----- DIRECTIONS ----- Welcome to the titration simulator! While simple, I hope it helps provide some valuable practice! You'll be titrating an unknown molarity of HF with NaOH. Click the NaOH button to add NaOH to the solution. Hover over the pH menu to see the pH at each point in the titration. **If you want to calculate the pH for yourself, don't look!** Have fun! ----- GIVEN VALUES ----- These will be helpful in calculations! Ka of HF = 6.6 x 10^-4 NaOH is 0.25M ----- QUESTIONS ----- 1. Sketch a titration curve for this experiment. Include coordinate points for the initial pH, 1/2 Equivalence point pH, and the equivalence point pH. 2. What is the molarity of the HF solution? 3. What is the initial pH of the HF solution? 4. What is the pH of the NaOH solution? 5. What major species are present at the equivalence point? 6. Calculate the Kb of F- (@ 25 degrees C) 7. What is the pH at the equivalence point? 8. You got a higher HF molarity value than expected. What are some possible errors that could cause this? BONUS: Calculate the pH after every 10mL addition of NaOH. STOP! Are you ready to check your answers? Are you sure you finished? Alright, you earned it. Here's the answers! ----- ANSWERS ----- 2. Molarity of HF solution = 1.0M 3. Initial pH = 1.59 4. NaOH pH = 13.40 5. H2O, F-, and Na+ 6. Kb = 1.5 x 10^-11 7. pH = 8.24 at equivalence point 8. The NaOH buret was rinsed with distilled water instead of NaOH, or any other valid reason that will increase the amount of NaOH used. BONUS: 10mL total: pH = 1.59 20mL total: pH = 2.72 30mL total: pH = 3.20 40mL total: pH = 3.68 50mL total: pH = 8.24
A little project I made for AP Chemistry :) Let me know if there's anything I should add or change!
