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- Ule the Keferences to access important values if needed for this yestinn When a 23.2 mL sample of a 0.386 M aqueous hypochlorous acid solution is titrated with a 0.438 M aqueous bariem hydroside solution. (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 15.3 ml. of barium hydroxide have been added? Submit Answer 2 question attempts remainngTitration of a 86.00mL KOH solution required 398.00 ml of 0.0240 M acetic acid. What is the molarity of KOH solution?For the titration curve below, select one option from the list below for each of these three identification requests: 1) select the most likely type of solutions being mixed from the options provided 2) identify the correct description of the vertical regions noted with "A" from the options provided 3) identify the correct description of the horizontal regions noted with "B" from the options provided
- 6.9 g of citric acid (MM = following balanced chemical equation. 192.1 g/mol) can be titrated with NaOH according to the %3D H3C,H5O7 (aq) + N2OH(aq) → H20(1) + Na H2C,H507(aq) a) Choose the correct titration curve for the titration of the neutralization of the three hydrogens of this acid with NaOH. PH PH pH Titrant Titrant A Titrant B PH PH pH Titrant Titrant D Titrant PHWhat weight of sample should be taken for analysis sos that the volume of 0.1074N NaOH used for titration equals the percentage of potassium acid phthalate (KHC8H4O4) in the sample (Answer 2,193 g)Determine the pH during the titration of 62.0 mL of 0.342 M formic acid (K,- 1.8x104) by 0.342 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 15.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 93.0 mL of KOH
- Titration of unknown acid 1.trial 2.trial 15.0 mL of unknown acid + 12.2 mL NaOH 15.0 mL of unknown acid + 12.4 mL NaOH Calculation of the moles and molarity of the unknown acid solution;What volume of 0.85 M NaOH (in mL) is needed to reach the equivalence point in a titration of 83.0 mL of 0.90 M HCIO4? Your Answer: Answer unitsA 93.0 mL sample of 0.0100 M HIO4 is titrated with 0.0200 M LIOH solution. Calculate the pH after the following volumes of base have been added. (a) 14.4 mL pH = 2.57 (d) 47.4 mL pH = X X (b) 44.2 mL pH = (e) 78.1 mL pH = X X (c) 46.5 mL pH = X
- 5 6 7 8 Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The K, of hypobromous acid is 2.8 x 10¹⁹. A 30.00 mL solution of 0.300 M hypobromous acid (HBrO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LiOH). What is the initial solution pH (i.e., when 0.00 mL of titrant have been added)? (Two decimal places) Type your answer... Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The K, of hypobromous acid is 2.8 x 10¹⁹. A 30.00 mL solution of 0.300 M hypobromous acid (HBrO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LiOH). What volume (in mL) of titrant will have been added at the half-equivalence point? (One decimal place) Type your answer... Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The K₂ of hypobromous acid is 2.8 x 10.⁹. A 30.00 mL solution of 0.300 M hypobromous acid (HBrO) is being titrated with a solution that is 0.600 M in lithium hydroxide…1. The titration curve shown at right represents which type of reaction? (a) A strong acid added to a strong base. (b) A strong base added to a strong acid. (c) A strong acid added to a weak base (d) A strong base added to a weak acid. volume of titrant added (from buret) pH of flaskYou can measure the amount of FeSO4 in an aqueous solution by titrating the solution with a standardized solution of any if the following except… Group of answer choices HCl EDTA NaOH KMnO4