Calculate the final pH of 25 mL of buffer 0.1M Tris.HCl/Tris buffer, pH=6.60 after the addition of 1.00mL of 0.1M NaOH. pKa is 8.08.
use the 0.10M Tris.HCl and 0.10M Tris to prepare 100mL, pH=6.6 solution. it calculated by pre-lab, it need 96.8 mL 0.10M Tris.HCl and 3.2mL Tris. and take 25mL pH=6.6 solution, then add 1mL of 0.1M NaOH. Show the final pH
I used similar to the previous problem steps get 6.97, is it right?
Solution Preview
I'm assuming your pre-lab calculations are correct. (If you need me to check your pre-lab calculations as well, do create a new posting).
100 mL of buffer contains 96.8 mL x 0.1 mmol/mL = 9.68 mmol of Tris.HCl
Hence 25 mL of ...
Solution Summary
The pH of a Tris.HCl buffer is calculated after addition of NaOH.
I have four problems that I don't understand how to figure out. I've done problems 16-20 but don't know how to do 21-24.
I've attached the whole page from the exam for the information it provides. I've boxed my previous answers in case they are needed to figure out the four questions.
I need help on the third page. The secon
A buffer solution is made of 0.100 M HOCl and 0.250 M NaOCl. What is the pH of the resulting solution when a 15.0-mL portion of 0.200 M HCl is added to 100.0 mL of the buffer?
See attached file for full problem description.
13. A hydrocholoric acid solution is standardinzed by titrating 0.4541 g of primary stardard tris(hydroxymethyl)aminomethane. If 35.37 mL is required for the titration, what is the molarity of the acid?
15. A sodium hydroxide solution is standardized by titrating 0.8592 g of
Calculate Titration. See attached file for full problem description.
19. Calculate the pH at 0, 10.0, 25.0, 50.0, and 60.0 mL of titrant in the titration of 25.0 mL of 0.200 M HA with 0.100 M NaOH. Ka = 2.0 * 10^-5.
20. Calculate the pH at 0, 10.0, 25.0, 50.0, and 60.0 mL of titrant in the titration of 50.0 mL of 0.100 M N
1- Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution:a solution that is 0.165M in HC 2 H 3 O 2 and 0.120M in KC 2 H 3 O 2. Express your answer using two decimal places.
2- A buffer contains significant amounts of ammonia and ammonium chloride.Write an equation showing how this buffer
What volume (in mL) of 0.37M HCI solution must be added to 265.00 mL 0.29M ammonia solution to give a buffer solution with pH 9.1? (Kb for ammonia 1.80e-5) 1.80 x10^-5
Find the solutions without using the Henderson-Hasselbalch equation. Please show all calculations.
Question #1
A student dissolves 0.25 moles of the acid HA in water and dilutes the solution to the final volume of 500 mL. The student then gives a small portion of the solution to her professor. The professor uses a pH meter
1. Describe how you would prepare 1 liter of each of the following solutions.
a). 1.5 M glycine
b). 0.5 mM glucose
c). 10 mM ethanol
d). 10 mM hemoglobin
2. Describe how you would prepare just 100ml of each of the solutions in problem #1 above
3. When preparing a solution, why do you dissolve the component in less d
Calculate the molarity of a solution prepared by dissolving 3.12 grams of gaseous HCL in enough water to make 26.8 mL solutions.
a. 1.6 M HCL
b. 0.8 M HCL
c. 3.2M HCL
d. 5.4 M HCL
