100 mL of a 100 mM Tris at pH 7.8 is diluted to 1L. What is...

100 mL of a 100 mM Tris at pH 7.8 is diluted to 1L. What is the resulting pH?

Expert Solution

initial volume = 100 ml

initial concentration of Tris = n/v = 100/100 = 1 M

dilution formula, M1V1 = M2V2

(1*0.1) = M2*1

M2 = final concentration of TRIS solution = 0.1 M

after dilution ,

pH of tris = 1/2(pka - logC)

pka of tris = 8.07
= 1/2(8.07-log0.1)

= 4.535

queen_honey_blossom answered 2 years ago

1. Tris buffer a. 100 mM Tris-HCl, pH 8.0 b. 100 mM Tris-HCl, pH 6.0 Make...

1. Tris buffer a. 100 mM Tris-HCl, pH 8.0 b. 100 mM Tris-HCl, pH 6.0 Make this buffer by dissolving an appropriate amount (which you must calculate using the formula weight) of solid Tris in APPROXIMATELY 80 mL of water. Use the Henderson-Hasselbalch equation to calculate how much 1 M HCl is needed to achieve the final pH?

What is the pH of a 100 mL solution of 100 mM acetic acid at pH...

What is the pH of a 100 mL solution of 100 mM acetic acid at pH 3.2 following addition of 5 mL of 1 M NaOH? The pKa of acetic acid is 4.70. A) 3.20. B) 4.65. C) 4.70. D) 4.75. E) 9.60.

How would you make up 100 ml of 50 mM Tris-HCl buffer at pH 7.4, using...

How would you make up 100 ml of 50 mM Tris-HCl buffer at pH 7.4, using the 0.5 M Tris base stock solution, and any other required materials?

You add 100 mL of 60 mM NaH2PO4 and 100 mL of 40 mM Na2HPO4 to...

You add 100 mL of 60 mM NaH2PO4 and 100 mL of 40 mM Na2HPO4 to 300 mL water. What is the final pH of the solution?

A 10.0 mL sample of liquid bleach is diluted to 100. mL in a volumetric flask....

A 10.0 mL sample of liquid bleach is diluted to 100. mL in a volumetric flask. A 25.0 mL aliquot of this solution is analyzed using the procedure in this experiment. If 10.4 mL of 0.30 M Na2S2O3 is needed to reach the equivalence point, what is the percent by mass NaClO in the bleach? Hint: Percent by mass is grams of NaClO / mass of bleach. Presume a density for the bleach of 1.00 g/mL.

Given stock solutions of 25 mM nitrophenyl phosphate, and 1.5 M tris,pH 7.2, 7.5 mM MgCl2....

Given stock solutions of 25 mM nitrophenyl phosphate, and 1.5 M tris,pH 7.2, 7.5 mM MgCl2. If you mix 0.1ml of the nitrophenyl phosphate, 0.7 ml of the tris solution and 0.2 ml of water to bring the total volume to 1 ml, what is the final concentrations of each of the components in the final solution? Show work Nitrophenyl phosphate in mM Tris in M Magnesium chloride in mM

Compare the binding isotherm of normal hemoglobin (at pH 7.4, with 7.8 mM 2,3 BPG) with...

Compare the binding isotherm of normal hemoglobin (at pH 7.4, with 7.8 mM 2,3 BPG) with that of the following variations. For each variant, clearly explain why or why not the binding isotherm changes the way it does. Explain Please! a) Hemoglobin at pH 6.9, 7.8 mM 2,3 BPG b) Hemoglobin in which a glutamate residue (at a position normally exposed to the solvent) has been substituted for a valine residue (at pH 7.4, with 7.8 mM 2,3 BPG) c)...

100 mL of 0.5M NaCl in 25 mM sodium phosphate, pH 8.0. Provide calcualtions and explain...

100 mL of 0.5M NaCl in 25 mM sodium phosphate, pH 8.0. Provide calcualtions and explain how the 0.5M NaCl in 25 mM sodium phosphate buffer, pH 8, will be prepared.

Suppose you want to make 500 mL of a 0.20M Tris buffer at pH 8.0. On...

Suppose you want to make 500 mL of a 0.20M Tris buffer at pH 8.0. On the shelf in lab, you spot a bottle of 1.0M Tris at pH 6.8 and realize you can start with that to make his new buffer. Assuming you have 5.0M HCl and 5.0M NaOH at your disposal, how could you make this 0.20M Tris buffer at pH 8.0 from the 1.0M Tris, pH 6.8? (The pKa of Tris is 8.06.)

If you have 140. mL of a 0.150 M TRIS buffer at pH 8.30 and you...

If you have 140. mL of a 0.150 M TRIS buffer at pH 8.30 and you add 3.00 mL of 1.00 M HCl, what will be the new pH? (The pKa of TRIS is 8.30.)

Question