Bicarbonate Buffer a. Prepare 100 mL of 0.200 bicarbonate buffer, pH 10, by calculating the mass of sodium bicarbonate and sodium carbonate. b. Use the Henderson-Hasselbalch equation to calculate the volume of each stock solution needed.                                pH = pKa + log [conjugate base] / [weak acid]1 c. Check your calculations with other students. See the instructor if there is uncertainty. d. Make the solution and check the pH of a portion of your buffer solution using the pH meter.                                                L = 245μL   Preparation of Bicarbonate Buffer Calculated Volume: CH3COOH = _______________ KH2PO4 = ________________ Actual pH of the buffer: _____12.65_____ NOTE: Please answer letter A, I need the volume. I already know how to calculate the actual pH. Thank you.

Q: Chemistry

A: Step 1:Step 2:Step 3:

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.