How does concentration affect the chemical equilibrium?
The effect of concentration change can be explained by Le Chatlier's law.If the concentration of a substance is changed, the equilibrium will shift to minimise the effect of that change.If the concentration of a reactant is increased the equilibrium will shift in the direction of the reaction that uses the reactants, so that the reactant concentration decreases. The forward reaction is favoured.The forward reaction is also favoured if the concentration of the product is decreased, so that more product is formed.If the concentration of a reactant is decreased the equilibrium will shift in the direction of the reaction that produces the reactants, so that the reactant concentration increases. The reverse reaction is favoured.The reverse reaction is also favoured if the concentration of the product is increased, so that product is used.
A base is added to water. What happens when the position of equilibrium lies to the left? The base is completely dissociating into products.?
A base is added to water. What happens when the position of equilibrium lies to the left? A) The base is completely dissociating into products. B) The base is partially dissociating into products. C) The base is not dissociating into any ions. D) The base is present in very small amounts.
On what side does equilibrium lie?
equilibrium will lie to the right hand side. The ammonium ion won't give up its proton to the ethanoate ion, (that's the reverse reaction) but the ethanoic acid will give up its proton to the ammonia molecule. (that's the forward reaction) You could say that the ammonia molecule is a stronger base than the ethanoate ion.
Acid and Base chemistry question.?
A NH4+ is the ammonium ion which is acidic. As an acid it will donate a proton to the other conjugate acid/base pair in the solution leaving NH3 ( a weak base).
Chemistry: Bases and Acids question?
Hi there, so my question is, with this equation: HCOO- + H2O <---> HCOOH + OH- ... I think that the position of equilibrium would be to the right, because HCOO- is a fairly strong base, and would rip of H+ off water to create HCOOH and OH- as a result. So the position of equilibrium is to the right. Is this correct? But before you answer, I am asking because I am fairly sure that is incorrect and actually the amount of OH- should be small. Why and is this correct? Thanks
What is the reaction of acetic acid in water?
Thanks for the A2A. Unfortunately I am not able to create superscripts and subscripts here on Quora to write chemical formulae, so bear with me.So first of all, pardon me, but I am going to be picky. The real name (IUPAC) of acetic acid is Ethanoic Acid, which - in a concentration of usually around 5% - forms vinegar. Through this name we can deduce the formula of the compound: CH3COOH - two carbon atoms (eth-) including that in the carboxyl group (-oic Acid).The reaction between a soluble compound and its solvent is known as dissociation, and it is usually an equilibrium. Ethanoic Acid is a weak monoprotic acid, which means it only donates one Hydrogen ion (proton) and its dissociation thus occurs in only one step. Much simpler than diprotic acids like Sulphuric Acid (H2SO4) and triprotic acids such as Phosporic Acid (H3PO4), especially one you have to calculate the pH of the resulting solution.Back to the dissociation of Ethanoic Acid, here is the equilibrium reaction:As you can see, CH3COOH acts as a Brønsted-Lowry acid by donating a proton to water (a Brønsted-Lowry base in this instance) yielding the Hydronium ion (H3O+). Without a Hydrogen ion (note that the one that ‘left’ was from the carboxyl group and NOT the methyl substituent group), Ethanoic Acid becomes an anion and here acts as a Brønsted-Lowry base as it can accept protons from H3O+ when the equilibrium shifts to the other direction due to Le Chatelier’s Principle (but that’s another topic :)).
Help! How does the Bronsted-Lowry model explain acid strength?
Ok, I am in major need of help. I have to teach a lesson to a high school class tomorrow and chemistry is not my best subject. One of the things I have to teach them about is how the Bronsted-Lowry model explains acid strength... I just don't understand the conjugate base business and equilibrium. What does equilibrium lying to the right even mean? I don't even know what equilibrium is in this case. Specifically, I need to teach them the information in the paragraph on page 646 of this book in the section called "Acid Strength and the Bronsted-Lowry Model". If anyone could take a look at this website with the paragraph on Page 646 and explain it for me, you would be a life saver. The website contains the chapter of the book that I am teaching. http://www.gofoster.com/downloads/twe/chap18.pdf Thank you!