A 1.0-L 0.010 M buffer with pH 6.50 is given as an assignment to a group of students. Which is the most appropriate weak acid to be used in the buffer preparation?
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- Calculate pH of buffer prepared by mixing; 10ml of 0.10M of CH3COOH and 20ml of 0.10M of CH3COONa.You need to prepare an acetate buffer of pH 5.43 from a 0.621 M acetic acid solution and a 2.95 M KOH solution. If you have 730 mL of the acetic acid solution, how many milliliters of the KOH solution do you need to add to make a buffer of pH 5.43? The pKa of acetic acid is 4.76. Be sure to use appropriate significant figures.Make a list of the five most critical qualities of an effective extraction buffer. Please provide a brief description of each.
- A buffer contains 0.015 mol of lactic acid (pK₁ = 3.86) and 0.080 mol of sodium lactate per liter. H₂C OH Lactic acid OH Calculate the pH of the buffer. H₂C. Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of the buffer. O OH Sodium lactate Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of pure water. O Na+ buffer pH: buffer pH change: water pH change: units unitsWhich of the following combinations would be the best choice to buffer the pH of a solution at approximately 7? Ionization Constants for Aqueous Weak Acids at 25 °C Acid K. (pK,) Conjugate Base Hydrogen phthalate ion, Cg H4(CO2H)(CO2) Acetic acid, CH3 CO,H Acetate ion, CH; CO2- 1.8 x 10-5 (4.74) Weak Acid Phthalic acid, C6 H4 (CO,H)2 1.3 x 10-3 (2.89) Dihydrogen phosphate Hydrogen phosphate ion, H2 PO4 Hydrogen phosphate ion, HPO42 6.2 x 10-8 (7.21) ion, HPO,2- Phosphate ion, PO,* 3.6 x 10-13 (12.44) O Na, HPO4 and NagPO4 O NaH2 PO4 and NazHPO4 O H;PO4 and NaH2 PO4What is the pH of the solution given the following information? Methyl orange = yellow Methyl red = yellow Bromothymol blue = green Note: use the provided reference table for color indicators below as a guide pH 5 pH 8 pH 7 pH 6
- How much of the enzyme proteinase k (solute) is required to make 250ml of a solution with a concentration of .01mg/ml? (Weight/volume ratio)The pHpH scale for acidity is defined by pH=−log10[H+] where [H+]is the concentration of hydrogen ions measured in moles per liter (M). A solution has a pH of 10.2. Calculate the concentration of hydrogen ions in moles per liter (M).I want to make a buffer solution containing 1 M glycene pH = 10 (Na+), 1 mM ZnCl2 , 1 mM MgCl2. I have the stock solutions 1 M glycene, 1 M MgCl2, 1 M ZnCl2, and 10 M NaOH. My final volume of buffer solution needs to be 250ml. how much (in ml) of each solution should i put into my buffer?