Concept explainers
Interpretation:
For each of the acid-base reaction, the acid, base, conjugate acid, and conjugate base are to be identified. The equilibrium constant for each of reaction is to be calculated.
Concept introduction:
An acid is a chemical substance that readily donates protons and a base is a chemical substance that can easily accept a proton. During an acid-base reaction, the interaction between an acid and a base is taken place because of the transfer of a proton.
The equilibrium constant expression for an acid-base reaction is written as follows:
Here
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Organic Chemistry - Standalone book
- Illustrate your answer and explain your answer for better understanding.arrow_forwardThis is a Brønsted-Lowry acid-base reaction. Draw structures for all the products, showing any non-zero formal charges in each one. Make sure your reaction is balanced. Note for advanced students: Draw only the most stable resonance structure for each product. ОН c=0 КОН Click and drag to start drawing a structure. ČH, c* ?arrow_forward4. a) A polyatomic ion of formula SCN is called thiocyanate. Draw a Lewis structure for thiocyanate anion based on the total number of valence shell electrons and a connectivity S-C-N. Show your work b) Next, apply the concept of resonance to arrive at a second resonance form for the ion with formal charge on a different atom. Circle the 2 elements that are Lewis basic in this polyatomic ion. c) Based on your answers above, state which intermolecular attractive forces are important in SCN".arrow_forward
- Decide whether each of the molecules in the table below is stable, in the exact form in which it is drawn, at pH=1. If you decide at least one molecule is not stable, then redraw one of the unstable molecules in its stable form below the table. (If more than one molecule is unstable, you can pick any of them to redraw.) OH HO Ostable of Ounstable OH Ostable Ounstable Ostable Ounstable O stable Ounstable : G Π P alo.arrow_forwardThe structure of Vitamin C (ascorbic acid) is shown below. As the name indicates, the molecule is somewhat acidic. Actually, one of the hydrogens on the four OH groups is much more acidic than the other three ones. Which one is the acidic hydrogen? Hints: To find the answer, you will again have to draw some resonance structures of the product formed after loss of H+. Consider the product after the loss of H+ for each of the OH groups. Only two of the OH groups have resonance structures after deprotonation; one of these two groups has a much better resonance structure than the other one (again after deprotonation). Note that the oxygen atom that is part of the five-membered ring has nothing to do with the problem.arrow_forwardPart 2 of 2 Draw the skeletal structure of the product(s) for the Lewis acid-base reaction. Include lone pairs and formal charges (if applicable) on the structures. The Click and drag to start drawing a structure.arrow_forward
- Decide whether each of the molecules in the table below is stable, in the exact form in which it is drawn, at pH=12. If you decide at least one molecule is not stable, then redraw one of the unstable molecules in its stable form below the table. (If more than one molecule is unstable, you can pick any of them to redraw.) HO ☑ O stable OH stable Ounstable unstable OH O stable O unstable stable unstable Garrow_forwardDecide whether each of the molecules in the table below is stable, in the exact form in which it is drawn, at pH = 2. If you decide at least one molecule is not stable, then redraw one of the unstable molecules in its stable form below the table. (If more than one molecule is unstable, you can pick any of them to redraw.) OH OH Ostable Ounstable Ostable unstable Ostable Ounstable OH 15 OH Ostable Click and drag to start drawing a structure. Ounstable O '7 X 0:0 X to Sarrow_forwardPractice q # 4 4. Which nitrogen in this molecule is the most basic? Explain briefly your choice. (3) H₂N. (4) H₂N. (2) O (1) HNarrow_forward
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- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning