10-14. The Zn in a 0.7556-g sample of foot powder was titrated with 21.27 mL of 0.01645 M EDTA. Calculate the percentage of Zn in this sample.

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For the titration of 50.00 mL of 0.300 M R6C7H5O2 (WB) with 0.200 M HNO3 (SA). Ka (HC7H5O2) = 6.3 x 105 Express pH value to two decimal places. Determine the pH after the addition 12.50 mL of HNO3.

Answer 8b

> C V B M Alt Alt Ctrl + Hc 9. I.C. Calculate the volume of a 0.50 M NaOH(aq) necessary to completely neutralize 50.0 mL of an aqueous 0.1 M CH3COOH solution. This would be considered equimolar amounts of acid and base (a.k.a. the equivalence point of a titration). Show your work.

In the potentiometric titration of phosphoric acid, pH readings at the first and second half-equivalence points were pH1 = 2.12 and pH2 = 7.21 respectively. Determine the Ka1 and Ka2 for phosphoric acid, rounded to 3 sig figs. At the half-equivalence points, pH = pKa. Also, pH = –log [H+] and pKa = –log Ka. Type your answers one below the other. Use formatting tools where applicable.

Answer 8F

10-6. Consider the titration of 100.0 mL of 0.100 M NaOH with 1.00 M HBr. What is the equivalence volume? Find the pH at the following volumes of HBr and make a graph of pH versus Va: Va = 0, 1.00, 5.00, 9.00, 9.90, 10.00, 10.10, and 12.00 mL.

1. What is the pH at the half-stoichiometric point (a.k.a. mid-point) for the titration of 0.22 M acetic acid(aq) with 0.10 M KOH(aq)? For acetic acid, Ka = 1.8 × 10-5.

3:21 1 4 7 +/- Question 7 of 10 In the titration of 230.0 mL of 0.4000 M HONH₂ with 0.2000 M HBr, how many mL of HBr are required to reach the equivalence point? 2 5 8 mL 3 60 9 O Submit Tap here or pull up for additional resources XU x 100