What is the pH of a 0.050 M solution of formic acid?Assume that you have two unlabeled bottles, one of which contains phenol (pKa = 9.9)and one of which contains acetic acid (pKa = 4.76). In light of your answer to previoussuggest a simple way to determine what is in each bottle.problem

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What is the pH of a 0.050 M solution of formic acid?

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter4: Polar Bonds, Polar Reactions

Section: Chapter Questions

Problem 28CTQ: For the previous four questions, label each molecule that appears in the question or your answer...

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What is the pH of a 0.050 M solution of formic acid?
Assume that you have two unlabeled bottles, one of which contains phenol (pKa = 9.9)
and one of which contains acetic acid (pKa = 4.76). In light of your answer to previous
suggest a simple way to determine what is in each bottle.
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Complete the equation for the reaction between each Lewis acid-base pair. In each equation, label which starting material is the Lewis acid and which is the Lewis base; use curved arrows to show the flow of electrons in each reaction. In doing this problem, it is essential that you show valence electrons for all atoms participating in each reaction. (a) (b) (c) (d)
The following are equivalent ways of asking about the acidity of an H atom: • What is the most acidic H on the molecule? • Which H is associated with the published pKa value? • Which H on the molecule is easiest to remove? • Which H on the molecule takes the least energy to remove? • Which bond to an H is most polarized? • For which H atom is removal least uphill in energy? • Which bond to an H atom, when broken, results in the lowest PE conjugate base? We will often find the last of these questions is easiest to answer. To do this, find all the different Hatoms on the molecule, and draw all possible conjugate bases.Only the lowest-energy one is the “real” conjugate base. Identify this structure, and you have found the most acidic H. Use this strategy to find the most acidic H on each of the following molecules. Note: Each structure hasat least three different kinds of H’s, so draw at least three unique conjugate bases for each.
If the K, of weak base H₂X is 7.12x10, then calculate the K, of H₂X. Answer: Check If the K, of weak acid HX is 5.60x10, then calculate the K, of X. Answer: Check
Give correct detailed Solution with explanation needed..don't give Handwritten answer..give correct answer
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e) Use the equation to determine what ratio of concentrations of ethanoic acid to sodium ethanoate is required to achieve a pH of 5.0 (Ka for ethanoic acid = 1.7 x 10-5) [base] = - log Ka – log [acid] [PH]
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Describe a molecule that can be a Lewis acid. Answer:
Name Turn in this page with your assignment. Where appropriate, you must show your work in order to receive credit for working a problem. Write the answer in the space provided. You may show your work on the back or attach pages with your work. 1) Which of the following is NOT a conjugate acid-base pair? A) H2SO3/HSO3- CNH4+/NH3 2) Of the following acids,, is a weak acid? A) Chloric Acid B) H₂504/5042- D) C2H3O2-/HC2H3O2 2) 1) B) Sulfuric Acid C) HF D) HNO3 E) HI 3) What is the pH of a 0.0065 M HClO4 solution? A) 0.0065 B) 0.013 3) C) 2.19 D) 11.81 4) Determine the [H+] in a 0.755 M HCIO solution. The Ka of HCIO is 2.9 × 10-8. 5) The pH of 0.45 M Vivianic Acid, HVi is 2.65. What is the value of Ka for HVi? A) 2.2 × 10-3 B) 1.1 x 10-5 6) What is the pOH of a 0.0030 M Sr(OH)2 solution? A) 11.48 B) 2.52 C) 2.65 4) 5) D) 4.4 x 10-1 6) C) 11.78 D) 2.22 r24 1
As we will see in later chapters, many steps in key reaction sequences involve acid–base reactions. (a) Draw curved arrows to illustrate the flow of electrons in steps [1]–[3]. (b) Identify the base and its conjugate acid in step [1]. (c) Identify the acid and its conjugate base in step [3].
Give correct answer please (don't use Ai for answering this) explain each point...I will give you upvote