You are to make 250mL of Edward’s Buffer, the recipe of which is as follows: 25mM EDTA, 250mM Sodium Chloride, 0.5% SDS, and 200mM Tris. But you only have the stock solutions of the following concentration: 150mM EDTA, 2M Sodium Chloride, 20% SDS, and 1M Tris. Explain what each result means in a brief sentence, and indicate how much water is needed.

Using the ionization constants (Ka and Kb), calculate the mass of sodium acetate (CH3COONa), in grams, that must be added to 250.0 mL of a 0.200 M acetic acid solution to make a buffer with pH = 5.00.  (Enter the numerical value in the space provided below.)

Determine the [H3O+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, CH3CO2HCH3CO2H (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. Solution 1.10 M Acetic Acid (mL) 0.900 M Sodium acetate (mL) [H3O+H3O+] (M) 1 8.00 2.00 Solution 1 Concentration 2 7.00 3.00 Solution 2 Concentration 3 6.00 4.00 Solution 3 Concentration 4 5.00 5.00 Solution 4 Concentration 5 4.00 6.00 Solution 5 Concentration 6 3.00 7.00 Solution 6 Concentration 7 2.00 8.00 Solution 7 Concentration 8 1.00 9.00 Solution 8 Concentration Solution 1 Concentration:   M Solution 2 Concentration:   M Solution 3 Concentration:   M Solution 4 Concentration:   M…

What is the highest pH that could be used as an effective buffer with B (a generic base) with Kp = (6.46x10^-10) and its chloride salt, HBCI? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible.

A student needs to prepare a buffer solution with a pH of 4.18. Assuming a pKa of 4.69, how many mL of 0.1 M NaOH would need to be added to 15.0 mL of 0.1 M HB to prepare this buffer? Please include a proper (abbreviated) unit. HINT : Use pH = pKa + log ([B minus]/[HB]) or, if concentrations are the same, pH = pKa + log (Volume of OH minus/ (Volume of HB minus Volume of OH minus)

calculate the ph of a buffer that contain the initial 1,00x10 ^-3 acetic acid and 1,00x10^-4 sodium acetate. ka for CH3COOH =1.80X10^-5 i ) USING HANDERSON -HASSELBACK equation. ii) without using HANDERSON -HASSELBACK equation.

How many grams of dry NH4Cl need to be added to 2.40 L of a 0.300 M solution of ammonia, NH3 , to prepare a buffer solution that has a pH of 8.56? Kb for ammonia is 1.8×10−5 . Express your answer with the appropriate units. (Gpt/ai wrong answer not allowed)