You wish to prepare a 0.0125 M buffer with a pH of 5.34. If the pKA of DOMINIC ACID is 5.74, what ratio of DOMINATE/DOMINIC ACID must you use?
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You wish to prepare a 0.0125 M buffer with a pH of 5.34. If the pKA of DOMINIC ACID is 5.74, what ratio of DOMINATE/DOMINIC ACID must you use?
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- what volume of acetic acid 0.1 M and what volume of sodium acetate 0.1 M should be added together to produce a solution (buffer) with a pH of 4.6?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 titration of a polyprotic acid with sufficiently different pKas displays two equivalence points. Why?
- Can someone please explain why and how the step 1 was done? What was its purpose? Why was only the pKa2 value was used in the second step 2? I don't understand shortcuts and I would appreciate it if it's explained step by step. This was the solution to my previous question in which I asked: What is the pH of a buffer prepared by mixing 100 mL 0.050 mM NaH2PO4 and 25 mL 0.075 mM Na2HPO4? (pKa1=2.2; pKa2= 7.21; pKa3=12.7)Find the mass of sodium formate that must be dissolved in 110.0 cm3cm3 of a 1.0 MM solution of formic acid to prepare a buffer solution with pHpH = 3.40. Express your answer to two significant figures and include the appropriate units.In Protein Precipitation, two liters of 5mM buffer solution with pH 5.2 is needed in the isolation of albumin. Note that the pKa is 4.73. Calculate and measure the amounts (in grams if solid and in mL if liquid) of weak acid and conjugate base needed to be able to prepare the chosen buffer system in part A above. Express your answer in useful units (that is, prepare it from practical amounts or concentrations of starting materials). Show the solution step by step.
- You make a 200mM potassium phosphate buffer (pKa of 7.20) with monobasic potassium phosphate (molecular weight 136.09 g/mol) and dibasic potassium phosphate (174.20 g/mol). For 100mL of buffer, at a pH of 7.20, how many grams of monobasic potassium phosphate are needed? Please walk through this step-by-step.How would the results of an experiment change if a basic buffer was utilized instead of an acidic one? in this experiment a strong base and strong acid are titrated agaisnt water and an acidic buffer. however, how were the reuslts differ with a basic buffer? please explainA buffer solution is prepared from an unknown weak acid (HA) and its conjugate salt (NaA). If 500.00 ml of this buffer solution contains 0.025 moles of HA and 0.066 moles NaA, and has a measured pH of 4.61, what is the pKa of the unknown weak acid?
- Determine the mass of solid NaCH₃COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH₃COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵. Let x represent the original concentration of CH3COO- in the water. based on the given values, set up the ICE table in order to determine the unknownWhat 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 ratio CH₃NH₂ to CH₃NH₃⁺ is needed to prepare a pH 10.30 buffer? (Kb for CH₃NH₂ is 4.4 × 10⁻⁴)