1. Interpret the hydrochloric acid addition change in terms of the methyl orange indicator and indicator...
1. Interpret the hydrochloric acid addition change in terms of the methyl orange indicator and indicator ion equilibria and the Le Chatelier principle.
Interpret the sodium hydroxide addition change in terms of the methyl orange indicator and indicator ion equilibria and the Le Chatelier principle
Would you predict more color change would come if HCl or HC2H3O2 were added to the indicator?
Homework Answers
In
acidic medium, methyl orange Is red in color. In basic medium, it
is yellow in color.
According to Lechatelier's principle, any change in factors at equilibrium will shift the equilibrium in that direction where it's effect get reduced.
When HCl is added, equilibrium will shift in that direction where it get reduced. Thus, equilibrium shift downward (see above pic.) and color become red.
When NaOH is added, equilibrium will shift upward and color become yellow.
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1. Interpret the hydrochloric acid addition change in terms of
the methyl orange indicator and indicator...
The equilibrium between the methyl orange indicator and indicator ion can be expressed in the following...
The equilibrium between the methyl orange indicator and indicator ion can be expressed in the following reaction: (CH3)2NHC6H4N=NC6H4SO3 +H2O (CH3)2NC6H4N=NC6H4SO3- + H3O+ Methyl Orange ((CH3)2NHC6H4N=NC6H4SO3 ) is red while the indicator ion ((CH3)2NC6H4N=NC6H4SO3-) is yellow-orange Describe the color changes on the addition of: HCl NaOH Interpret the hydrochloric acid addition change in terms of the methyl orange indicator and indicator ion equilibria and the Le Chatelier principle Interpret the sodium hydroxide addition change in terms of the methyl orange indicator...
First distilled water was added to a test tube. Then methyl orange indicator was added. The...
First distilled water was added to a test tube. Then methyl
orange indicator was added. The HCl and NaOH.
Part 1B: Acid/Base Indicator Equilibrium Chemical Reaction involved Initial color of the solution: 1. Adding HCI: a. Color change b. Equilibrium shifting 2. Adding NaOH: a. Color change b. Equilibrium shifting
Adding acetate ion produces a change in the color of the indicator. Watch Video-le where a...
Adding acetate ion produces a change in the color of the indicator. Watch Video-le where a drop of methyl orange is added to each of two 3-mL samples of 0.1 M CH3COOH (acetic acid). The 1 M Na CH3COO (sodium acetate) is added a few drops at a time (with mixing) to one of the samples. The effect on the dissociation of acetic acid that is produced by adding sodium acetate is called the common ion effect. Specify the color...
1. Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the...
1. Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMO(aq) = H(aq) + MO"(aq) red yellow If methyl orange is added to distilled water, the solution turns yellow. If a drop or two of 6 M HCl is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH the color reverts to yellow a. Why does adding 6 M HCl to...
In a titration using methyl orange as an indicator 25.0 cm of a solution of 0.1...
In a titration using methyl orange as an indicator 25.0 cm of a solution of 0.1 M sodium hydroxide reacted with 25.0 cm of 0.1 M phosphoric acid, H3PO4, solution. If the experiment is repeated using phenolphthalein in place of the methyl orange as the indicator the volume of the sodium hydroxide used to cause the indicator to change colour is 50.0 cm'. This is because phenolphthalein changes colour when a different number of hydrogen ions in the acid have...
2. Explain the effect upon the equilibrium, if any, for each of the substances added (sodium...
2. Explain the effect upon the equilibrium, if any, for each of the substances added (sodium acetate, sodium hydroxide and hydrochloric acid). If you believe that the addition effects the position of the equilibrium, indicate whether the equilibrium shifts toward reactants or products and why. Adding sodium acetate: Adding sodium hydroxide: Adding hydrochloric acid: Data: Observation Test solution Initial Acetic acid + methyl orange А Acetic Acid + methyl orange + first NaC,H,O2 Acetic Acid + methyl orange + second...
HC2H3O2(aq) + H2O() C2H3O2-(aq) + H3O+(aq) In the example equilibrium system, a drop of methyl orange...
HC2H3O2(aq) +
H2O()
C2H3O2-(aq) +
H3O+(aq)
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...
QUESTION 1 6 points Save Answer The purpose of an indicator in an acid-base titration is...
QUESTION 1 6 points Save Answer The purpose of an indicator in an acid-base titration is to indicate the of the titration. Use Table 10.2 for the following question. If an acidic solution is titrated with a basic solution and methyl violet is used as an indicator, the solution color will change from to QUESTION 2 3 points Save Answer The molarity of a solution prepared by dissolving 17.0 g of hydrochloric acid (HCI (aq) in 133 mL of water...
An impure sample of lime weighing 0.150g was reacted with 50.00cm3 of 0.8mol/L hydrochloric acid. After...
An impure sample of lime weighing 0.150g was reacted with 50.00cm3 of 0.8mol/L hydrochloric acid. After the reaction was complete the solution was transferred to a 250cm3 volumetric flask and made up to the mark with distilled water. A 25.00cm3 portion of this solution was then titrated against 0.25mol/L sodium hydroxide using methyl orange as the indicator. A 15.00cm3 volume of the sodium hydroxide was consumed. Calculate the percentage purity of lime sample. Unbalanced equations are as follows; CaCO3(s) +...
For Activity 2: Observations and Interpretations CH,COOH(aq) C CHCOO (aq) + 1) What was the color...
For Activity 2: Observations and Interpretations CH,COOH(aq) C CHCOO (aq) + 1) What was the color of the solution after adding the drop of methyl orange indicator red indicator showing high (H+] 2) What color did you observe after adding the sodium acetate, CH,COONa? it went on orange: indicator housing less 3) Assume that the dynamic equilibrium represented in the equation given above is present in the original solution you placed in the test tube. Based on LeChatelier's Principle, as...
First distilled water was added to a test tube. Then methyl
orange indicator was added. The HCl and NaOH.
Part 1B: Acid/Base Indicator Equilibrium Chemical Reaction involved Initial color of the solution: 1. Adding HCI: a. Color change b. Equilibrium shifting 2. Adding NaOH: a. Color change b. Equilibrium shifting
Adding acetate ion produces a change in the color of the indicator. Watch Video-le where a drop of methyl orange is added to each of two 3-mL samples of 0.1 M CH3COOH (acetic acid). The 1 M Na CH3COO (sodium acetate) is added a few drops at a time (with mixing) to one of the samples. The effect on the dissociation of acetic acid that is produced by adding sodium acetate is called the common ion effect. Specify the color...
1. Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMO(aq) = H(aq) + MO"(aq) red yellow If methyl orange is added to distilled water, the solution turns yellow. If a drop or two of 6 M HCl is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH the color reverts to yellow a. Why does adding 6 M HCl to...
In a titration using methyl orange as an indicator 25.0 cm of a solution of 0.1 M sodium hydroxide reacted with 25.0 cm of 0.1 M phosphoric acid, H3PO4, solution. If the experiment is repeated using phenolphthalein in place of the methyl orange as the indicator the volume of the sodium hydroxide used to cause the indicator to change colour is 50.0 cm'. This is because phenolphthalein changes colour when a different number of hydrogen ions in the acid have...
2. Explain the effect upon the equilibrium, if any, for each of the substances added (sodium acetate, sodium hydroxide and hydrochloric acid). If you believe that the addition effects the position of the equilibrium, indicate whether the equilibrium shifts toward reactants or products and why. Adding sodium acetate: Adding sodium hydroxide: Adding hydrochloric acid: Data: Observation Test solution Initial Acetic acid + methyl orange А Acetic Acid + methyl orange + first NaC,H,O2 Acetic Acid + methyl orange + second...
HC2H3O2(aq) +
H2O()
C2H3O2-(aq) +
H3O+(aq)
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...
QUESTION 1 6 points Save Answer The purpose of an indicator in an acid-base titration is to indicate the of the titration. Use Table 10.2 for the following question. If an acidic solution is titrated with a basic solution and methyl violet is used as an indicator, the solution color will change from to QUESTION 2 3 points Save Answer The molarity of a solution prepared by dissolving 17.0 g of hydrochloric acid (HCI (aq) in 133 mL of water...
For Activity 2: Observations and Interpretations CH,COOH(aq) C CHCOO (aq) + 1) What was the color of the solution after adding the drop of methyl orange indicator red indicator showing high (H+] 2) What color did you observe after adding the sodium acetate, CH,COONa? it went on orange: indicator housing less 3) Assume that the dynamic equilibrium represented in the equation given above is present in the original solution you placed in the test tube. Based on LeChatelier's Principle, as...
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