What are the dissociation equations for acetic acid and salicylic acid?
CH3COOH---------->CH3COO- + H+ C6H4OHCOOH------>C6H4OHCOO- + H+
What is the equation for the dissociation of acetic acid ?
acetic acid: CH3COOH CH3COOH(aq) --> CH3COO−(aq) + H+(aq)
What is the dissociation reaction of acetic acid?
acids donate protons CH3COOH(Aq) + H2O(L) ===> CH3COO-(Aq) + H3O+ (Aq_
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 :)).
What is the balanced net ionic equation for the dissolution of acetic acid in water?
CH3COOH + H2O ---> (CH3COO- ) + (H3O+)
Write a equilibrium constant expression Ka for dissociation a acetic acid HC2H3O2.?
CH3COOH +H2O <=> CH3COO- +H3O+ Ka is the dissociation constant of a acid. In your case Ka= [CH3COO-]*[H3O+]/[CH3COOH] a) mole balance of acid Cs*Vs=Ca*Va Cs: concentration of solution; Vs: volume of solution; Ca:concentration of acid; Va: Volume of acid; -> Va= (Cs/Ca)*Vs= (0.4/2)*100 ml= 20 ml
Net Ionic Equations in the balanced form?
Write the balanced equations in net-ionic form for: a. The dissociation of acetic acid into its component ions in water solution; b. The reaction of acetic acid with sodium hydroxide in water solution; c. Both steps of the acid dissociation of oxalic acid in water solution; d. Both steps in the reaction of oxalic acid with sodium hydroxide in water solution.