a pH of 3.33 using concentrated (23.6 M) formic acid (HCOOH) and solid sodium formate (HCOONa). K, for formic acid is 1.8 x 10 Save for Later Hint -/6 Attempts: 0 of 3 used E Submit Answer If the total molarity of formic acid plus formate ion in the buffered solution is 0.200 M, calculate the volume of concentrated acid and mass of sodium formate that must be dissolved in 1.00 L of water. mL formic acid g sodium formate