We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
CH2CN-5 3. (Solubility). Explain why the following observation takes place about the Nicotine. (5 pts) Solubility...
C. Explain about solubility of an amino acid when subjected to an acidic media and basic media. Indicate the compound which would be at the isoelectric point. (Draw a diagram to help explain) c. Explain about the solubility of and amino acid when subjected to an acidic media and basic media. Indicate the compound which would be at the isoelectric point. (Draw a diagram to help explain). (3 marks) Amino acids are the building blocks of proteins, acidic amino acids...
Explain why benzocaine precipitates out of solution when a pH of 8 is achieved? Hint: It might be easier to approach this question from the other point of view - why is the benzocaine soluble in water before a pH of 8 is achieved? As part of the answer to this question, you must show me how benzocaine looks at an acidic pH and explain the relevance of this structure. In the box provided, draw what benzocaine looks like at...
1.) Explain why I, is insoluble in water, but soluble in CCI: (5 pts) 2.) The partial pressure of carbon dioxide inside a bottle of cola is 4.0 atm at 25°C. What is the solubility of CO,? The Henry's law constant for CO, in water is 3.3 x 10 mol/L(atm) at 25 °C. (5 pts)
place the following compounds in order of increasing their solubility in water and explain your ordering : nitric oxide, propane, butane, 1-propanol, 1-butanol.
Could you explain why C is the correct answer 13. (3 pts) Of the following compounds, which is the most acidic? A)
Please explain Solubility Equilibria and the Solubility Product Constant. Below you will find key questions. 1. Know that the solubility product constant, Ksp, defines the equilibrium constant for the dissolution of an ionic compound into its constituent ions. 2. Calculate the molar solubility of an ionic compound in pure water using the Ksp expression and an ICE table. 3. Know that the solubility of an ionic compound is lower in a solution containing a common ion than in pure water....
B. Solubility Equilibrium; Finding a Value for Ksp 2. Explain why PbCl 2 did not precipitate immediately on addition of HCl. What conditions must be met by [Pb2 + ] and [Cl- ] if PbCl 2 is to form? 3. Explain your observations in Steps 3 (The amount of precipitate begins to decrease as it dissolves in the hot water.) and 4 (The precipitate reappears, forming after the test tube was put in ice water.) of the procedure. In which...
3. (Solubility and equilibrium) Explain the following changes in equilibrium observedin experiments. The explanation must consider all compounds and all of major factors. (5 pts) NaCl CH3CI CH3ONA CH3ОCH3 + in water: nearly 100% yield in hexane: nearly 0 % yield
3. (Solubility and equilibrium) Explain the following changes in equilibrium observedin experiments. The explanation must consider all compounds and all of major factors. (5 pts) CH3CI + CH3ONa CH3OCH3 Naci in water: nearly 100% yield in hexane: nearly 0% yield
Question 1 3.03 pts Assuming the following reaction takes place in an acidic solution, write a balanced equation for the overall reaction. Fe2+ + CrO2-Fe3+ + Crº 8H+2Fe2+ + CrO422Fe+++4H20 OSH* +3Fe2+ + CrO 2 + 3Fe3++C++ 4H20 2Fe2+ CrO42- 2Fe3+ + Cr3+ + 4H20