A buffer with a pH of 11.2 contains CH3NH2 and CH3NH3C1 in water. You may want to reference (Page) Section 17.2 while completing this problem. Part A What can you conclude about the relative concentrations of CH3NH2 and CH3NH3C1 in this buffer? For CH3 NH2, pK, = 3.36. CH3NH2 = CH3NH3C1 CH3NH2 >CH3NH3 Cl CH3NH2
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Q: Study guide answer is 4.77 for part 2 please show steps thanks
A:
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- The Tris buffer system is commonly used in biochemistry as its pKa of 8.1 allows it to buffer close to physiological pH. (CH2OH)3CNH2 + H+ Û (CH2OH)3CNH3+ What concentrations of Tris and Tris H+ are obtained in a 200 mL solution at pH 8.20 containing 6.1g of Tris? The molecular mass of Tris is 121.1 gmol-1 Please do this step by step thank you!If the solubility of Li2CO3(s) is 1.3 x 10-4 mol/L, what is its Ksp?What is the proper unit of molar ratio of weak acid and its conjugate base in a buffer solution? Is it mol to mol or part to part? Or is it unitless? I need to express the answer 1.45/1 = [A]/[HA] to the right unit. See image for more details. the buffer is acetic acid/sodium acetate buffer.
- The following text may be found at the ThermoFisher website: "PBS (phosphate buffered saline) is a pH-adjusted blend of ultrapure-grade phosphate buffers and saline solutions which, when diluted to a 1X working concentration, contains 137 mM NaCl, 2.7 mM KCl, 8 mM Na2HPO4, and 2 mM KH2PO4. Each 10X PBS solution is ready to use upon dilution to the desired concentration." This means that the product that you purchase has a concentration 10 times the concentration at which it is used. 1. Look up the pKa values for phosphoric acid and list them as a part of your response. 2. Based on the description of the contents of the PBS buffer, calculate the pH of the 1X solution. 3. Assume that you wish to use a pH = 7.00 buffer. If your answer to 2 was more acidic than pH 7.00, calculate how much 1.00 M NaOH you would need to add to get to pH = 7.00. If your answer to 2 was more basic than pH 7.00, calculate how much 1.00 M HCl you would need to add to get to pH = 7.00.How the pH at the equivalence point is determined by the species present; why the pH at the midpoint of the buffer region equals the pKa of the acidThe ratio CH₃NH₂ to CH₃NH₃⁺ is needed to prepare a pH 10.30 buffer? (Kb for CH₃NH₂ is 4.4 × 10⁻⁴)
- A solution is made by dissolving 0.1283 g of the acid form of the buffer TRIS (molecular mass = 157.60 g/mol) along with 0.1975 g of the basic form of TRIS (molecular mass = 121.136 g/mol). The pK a of TRIS is 8.08. A very small amount of potassium dihydrogen phosphate is added (not enough to cause any change in the pH). What is the fractional amount of the potassium dihydrogen phosphate that is in the PO 4 3- form? Phosphoric acid is a triprotic acid with pK a1 = 2.16, pK a2 = 7.21 and pK a3 = 12.32.How do the concentrations of Pb2+ and S2− change when K2S is added to a saturated solution of PbS? The concentration of Pb2+ will ---Select--- increase, decrease, remain the same and the concentration of S2− will ---Select--- increase, decrease, remain the same .How did diluting the buffer affect the pH of the buffer solution itself? ( pls explain it asap!) Thank you
- Hello, can someone please help me with these chem questions and give me a clear step-by-step solution. Thank you very much for your help. (there is also a chart that is included in the question) Question: Determine the [H3O+] of the eight buffer solutions made by mixing 1.10 M acetic acid and 0.900 M sodium acetate solutions according to the following volumes. The pKa for acetic acid, CH3CO2H (HAc), is 4.745. You will also need this information in your post-lab. It is highly suggested you write these calculations down (both unrounded and rounded values) to use later. To enter exponential values, use the format 1.0e-5:Calculate the pH of a bicarbonate buffer that is composed of a solution that is 0.5 M sodium carbonate and 0.05 M carbonic acid. The pK is 6.10.You will be handling cells that are viable at pH 5.5. Which of the following buffer systems should you use for these cells? Explain your answer. A. CH3COOH - CH3COO- , Ka of CH3COOH = 1.8x10^(-5) B. NH3 - NH4+ , Kb of NH3 = 1.8x10^(-5) C. HONH2, HONH3+ , Kb of HONH2 = 9.1x10^(-9) D. C5H5N, C5H5NH+ , Kb of C5H5N = 1.5x10^(-9)