To make ethyl acetate, react ethanol with ethanoic acid in the presence of concentrated sulphuric acid. Another method is by preparing industrially using the Tishchenko reaction by combining two equivalents of acetaldehyde in the presence of an alkoxide catalyst.
If you drip H2SO4 into NaCl it will release HCl gas and produce Na2SO4. So set up a three neck round bottom loaded with NaCl and a stir bar (No solvent). Put a stopper into one of the necks, an addition funnel full of H2SO4 in the second and then a hose adapter on the third. Attach one end of the hose to the reaction flask and the other to the inlet of a bubbler loaded with more H2SO4 (This will dry the HCl gas). Attach a second hose to the outlet of the bubbler. This hose should lead to a needle or bubbling apparatus in a chilled flask of ethyl acetate. (The point is to bubble the HCl through the ethyl acetate) The ethyl acetate flask should also be vented because not all the HCl will dissolve.
Based on how much ethyl acetate you use you should be able to calculate the mass gained from the dissolved HCl. Using that gain in mass you can monitor concentration. So, keep bubbling until you hit 3M or go over 3M and dilute back down. In my experience, this isn't terribly efficient and will take quite a bit of NaCl and H2SO4, but it works!
synthesis, isolation and purification
Add naoh then oxidation
Loperamide(R) is soluble in ammonium acetate buffer (0.01 M, pH=5), diluted 0.001M HCl and methanol.
Anhydrous sodium acetate is added to buffer the phenylhydrazine HCl so that it may function properly. Regards mawaisnawaz@hotmail.com
g HCl solution = 2500 mL of HCl * 1 liter/1000 mL * 1190 g/L = 2975 g 37% solution (37 g HCl/100 grams of solution) gives you the grams of HCl: g HCl = 0.37 * 2975 g = 1100.8 g HCl Moles HCl = 1100.8/(36.46 g/mole) = 30.2 moles Therefore the molarity, which equals the normality in this case = 30.2 moles/2.5 L = 12.07 M = 12.07 N If you want to make 100 mL of a 0.1 N solution, Volume of HCl solution needed = (0.1 N * 100 mL) /12.07 N = 0.83 mL Take 0.83 mL of the 37% HCl, and dilute it with water to 100 mL.
To dilute it.
you can add some pieces of pure tin or tin powder in HCl . Sn (s) + 2 HCl (aq) → SnCl2 (aq) + H2 (g)
add HCl and a vinegar smell should produce
The question is in poorly worded. I will assume the question is "why adjust the pH of Tris buffer with HCl and not Sodium Acetate?" I would assume the answer is - because sodium acetate is the conjugate base of a weak acid, and HCl is a strong acid. Also the salts you would be putting into the solution as a result would be different. I think the question is actually, "The pH of Tris is adjusted with HCl, why isn't the pH of sodium acetate adjusted with HCl?". I'm not sure of the answer exactly, but I've always assumed its because if you adjust the pH with glacial acetic acid instead of HCl, you won't introduce chloride ions.
You cannot make HCL out from just Xhlorine. U will need Hydrogen to. Hcl is a Hydrochloric solution so u will need a method to combine Hydroger and chlorine in order to make HCL
If the solution is not a buffer, the HCl will react with the solution to form a product.
To convert make a dillute solution from a concentrated one, take the amount of moles needed for the final solution as mL of concetrated solution, and dillute with water until the desired volume is reached.
Add 200 mls of the 1.0N HCl solution to a 1 liter volumetric flask. Make up to the mark with water. Standardize against a known weight of Sodium Carbonate.
44.5 ml HCl TAKE AND DILUTE UP TO 1000 ML WATER MAKE A 0.5 M HCl SOLUTION
combine 100 mL 6 M HCl with 500 mL H2O
When ethyl chloride is reduced with atomic hydrogen ethane and HCl are formed, Zn + 2HCl -------> ZnCl2 + 2[H] CH3-CH2-Cl + 2[H] -----> CH3-CH3 + HCl
Find moles of HCl first. 1.56 grams HCl (1mole HCl/36.458 grams) = 0.0428 moles HCl Molarity = moles of solute/volume of solution Molarity = 0.0428 moles/26.8 ml = 0.00160 milli-Molarity, or more to the point; = 1.60 X 10^-6 Molarity of HCl
HCl is a gas. It's therefore very difficult to accurately weigh out the proper amount to use to make a solution of any given concentration, and as the solution sits, some HCl may escape as gas. In contrast, it's very easy to weigh out a solid base to high precision, and use a solution made from it to standardize the only-approximately-known HCl concentration.
when any ionizable cpmpound is dissolved in water it becomes an electrolytic solution as NaCl or HCl in water....