Write a one or two paragraphs of -what was study in Introduction to Equilibrium Le Chateliers Principle -Summarize what happened in these results shown below -what results did this experiment end up with whether this lab was successful or not Reaction 1 K₂CrO₄ (yellow), NaOH (colorless) HCl (colorless)   The solution changed from yellow (chromate, CrO4²⁻) to orange (dichromate, Cr2O7²⁻) as the equilibrium shifts. Added NaOH to shift the equilibrium back toward chromate ions. - Orange to Yellow Reaction 2 HCl (colorless) AgNO3 (colorless) CoCl2 (Pink (when hydrated) or blue (when dehydrated)) CoCl2 in the presence of Cl⁻ ions: Formed a blue complex, CoCl42- The addition of water dissolved the AgCl precipitate (to some extent) and hydrated CoCl42-, turning the solution back to pink (Co(H2O)62+​). Blue (from CoCl42-) to Pink (from Co(H2O)6​). Reaction 3 NH4Cl saturated (colorless) HCl (colorless) NH4Cl solid (white crystalline solid) The solution remained colorless, with the possible formation of more solid NH4Cl Dilution with water can redissolve the precipitated NH4Cl by reducing the concentration of chloride ions. No visible color change, but the solid NH₄Cl would dissolve. Reaction 4 NaOH (colorless) HCl (colorless) Methyl Orange (Orange in neutral solutions)     Mixing NaOH with HCl while using methyl orange has led to a transition from yellow to red as the pH becomes acidic Added NaOH to a solution that was red due to methyl orange in acidic conditions will shift it back toward yellow as the pH becomes more basic. Red to Yellow. Reaction 1 for shifting: 0.1 M K2CrO4 (potassium chromate), 1 M NaOH, and 3 M HCl Adding NaOH: NaOH provides OH⁻ ions, which react with the H⁺ ions: OH−+H+ → H2​O This decreases the concentration of H⁺ ions, causing a shift to the left to produce more H⁺ ions and increase the concentration of CrO₄²⁻. The formation of chromate ions leads to a yellow color. Adding HCl: HCl dissociates into H⁺ and Cl⁻ ions. The increase in H⁺ ions shifts the equilibrium to the right to reduce the H⁺ concentration, forming more Cr₂O₇²⁻ ions, which causes a color change to orange due to the formation of dichromate ion

Reaction 1

K₂CrO₄ (yellow),

NaOH (colorless)

HCl (colorless)

  The solution changed from yellow (chromate, CrO₄²⁻) to orange (dichromate, Cr₂O₇²⁻) as the equilibrium shifts.

Added NaOH to shift the equilibrium back toward chromate ions.

^-

Orange to Yellow

Reaction 2

HCl (colorless)

AgNO₃ (colorless)

CoCl₂ (Pink (when hydrated) or blue (when dehydrated))

CoCl₂ in the presence of Cl⁻ ions: Formed a blue complex, CoCl₄^2-

The addition of water dissolved the AgCl precipitate (to some extent) and hydrated CoCl₄^2-, turning the solution back to pink (Co(H₂O)₆²⁺​).

Blue (from CoCl₄^2-) to Pink (from Co(H₂O)₆​).

Reaction 3

NH₄Cl saturated (colorless)

HCl (colorless)

NH₄Cl solid (white crystalline solid)

The solution remained colorless, with the possible formation of more solid NH₄Cl

Dilution with water can redissolve the precipitated NH₄Cl by reducing the concentration of chloride ions.

No visible color change, but the solid NH₄Cl would dissolve.

Reaction 4

NaOH (colorless)

HCl (colorless)

Methyl Orange (Orange in neutral solutions)

Mixing NaOH with HCl while using methyl orange has led to a transition from yellow to red as the pH becomes acidic

Added NaOH to a solution that was red due to methyl orange in acidic conditions will shift it back toward yellow as the pH becomes more basic.

Red to Yellow.