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- Need both parts ans. Should correct. (Gpt/ai wrong answer not allowed) 1.Calculate the pH when 82.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CH₃NH₂ (Kb = 4.4 × 10⁻⁴). 2.In the titration of 83.0 mL of 0.400 M HCOOH with 0.150 M LiOH, how many mL of LiOH are required to reach the equivalence point?Calculate the pH at 0.0, 10.0, 25.0, 50.0, and 60.0 mL of titrant in the titration of 50.0 mL of 0.100 M NH3 with 0.100 M HCl. Pls answer thank youA titration of 41.0 mL of a malonic acid (H₂C₃H₂O₄) solution of unknown concentration with 0.505 M NaOH requires 65.0 mL to reach the second equivalence point. What is the concentration of the malonic acid solution? Answer: _________ M
- Calculate the pH at the equivalence point for the titration of 0.250 M0.250 M methylamine (CH3NH2)(CH3NH2) with.0.250 M HCl. The ?b of methylamine is 5.0×10−4 (Please type answer no write by hand)Hello ! I have to answer to this question : Generate a curve for the titration of 50.00 mL of a solution in which the analytical concentration of NaOH is 0.1000 M and that for hydrazine is 0.0800 M. Calculate the pH after addition of 0.00, 10.00, 25.00, 35.00, 45.00 and 50.00 mL of 0.2000 M HClO4.I can't do this exercice with Excel and I need to determinate if there are approximations at each step and if there are, I need to verify them . And I can't do it.. Can you help me ? Thank you PaulineChemistry What volume (in mL) of 0.150 M KOH is needed to reach the equivalence point during a titration of 20.0 mL of 0.300 M HBrO
- Titration of a 21.0 mLmL solution of KOH requires 20.0 mL of 0.0150 M H2SO4 solution. What is the molarity of the KOH solution? please be right I got screwed over.Be sure to answer all parts. Find the pH and the volume (mL) of 0.487 M HNO3 needed to reach the equivalence point in the titration of 2.65 L of 0.0750 M pyridine (C5H5N, Kb = 1.7 × 10−9). Volume = mL HNO3 pH =What is the pH at the equivalence point in the titration of 50mL 0.240M HCN with 0.200M KOH, given that Ka for HCN is 4.9 x 10-10? Answer rounded to one decimal place.
- Which of the following is an exact or approximate value of the pH at the equivalence point of a titration of a weak acid with a strong base? Group of answer choices a) 7.00 b) 5.12 c) 9.46 d) 1.55 Need answer with detailed explanation. Will appreciate your efforts. Thank youConsider the titration of 36.0 mL of 0.123 M ammonia with 0.0766 M HCl. (See the Acid-Base Table attached.) (a) How many mL of HCl are required to reach the equivalence point?57.8 mL(b) What is the pH at the equivalence point? 5.29(c) What is the pH of the solution after the addition of 17.2 mL of acid? (d) What is the pH of the solution after the addition of 84.3 mL of acid? (only need help witn c and d)Which solution(s) could be added to 100.0 mL of 0.500 M CH3COOH to produce a buffer solution? Select all that apply. 125.0 mL of 0.500 M KOH Correct! 125.0 mL of 0.500 M NaCH3COO Correct! 75.00 mL of 0.500 M NaOH Correct! 100.0 mL of 0.400 M KCH3COO