If you add strong acid (such as HCl) to the Tris solution above(25mM solution in 200mL)...

If you add strong acid (such as HCl) to the Tris solution above(25mM solution in 200mL) you can lower the pH. Using the Henderson-Hasselbalch equation (H-H), calculate how much strong acid in mM is need to lower the pH from 10.4 to 8.0.

Remember pKa is 8.2.

You might start by determining the amount of acid and base you have at each pH using the H-H equation. Then compare the differences in this ratio between the two pH values.

Expert Solution

queen_honey_blossom answered 2 years ago

You add 300 mL of Tris-HCl at 0.1 M to a 0.2 L solution of 0.9%...

You add 300 mL of Tris-HCl at 0.1 M to a 0.2 L solution of 0.9% (w/v)NaCl, and to which you add 500 mg of NaCl (powder). What is the concentration of Tris-HCl in mM and in g/L? Tris-HCl : MW 121.14 NaCl : MW 58.44

you add 1 ml of 0.1M HCl to a solution containing 10ml of 0.2M acetic acid...

you add 1 ml of 0.1M HCl to a solution containing 10ml of 0.2M acetic acid (Ka = 1.8x10-5) and 10ml of 0.2 M sodium acetate. What is the resulting pH?

Additional aspects of aqueous solution: 4. In a 50.0mL titration of a strong acid (HCl) with...

Additional aspects of aqueous solution: 4. In a 50.0mL titration of a strong acid (HCl) with a strong base (NaOH) calculate the pH when the following volumes of a 0.100M NaOH solution are added: a.45.0mL b.51.0mL

If I have an unknown acid that has a pH of 6.87 and I add 200ml...

If I have an unknown acid that has a pH of 6.87 and I add 200ml water to make is a solution with a pH of 5.33 and then I titrate it with 11.1 ml of 0.100M NaOH and at my equivalence point i have added 2.089 ml NaOH and the pH is 7.10 and my half equivalence point is after adding only 1.0445 ml of NaOH with a pH of 6.04. 1. What is the pH of the unknown...

consider the titration of a strong acid, HCL, with a strong base NaOH. The 35 ml...

consider the titration of a strong acid, HCL, with a strong base NaOH. The 35 ml of .1 M HCL is in the flask. What is the pH of the solution after 40 ml of .100 M NaOH has been added to to it?

If you add 35.6mL of 5.20M Hcl to 35.6mL of 7.40M NaOH, the solution that you...

If you add 35.6mL of 5.20M Hcl to 35.6mL of 7.40M NaOH, the solution that you generate is what percent NaCl? (Keep in mind the following... you must balance the equation to ge the answer and you must also consider what is the final volume of this solution?)(molar mass of NaCl is 58.44g/mol)

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?

If you have 1 M Tris-HCl solution NaCl 100% Tween How would you make 500 mL...

If you have 1 M Tris-HCl solution NaCl 100% Tween How would you make 500 mL of 0.5 M NaCl, 0.1% Tween, and 100 mM Tris-HCl? i suck at buffer questions.... please help !!!

Consider the titration of a weak base (B- ) with a strong acid (HCl). Draw (this...

Consider the titration of a weak base (B- ) with a strong acid (HCl). Draw (this can be hand drawn) a pH (not pOH) vs mL HCl graph (it will not look the same as the one in question #13; if you start with a weak base, will the pH be low or high? As H+ is added, will the pH increase or decrease?). Label the titration curve with letters A-E, and describe the relative quantities of the dissociated base...

Calculate the pH of each of the following strong acid solutions. (a) 0.00526 M HCl pH...

Calculate the pH of each of the following strong acid solutions. (a) 0.00526 M HCl pH = (b) 0.839 g of HBr in 29.0 L of solution pH = (c) 46.0 mL of 8.80 M HCl diluted to 4.20 L pH = (d) a mixture formed by adding 76.0 mL of 0.00851 M HCl to 23.0 mL of 0.00876 M HBr pH =

Question