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Part A What is the pH at the equivalence point in the titration of 100.0 mL...
Q2 Part B
What is the pH at the equivalence point in the titration of 100.0 mL of 0.0500 M HOCI (Ka = 3.5 x 10-8) with 0.400 M NaOH? Express your answer to two decimal places. ΤΕΙ ΑΣΦ ? pH = 19.76 Submit Previous Answers Request Answer X Incorrect; Try Again A certain weak acid, HA, with a Ka value of 5.61 x 10-6, is titrated with NaOH. Part A A solution is made by titrating 8.00 mmol (millimoles)...
What is the pH of a solution of 40.0 mL of 0.100 M acetic acid (Ka = 1.8 x 10-5) after 50.0 mL of 0.100 M NaOH has been added? Calculate the concentration of dissolved Ba2+ ions when BaSO4 is added to water at 25°C. Кsp? = 1.10 x 10-10 A particular saturated solution of silver chromate (Ag2CrO4), has [Ag+] = 5.0 x 10 Mand (CrO4) = 4.4 x 10M. What is value Ksp for silver chromate? As a result...
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Calculate the concentration of dissolved Ba2+ ions when BaSO4 is added to water at 25°C. Кsp? = 1.10 x 10-10 A particular saturated solution of silver chromate (Ag2CrO4), has [Ag+] = 5.0 x 10 Mand (CrO4) = 4.4 x 10M. What is value Ksp for silver chromate? As a result of mineral erosion and biological activity, phosphate ion is common in natural waters. If [Ca 2+] = 1 x 10-6 M and [PO43-)...
Find the pH of each of the following solutions of mixtures of acids. Part A 0.120 M in HBr and 0.125 M in HCHO, Express your answer to three decimal places. A 2 ? IVO AJD pH = .613 Submit Previous Answers Request Answer * Incorrect; Try Again; 4 attempts remaining Part B 0.170 M in HNO2 and 8.5x10-2 Min HNO3 Express your answer to two decimal places. IVO AQ R O 2 ? pH = 0.593 Submit Previous Answers...
B, C, and D are wrong. Please show all work. Thank you! Ka was
not provided in the info.
<Assignment 13 (Chapter 16) Problem 16.88 ③ 5 of7 Review Constants 1 Periodic Table Consider the titration of 44.0 mL of 0.270 M HF with 0.190 M NaOH. Calculate the pH at each of the following points. Part A How many milliliters of base are required to reach the equivalence point? Express your answer using three significant figures. VNaOH = 62.5...
Rank the following titrations in order of increasing pH at the equivalence point of the titration (1 = lowest pH and 5 = highest pH). 1 2 3 4 5 100.0 mL of 0.100 M HNO2 (Ka = 4.0 x 10-4) by 0.100 M NaOH 1 2 3 4 5 100.0 mL of 0.100 M HOCl (Ka = 3.5 x 10-8) by 0.100 M NaOH 1 2 3 4 5 100.0 mL of 0.100 M C2H5NH2 (Kb = 5.6 x 10-4) by 0.100...
What is the pH of the analyte in a titration at the equivalence point when a 10.00 mL aliquot of 0.25 M HF ( Ka = 3.5 x 10-4, pKa = 3.46) is titrated with 0.10 M NaOH? 8.23 8.15 7.00 5.85
Need help with Part E.
Calculate the pH after the following volumes of acid (31.0 mL)
have been added.
Will rate high is answer is correct. Thank you!
M Review Constants Periodic Table You may want to reference (Pages 729 - 739) Section 17.3 while completing this problem. pH = 2.17 A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HCIO4 solution. Calculate the pH after the following volumes of acid have been added. Submit Previous Answers...
Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. First what is the initial pH (before any NaOH is added)? The Ka for HOCI is 3.0 x 10-8 M. Need help? Hint, given in general feedback. Answer: 3.96 Make ICE table and use simplified method of successive approximations (no iterations needed). How many mL of NaOH are added to reach the equivalence point? Answer: 8 What is the pH after 3.20...
Part B What is the pH of a buffer solution containing 0.25 M H2CO3 and 0.061 MNaHCO3 ? Express your answer using two decimal places. 10 AED # O ? pH = Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining rt C Complete previous part(s)