How does the change in temperature of Acetate buffer affect the pH of the Acetate buffer when Sodium hydroxide is added?

1. Set the 20.0 °C Acetate buffer solution below the burette system

1. Set up the 25.0 cm³ burettes and the stand like in figure 1
2. Rinse the burette using pure water and repeat 2 times
3. Rinse the burette using 1.00 mol dm^-³ NaOH and repeat 2 times
4. Connect the pH meter and Laptop to the system
5. Pour 25.0 cm³ NaOH into the burette, using a funnel

1. Change the Acetate buffer's temperature to 30.0, 40.0, 50.0, and 60.0°C, correspondingly, for each repetition of sections 6–7.
2. Repeat section ① ~⑧.1 for two more times to maintain the accuracy by having three trials

When small volumes of acidic or alkali are introduced to a solution, a buffer solution assists to limit the pH change (Neuss). The buffer solution is typically created by combining an aqueous solution of a weak base or acid with an equivalent solution of strong alkali or strong acid. Acetic acid (CH₃COOH), a weak acid, sodium acetate (NaCH₃COO), a salt of a weak acid, and a strong alkali will be used in this experiment. In the table below, in section [1], is the equation.

NaOH will be consumed by the reaction and CH₃COOH will remain at a concentration of 0.500 mol because CH₃COOH is the excess reactant and NaOH is the limiting reactant. NaCH₃COO and H₂O will therefore be generated in an amount of 0.500 mol. A weak acid and its salt, which is made from a weak acid and a strong base, are both present in equal proportions in the final solution. Referring to [1],

Additionally, since CH₃COOH is a weak acid when combined with NaCH₃COO, equilibrium will be to the left. (Use the equation in [2] as a guide.) Due to this, the concentration of CH₃COOH is increased.

CH₃COO-(aq), on the other hand, is a soluble salt and is completely dissociated in the solution (Refer to the equation in [3]). As a result, the mixture contains significant amounts of both the conjugate base CH₃COO- and the acid CH₃COOH.

The buffer solution will react with the sodium hydroxide (NaOH) to produce sodium acetate and water. (See equation [4]) As H+(aq) is withdrawn from the solution by interacting with OH- to create H₂O (l), the pH initially rises (Neuss).

Table of equations used in the experiment

1. Check that all equipment is dry
2. Using a 100cm³ graduated cylinder, pour 185cm³ of CH₃COOH.
3. Measure 15.0 cm³ of NaCH3COO with a graduated cylinder of 20.0 cm³.
4. Mix 2 and 3 into a 1.00 dm³ beaker
5. Measure 800cm³ of pure water using a 100 cm³ graduated cylinder and pour it into the 1.00 dm³ beaker
6. Mix and stir using a glass rod
7. Clean up the step 2 beaker and glass rod and wash at the sink

1. Check that all equipment is dry
2. Using a 50.0 cm³ graduated cylinder, measure 50.0 cm³ of 1.00 mol dm^-3 CH₃COOH and pour it into a 500 cm³ volumetric flask.
3. Add pure water to (2) graduated cylinder and rinse it and add to the (2) volumetric flask
4. Add the total of pure water to a 450cm³ (2)volumetric flask using the beaker
5. Using a 50.0 cm³ graduated cylinder, measure 50.0 cm³ of 1.00 mol dm^-3 NaOH, and then pour it into a 500 cm³ volumetric flask.
6. Add pure water to the (5) graduated cylinder and rinse it and move to the (5) Volumetricflask
7. 450 cm³ of pure water total should be added to five volumetric flasks.
8. Shake each volumetric flask of 500 cm³ to ensure proper mixing.

1. Set up the equipment for heating the solution
2. Using the Graduated Cylinder, take out50.0 cm³ of Acetate buffer and pour it into a 100 cm³ beaker
3. Prepare the 50.0cm³ of Acetate buffer solution near the system
4. Set on the Heater
5. Put the Acetate buffer on the heater
6. Use a thermometer to measure and healthy Acetate buffer solution until 20.0 °C

1. Measure the pH of the solution (initial pH)using a pH meter before opening the cook
2. Record it on the paper
3. Open the cock of the burette and drop 1 drop of NaOH into the Acetate buffer
4. Close the cock of the burette
5. Measure the pH using a pH meter for every10.0 drop (0.500 cm³ ) and record it on the paper.
6. Repeat 3 and 4 until the pH reaches 14.0

1. Chemicals
   • 1.00 mol dm^-³ CH₃COOH
   • 1.00 mol dm^-³ NaOH
2. Clothes
   • Lab coat/Eye goggles
   • Cloves/ Cloth
   • Lab coat/Eye goggles
   • Cloves/ Cloth
   • 50 cm³ Burette(± 0.0500 cm³ ) ( handstand )
   • 1.00 dm³ beaker (±3.00cm³ )
   • Electric Heater
   • Alcohol Thermometer (± 0.500 °C
   • Glass Rod
   • pH meter
   • Laptop with Logger Pr
   • Paper and Pencils
3. Equipment
   • 2× 200 Flask ( ±0.0800 cm³ )
   • 2× 500 cm³ Volumetric Flask ( ±0.200cm³ )
   • 10.0 cm³ Graduated Cylinder (±0.0500cm³ )
   • 20.0 cm³ Graduated Cylinder (±0.100cm³ )
   • 50.0cm³ Graduated Cylinder (±0.250cm³ )
   • 100cm³ Graduated Cylinder (±0.500cm³ )

How does the pH of the acetate buffer alter when sodium hydroxide is introduced when the temperature of the acetate buffer changes?

In my chemistry lesson in the fall of 2020, I learned about the buffer solution. As I studied, I discovered how my body's buffer system functions. I was interested to know if blood pH is affected by body warmth. I, therefore, attempted to conduct the experiment involving the change in buffer temperature.

I want to gradually raise the temperature of the buffer solution during this IA by 20.0, 30.0, 40.0, 50.0, and 60.0 °C while monitoring the pH change until the buffer achieves a pH of 12. Then, I want to measure the temperature dependency of the buffer solution and use equation [10] to compute the buffer capacity.

 \([10]\ β=\frac {n}{ Δ𝑝H}\)

The amount of hydrogen ions or hydroxide ions that a buffer can hold without causing a pH shift is known as buffer capacity (Manik). The formula for determining the buffer capacity is shown in [10]. The amount of NaOH added to the acetate buffer solution ("n") to get it to pH 12 is given. The pH difference between the initial and final pHs should be between 3 and 12. The acetate buffer may require more NaOH to be added until it reaches a pH of 12 as the temperature rises. Since the numerator rises and pH should remain nearly constant, the buffer's capacity should rise as well. (Shadi)

1. Pour 500cm³ of 1.00 mol dm^-³ NaOH into the1dm³ beaker