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1)
Given,
Concentration of CH3COOH solution = 0.15 M
[CH3COOH] = 0.15 M
Concentration of NaCH3COO solution = 0.10 M
[NaCH3COO] = 0.10 M
Acid dissociation constant (Ka) for CH3COOH = 1.8 × 10-5
pH of a buffer solution = ?
Step by step
Solved in 4 steps with 1 images
- Sodium acetate buffers are used for purification and precipitation of nucleic acids, as well as for protein crystallization and staining gels used in protein electrophoresis. It is very popular in hematology, since there is some evidence that acetate-buffered infusions show improved stability. Acetate buffers are inexpensive and simple to prepare, and can be stored at room temperature. 27-29. Calculate the pH of the acetate buffer solution that contains 0.50M acetic acid (Kb=5.56x10-10) and 0.50M sodium acetate. 30-32. Calculate the change in pH that occurs when 0.010 mol NaOH(s) is added to 1.0L of the acetate buffer. 33-35. Compare the pH change with that when 0.010M of NaOH is added to 1.0L of pure water. 36-40. How can the pH of the buffered solution not increase even though a strong base, NaOH, is added? Explain using the ions present.(5) a) A nitrous acid/sodium nitrite buffer solution is prepared. 20.0 mL of 6.50 M nitrous acid (HNO2) and 8.52 g of sodium nitrite (NaNO2, molar mass 68.99 g/mol) are placed in a 250. mL volumetric flask. The flask is filled to the mark with water and inverted 10 times to mix thoroughly. What is the pH of this buffer? Take Ka for Nitrous Acid to be 4.52 x 10-4. pH: b) 2.00 mL of a 2.50 M solution of NaOH is added to 75.0 mL of the buffer prepared above. What is the pH of this solution? How much did the pH change? pH: change in pH: c) What is the pH of pure distilled water (just give the pH, no calculations are necessary). d) If 2.00 mL of 2.50 M…please stop rejecting. we pay for this service, so we deserve getting our answer! I do not want to have to put a claim in and report Use acid-base titration to determine theconcentration of:– A strong acid: HCl 0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOH Phenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10
- In Protein Precipitation, two liters of 5mM buffer solution with pH 5.2 is needed in the isolation of albumin. 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). Pls. show the step by step process on solving the problem.a) At temperature 25°C, 0.02 M hydrazine, N2H4 solution is 0.69% ionised. Calculate the i. Concentration of OH- ion ii. ionisation constant, Kb b) Calculate the mass of sodium benzoate, C6H5COONa that should be added to 500 mL of 0.2M aqueous benzoic acid, C6H5COOH solution to produce a buffer with pH 3.50?[ Ka for C6H5COOH = 6.3 x10-5] c) When a 1 x 10-3 moldm-3 solution of CaCl2 is mixed with an equal volume of a 1 x 10-3 moldm-3 solution of Na2SO4, will precipitate form? (Ksp CaSO4= 2 x 10-5) Do you mean that pH? That was all the given information the question gave.. I don't understand how to use the ionised part the mostYou 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.
- Caclulate the buffer intensity, b, of a 10-1 M (= CT) acetic acid solution at pH 5 and pH 7. For each pH determine the individual contributions of the acetic acid (bHAc) and of water (bH20) to the total buffer intensity (b).Compute the solubility of Mg(OH)2 in a buffer solution at pH=10.42. The solubility product of magnesium hydroxide is 1.2E-11Include at least 3 significant figures in your answer.In the supersaturated solution Group of answer choices Q = Ksp Q < Ksp Q > Ksp Ka = Ksp Calculate the pH of a buffer solution prepared by mixing 25 mL 0.400 M butyric acid, HC4H7O2 and 35 mL of 0.200 M potassium butyrate, KC4H7O2. Ka of butyric acid is 2.76 x 10-6. Group of answer choices 5.40 3.60 6.30 4.50
- When a drop (taken to be 0.20 cm3) of 1.0 M HCI(aq) is added to 25 cm3 of pure water, the resulting hydroniumion concentration rises to 0.0080 mol dm- 3 and so the pH changes from 7.0 t o 2.1, a big change. Now suppose the drop is added to 25 cm3 of an ethanoate buffer solution that is 0.040 MNaCH3CO2(aq) and 0.080 M CH3COOH(aq). What will be the change in pH?Methodolody: (Include a short summary of the overall experimental plan you are going to run. You may use flow chart or bullet form for this part. Sketches of any experimental set-ups used in the experiment or the workup procedures). Preparation of buffers Prepare 250ml of the following buffer solutions. Concentration Buffer solution pka Desired ph 0.50 M Phosphate 2.12 3.0Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution. 2MnO4- + 5C2O4-2 +16H+ -> 2Mn2+ + 10CO2(g) + 8H2O Calculate the molar concentration of the KMnO4 solution. Pls show step by step. What type of molecules will interfere in this analysis ?