How would you make 100mL of tartrate buffer, pH 3.5, from 0.100 M tartaric acid, 1M NaOH and deionized and distilled H2O? You need to consider the ionization of two the two acidic groups separately.
Well, making a tartrate buffer is a piece of cake! Let's break it down and have some fun!
First, let's pretend we're in a chemistry magic show. To create your 100 mL of tartrate buffer, pH 3.5, you'll need two main ingredients - tartaric acid and NaOH. Just remember, safety goggles and lab coat are essential for this magical adventure.
Step 1: Grab your magician's hat and measure 50 mL of your 0.100 M tartaric acid solution. This will provide you with an acidic kick to start the buffer creation.
Step 2: Now it's time to neutralize that acidity! Take your wand, I mean your pipette, and carefully measure the exact amount of 1M NaOH needed to achieve pH 3.5. This may require some tinkering and adjusting, but remember, practice makes perfect!
Step 3: Ah, the joy of balancing act! Add the NaOH drop by drop to your tartaric acid solution and watch the pH meter dance. Take your time, my magical friend, and remember, patience is key.
Step 4: As you approach the desired pH of 3.5, you might feel like you're walking on a tightrope. But fear not, keep adding those NaOH drops and gently stirring until the pH meter shouts, "Ta-dah! pH 3.5!".
Step 5: Now, take a moment to appreciate your creation. You've conjured a magnificent 100 mL of tartrate buffer with a pH that would make any chemist proud.
Step 6: Finally, fill the rest of the 100 mL volumetric flask with some deionized and distilled water to complete your buffer solution. And there you have it, a perfectly balanced buffer ready to regulate pH in the most whimsical way possible!
Remember, my dear magician, always keep a sense of humor while working with chemicals. Chemistry can be challenging, but with a little bit of magic, laughter, and safety precautions, you'll always succeed!
To make a 100 mL tartrate buffer solution with a pH of 3.5, using tartaric acid and sodium hydroxide (NaOH), you need to consider the ionization of both acidic groups in tartaric acid separately.
Here's how you can proceed:
1. Calculate the amount of tartaric acid required:
Tartaric acid has two acidic groups that can ionize independently. To calculate the required amount of tartaric acid, you need to determine how much of it is needed to reach a specific concentration of the tartrate ion.
The pKa values for tartaric acid are 2.97 and 4.34. Since you want a pH of 3.5, which is between the two pKa values, the buffer will consist of a mixture of the acid and its conjugate base.
Using the Henderson-Hasselbalch equation (pH = pKa + log [A-]/[HA]), we can calculate the ratio of [A-] to [HA] required to achieve pH 3.5.
At pH 3.5:
pKa = 2.97
[A-]/[HA] = antilog(pH - pKa) = 10^(3.5 - 2.97) = 3.63
Let's assume 'x' as the amount (in moles) of tartaric acid required. Then, the amount of tartrate ion (A-) formed will be 3.63 times 'x'.
2. Calculate the volume of 0.100 M tartaric acid solution:
Now, you can calculate the volume of the 0.100 M tartaric acid solution needed to obtain 'x' moles of tartaric acid.
Volume (V) = moles (n) / concentration (C)
V = x / 0.100
3. Calculate the amount of NaOH required:
The amount of NaOH required will depend on the number of moles of tartaric acid. Since there is a 1:1 stoichiometric ratio between tartaric acid and NaOH, the amount required will be the same as the moles of tartaric acid.
4. Calculate the volume of 1 M NaOH solution:
Using the concentration and the amount required, we can calculate the volume of the 1 M NaOH solution needed.
Volume (V) = moles (n) / concentration (C)
V = x / 1
5. Prepare the buffer solution:
Combine the calculated amounts of tartaric acid, NaOH, and deionized/distilled water to make 100 mL of solution. First, dissolve the tartaric acid in a portion of the water and then add NaOH until the solution reaches the desired pH of 3.5. Finally, add more water to make the total volume up to 100 mL.
Remember to take proper safety precautions while handling chemicals, use proper lab equipment, and follow any specific guidelines given by your instructor or institution.