Question

In the example equilibrium system, a drop of methyl orange indicator was added. For this indicator, the solution will be red in high concentrations of HO+, and the solution will turn yellow in low concentrations of H,O+ Initially the equilibrium solution was orange. What color is expected after the addition of the NaC,H,O2? Explain your reasoning. a. b. Initially, the equilibrium solution was orange. What color is expected after the addition of a strong acid which donates H O+ ions? Explain your reasoning 13 Initially the equilibrium solution was orange. After heating the solution it changed to yellow-orange. Which way did the system shift? Explain your answer

HC₂H₃O₂(aq) + H₂O( $\l$ ) $\rightleftharpoons$ C₂H₃O₂^-(aq) + H₃O⁺(aq)

Answer 1

Since the solution is orange in colour it is indicating a neutral solution

Upon heating the colur of the solution changes into yellow-orange.This means the equilibrium has shifted towards left, turning less acidic or alkaline.

The reaction is exothermic. It gives off heat. If the temperature on the system were increased, the reaction would move to the left, thereby absorbing some of the heat added.

HIn + H2O = H3O⁺ + In^-

Red Yellow-Orange

HIn represents the protonated (acid) form of the methyl orange indicator, and In- represents the deprotonated (basic) form.