When common hydroxide salts (i.e. those of sodium or potassium) are added 1:1 to a strong acid, $HX$, a neutralization reaction occurs to give $NaX$, or $KX$. i.e. $HX...
1 Answers 1 viewsSimply from the $K_a$, or the $"pKa"$. Or, the $K_b$, or the $"pKb"$, if comparing by dissociation in water. The higher the $K_a$ or lower the $"pKa"$, the stronger...
1 Answers 1 viewsAcidity (and we usually specify an aqueous solvent) is assessed on the basis of the completeness of the following equilibrium: $HCl(g) + H_2O(l) rightleftharpoons H_3O^(+) + Cl^-$ Hydrogen chloride is...
1 Answers 1 views.....and propose that a strong acid is a species for which the following equilibrium lies to the RIGHT as written: $HX(aq) +H_2O(l) rarr H_3O^(+) + X^-$ And further that a...
1 Answers 1 viewsSince strong acids completely dissociate in water, their conjugate bases cannot bond to a $H^+$. This is why there is not an equilibrium when strong acids are in water....
1 Answers 1 viewsIf, say, we have equimolar, say $1.0*mol*L^-1$ $HX_"i"$ and $HX_"ii"$, where $HX_"ii"$ is a weak acid, then clearly, for equivalence, we need to add equimolar quantities of strong base. There...
1 Answers 1 viewsA will take place when the hydronium cations produced by the acid in solution will react with the hydroxide anions produced by the base to form water. $"OH"_text((aq])^(-)...
1 Answers 1 viewsIt decreases the concentration of your acid solution, so you may need to swirl your solution more every now and then to ensure that the titrant is distributed throughout the...
1 Answers 1 viewsThe thing to remember about buffers is that they resist significant changes in because they convert strong acids or strong bases to weak acid or weak bases, respectively. In...
1 Answers 1 viewsQUICK ANSWER The temperature of the solution will increase by $2^@"C"$ regardless of how much strong acid and strong base you're mixing because the change of , $DeltaH_"neut"$, is...
1 Answers 1 views