The breaking buffer that we use this week contains 10mM Tris, pH 8.0, 150mM NaCl. The elution buffer is breaking buffer that also contains 300mM imidazole. The instructor made 3L of elution buffer for all the students. The instructor had 500ml of 4M of Tris (121.1 g/mole) (pH8.0), 750ml of 5M NaCl (MW = 58.44 g/mole) and1.5Ll of 1M imidazole (68.08 g/mole). How much of each stock solution did they need? Show your calculations for credit.

A student added 501 mL of 0.35 M HCl to a buffer solution made up of 0.500 mol of citrate (A-), 0.500 mol of citric acid to 1.5 L of water (total volume = 1.5 L) (Ka = 7.41 x 10-4).   A.) Calculate the pH of the initial buffer solution (before the addition of the acid). B.) Calculate the pH of the solution after the addition of HCl referenced above. C.) Did the buffer solution exceed its buffer capacity?

Explain how the calculation of the molar solubility will be affected if a small amount of the sample adhering to the side of the flask was left unreacted when the end point was thought to have been reached. Procedure: Pipet 25 mL of the saturated Ca(OH)2 solution (without added CaCl2) into a 125 mL flask and add 2 drops of methyl orange indicator. Titrate the Ca(OH)2 solution to the methyl orange endpoint, where the color changes from yellow to red. Titrate two additional 25 mL aliquots of the saturated Ca(OH)2 solution

grade 12 chem:  include units, keep work as precise as possible and apply sig figs only to final answers  If 650 mL of 4.15x10^-4 mol/L BaCl2 is mixed with 550 mL of 4.00 x10^-4 mol/L Na2SO4, will a BaSO4 precipitate form? Ksp (BaSO4) = 1.0 x 10^-10

3. Calculate the molar amount AND the mass (in grams) of sodium acetate (CH,COONa) that must be added to a 1.00-L solution of 0.050 M acetic acid in order to have a buffer with pH <<= 5.20. K.(CH₂COOH) = 1.8 x 10-5 Answers: mol CH:COONa grams CH3COONa:

In acetic acid/sodium acetate buffer the solute particles were Na+, C₂H3O2¯, and HC₂H3O2. With which of these particles did added hydroxide ions (from NaOH solution) react? H₂O O HC₂H₂O2 Na+ O H₂O + C₂H3O2™ C2H3O2 H₂O + HC₂H302

Part A A 350.0 mL buffer solution is 0.150 mol Llin HF and 0.150 mol L-lin NaF. Ka(HF) = 6.3 × 10–4 What mass of NaOH could this buffer neutralize before the pH rises above 4.00? Express your answer using two significant figures. Templates Symbols uado redo reset keyboard shortcuts help m = g Submit Request Answer Part B If the same volume of the buffer was 0.370 mol L-'in HF and 0.370 mol L-lin NaF, what mass of NaOH could be handled before the pH rises above 4.00? Express your answer using two significant figures. Templates Symbols uado redo resat keyboard shortcuts help, m =

Choose the buffer with the greatest buffering  capacity:     d. 0.25M formic acid/formate buffer at pH 3, pKa 3.75   b. 0.25M  HEPESH+/HEPES buffer at pH 10, pKa = 8.08   c. 0.75M acetic acid/acetate buffer at pH 4.76, pKa = 4.76   a. 1M acetic acid/acetate buffer at pH 4.76, pKa = 4.76     Next Page