Answer Happy

Part A Consider the titration of 36.4 mL of 0.260 MHF K = 3.5 x 10) with 0.220 M NaOH. Calculate the pH at each of the following points. How many milliliters of base are required to reach the equivalence point? Express your answer using three significant figures. V AED ? VOR mL Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining 1 Part B Calculate the pH after the addition of 9.10 ml of base Express your answer using two decimal places. ΟΙ ΑΣφ ? pH

Part C Consider the titration of 36.4 mL of 0.260 M HF К. 3.5 x 10 *with 0.220 M NaOH. Calculate the pH at each of the following points. Calculate the pH at halfway to the equivalence point. Express your answer using two decimal places. 170 ΑΣφ pH- Submit Request Answer Part D 1 Calculate the pH at the equivalence point Express your answer using two decimal places po AEC ? pH- Submit Request Answer

Request Answer Part E Calculate the pH after the addition of 72.8 mL of base. Express your answer using two decimal places. ΟΙ ΑΣφ ? pH = 1