- 21 Using The Molarity Equation Calculate The Moles Of Naoh At The Equivalence Point Needed To Consume The Hydronium I 1 (87.57 KiB) Viewed 28 times
# 26 Next, Using your results from above you will calculate the Ka of the unknown (mono-protic) acid. First, fill out the following ICE table. Hint: The molarity of the acid you calculated in the previous question is the initial molarity. You also know the equilibrium concentration of hydronium ions. Click here for an example problem. Initial concentration: Edit Submit For Grading Change: Equilibrium concentration: √O # 27 Calculate the Ka of the unknown (mono-protic) acid. Hint: You measured the pH of the acid already. 0 Answer format: Scientific Notation, 2 sig figs: ex: 2.3e-4 % # 28 Please show your work for this answer using the formula editor below. «ΩΙ [bg] {g ΙΡ:ΙτΙΣUI do lime + / 2 - [0] € ∞o √0 Submit i 0² (0) 0 0 101 (0) Submit x ± HA (aq) + + H₂O (1) N/A N/A N/A כ w ØBA S € C ∞ X c 1b Q Mo n TT 4 1b TI Fo... H3O+ (aq) + Siz... - A (aq) C unanswered not_submitted No Retakes. G unanswered not_submitted Attempts Remaining: 10 G unanswered not submitted No Retakes
Get a buret from the stockroom. Fill the buret with about 10 mL of 0.1 M NaOH. Titrate the unknown acid solution in the Erlenmeyer flask by adding small quantities of base from the buret at a time and record the pH of the acid solution after each addition (see suggested amounts for each addition in column-2 of the table below). Record appropriate data and plot pH (column-4) on the Y-axis vs the total volume of NaOH added (column 3) on the X-axis in Excel. When your titration curve has the "S" shape, you can stop collecting the data. Be sure to label the axes in the plot and also give your plot a title. Note: You will see that the pH increases as more and more base is added. Also, the pH will fluctuate more as you get closer to the equivalence point. At the equivalence point, there will be a sudden jump in pH. Keep adding NaOH even after this point to get the S-shaped plot. You may add in larger increments after the equivalence point when the pH begins to somewhat level off. Watch this video on titration curves for reference. Total volume of solution (mL) 10.00 11.00 12.00 12.50 13.00 13.20 13.40 13.50 13.60 13.70 13.80 13.85 13.90 Volume of NaOH added at each step (mL) 0 1.00 1.00 0.50 0.50 0.50 0.20 0.20 0.10 0.05 0.05 0.05 0.05 Total Volume of NaOH added (mL) 0 1.00 2.00 2.50 3.00 3.20 3.40 3.50 3,60 3.70 3.80 3.85 3.90 pH 3,29 12.71 13.11 13.22 13.29 13.32 13.34 13.35 13.36 13.37 13.38 13.39 13.39