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Questions and Answers
What is the observation when testing for Mn2+ with NaOH?
What is the observation when testing for Mn2+ with NaOH?
Which reagent, when added to an unknown sample, produces a black precipitate confirming the presence of Co2+?
Which reagent, when added to an unknown sample, produces a black precipitate confirming the presence of Co2+?
What color precipitate indicates the presence of Ba2+ when tested with K2CrO4?
What color precipitate indicates the presence of Ba2+ when tested with K2CrO4?
What happens when Ni2+ is treated with NH4OH?
What happens when Ni2+ is treated with NH4OH?
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What is the observation for the testing of Ca2+ with K2CrO4?
What is the observation for the testing of Ca2+ with K2CrO4?
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Which test reliably confirms the presence of Zn2+?
Which test reliably confirms the presence of Zn2+?
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When testing for Co2+, what is produced when O.S. is treated with K4[Fe(CN)6]?
When testing for Co2+, what is produced when O.S. is treated with K4[Fe(CN)6]?
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Which combination of reagents will provide a black precipitate indicating Mn2+ when tested?
Which combination of reagents will provide a black precipitate indicating Mn2+ when tested?
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What occurs when acids, bases, and salts dissolve in water?
What occurs when acids, bases, and salts dissolve in water?
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Which statement accurately describes cations?
Which statement accurately describes cations?
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What principle ensures electrical neutrality in a solution of dissociated ions?
What principle ensures electrical neutrality in a solution of dissociated ions?
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What implication does the formation of cations and anions have on the charge of the solution?
What implication does the formation of cations and anions have on the charge of the solution?
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What is the result of non-metals gaining electrons during dissociation?
What is the result of non-metals gaining electrons during dissociation?
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In the context of ion formation, what do the charges of cations and anions correspond to?
In the context of ion formation, what do the charges of cations and anions correspond to?
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What would indicate that Pb2+ may be present in a qualitative analysis?
What would indicate that Pb2+ may be present in a qualitative analysis?
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What is the role of the test tube holder in laboratory procedures?
What is the role of the test tube holder in laboratory procedures?
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What observation indicates the presence of NO3- when copper fillings are added to concentrated H2SO4 and heated?
What observation indicates the presence of NO3- when copper fillings are added to concentrated H2SO4 and heated?
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In the confirmatory test for the anion, what is the significance of observing a brown ring at the junction of two solutions?
In the confirmatory test for the anion, what is the significance of observing a brown ring at the junction of two solutions?
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Which method is employed to identify the anion in Sample Solution 1?
Which method is employed to identify the anion in Sample Solution 1?
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What is an expected observation when a salt containing nitrate ions is dissolved in water?
What is an expected observation when a salt containing nitrate ions is dissolved in water?
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Which of the following salts can be expected to yield the anion identified in Sample Solution 1?
Which of the following salts can be expected to yield the anion identified in Sample Solution 1?
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When preparing the confirmatory test for nitrate ions, why is it important to add the iron(II) sulfate solution slowly?
When preparing the confirmatory test for nitrate ions, why is it important to add the iron(II) sulfate solution slowly?
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What inference can be drawn if no color change is observed with the addition of concentrated H2SO4 to the sample solution?
What inference can be drawn if no color change is observed with the addition of concentrated H2SO4 to the sample solution?
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In the confirmatory test for an anion, what is the role of freshly prepared FeSO4 solution?
In the confirmatory test for an anion, what is the role of freshly prepared FeSO4 solution?
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What percentage of the total marks is allocated for the timely submission of the report?
What percentage of the total marks is allocated for the timely submission of the report?
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Which aspect of identification contributes the most to the practical marks?
Which aspect of identification contributes the most to the practical marks?
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How are the total marks distributed between process related and product related assessments?
How are the total marks distributed between process related and product related assessments?
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Identifying the two states of matter contributes to what percentage of the practical marks?
Identifying the two states of matter contributes to what percentage of the practical marks?
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What is implied about the heat storage capacities of different forms of matter?
What is implied about the heat storage capacities of different forms of matter?
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What does the practical significance focus on regarding the states of matter?
What does the practical significance focus on regarding the states of matter?
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What is a required outcome that is expected by industry or employers regarding student performance?
What is a required outcome that is expected by industry or employers regarding student performance?
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Which statement best reflects the goals outlined for the identification of anions?
Which statement best reflects the goals outlined for the identification of anions?
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What role does the dated signature of faculty play in the assessment?
What role does the dated signature of faculty play in the assessment?
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What is the total score for practical assessments in this evaluation?
What is the total score for practical assessments in this evaluation?
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What key benefit does determining the electrode potential of a metal provide?
What key benefit does determining the electrode potential of a metal provide?
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Which of the following outcomes is expected from students in practical learning?
Which of the following outcomes is expected from students in practical learning?
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What is a critical skill that students are expected to learn related to glass wares?
What is a critical skill that students are expected to learn related to glass wares?
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Why is knowledge of metal's electrode potentials applicable in engineering?
Why is knowledge of metal's electrode potentials applicable in engineering?
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What type of meter is used to measure the electrode potential in practical learning?
What type of meter is used to measure the electrode potential in practical learning?
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What does copper's position in the electrochemical series indicate?
What does copper's position in the electrochemical series indicate?
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Which of the following is NOT mentioned as a relevant course outcome?
Which of the following is NOT mentioned as a relevant course outcome?
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What might be a consequence of not understanding electrode potentials in engineering?
What might be a consequence of not understanding electrode potentials in engineering?
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Which of these practices is directly associated with observing during practical sessions?
Which of these practices is directly associated with observing during practical sessions?
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In practical terms, what is the primary purpose of setting an electrochemical cell as part of the experiment?
In practical terms, what is the primary purpose of setting an electrochemical cell as part of the experiment?
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Study Notes
Dissolving Acids, Bases, and Salts
- When acids, bases, and salts dissolve in water, they break down into ions.
- Positively charged ions are called cations.
- Cations are formed when metal atoms lose electrons.
- Negatively charged ions are called anions.
- Anions are formed when non-metallic radicals or groups of non-metals gain electrons.
- The charges on the ions correspond to the valency of the elements.
- The total positive charge of cations equals the total negative charge of anions, resulting in a neutral solution.
Resources Required
- 6 Test tubes (15 ml each) are required for the experiment.
- A steel test tube holder with a wooden handle is required.
- A wooden test tube stand is required.
- Chemicals are needed, but the specific requirements are not stated.
- A 100 ml beaker is required.
Precautions for Experiment
- Use a test tube holder.
- Use a funnel to transfer solutions and reagents.
- Turn off the gas burners after use.
Identification of Cations
-
I Group
- Addition of dilute hydrochloric acid (HCl) to the solution creates a white precipitate. This indicates the possible presence of Pb²⁺ (lead ions).
- If no precipitate forms, add sodium dihydrogen phosphate (NaH₂PO₄). A white precipitate confirms the presence of Zn²⁺ (zinc ions).
- Addition of potassium hexacyanoferrate(II) ([Fe(CN)₆]⁴⁻) to the solution creates a white precipitate, confirming the presence of Zn²⁺.
-
Confirmatory Test (C.T.) for Mn²⁺
- Addition of sodium hydroxide (NaOH) produces a white precipitate that dissolves in excess NaOH. This confirms the presence of Mn²⁺ (manganese ions).
- Adding bromine (Br₂) to a solution containing Mn²⁺ and NaOH results in a black precipitate, confirming the presence of Mn²⁺.
- Addition of potassium hexacyanoferrate(II) to the solution creates a pinkish-white precipitate that's soluble in dilute hydrochloric acid, confirming the presence of Mn²⁺.
-
Confirmatory Test (C.T.) for Ni²⁺
- Addition of NaOH and bromine water creates a black precipitate, confirming the presence of Ni²⁺ (nickel ions).
- Addition of ammonium hydroxide (NH₄OH) results in a pale green precipitate that dissolves in an excess of NH₄OH and forms a blue solution, confirming the presence of Ni²⁺.
- Addition of dimethylglyoxime to the solution results in scarlet red precipitate, confirming the presence of Ni²⁺.
-
Confirmatory Test (C.T.) for Co²⁺
- Addition of NH₄OH creates a blue precipitate, confirming the presence of Co²⁺ (cobalt ions). The precipitate turns brown in excess NH₄OH.
- Addition of ammonium thiocyanate (NH₄CNS) results in a black precipitate, confirming the presence of Co²⁺.
- Addition of potassium hexacyanoferrate(II) forms a reddish precipitate, confirming the presence of Co²⁺.
-
Group IV Cations
-
Confirmatory Test (C.T.) for Ba²⁺
- Adding potassium chromate (K₂CrO₄) to the solution creates a yellow precipitate, confirming Ba²⁺ (barium ions).
- Adding ammonium oxalate ((NH₄)₂C₂O₄) results in a white precipitate, confirming Ba²⁺.
- Addition of dilute sulfuric acid (H₂SO₄) results in a white precipitate, confirming the presence of Ba²⁺.
-
Confirmatory Test (C.T.) for Ca²⁺
- Adding potassium chromate (K₂CrO₄) to the solution does not result in a precipitate, confirming the presence of Ca²⁺ (calcium ions).
- Adding ammonium oxalate ((NH₄)₂C₂O₄) results in a white precipitate that is insoluble in acetic acid, confirming the presence of Ca²⁺.
- Adding ammonium chloride (NH₄Cl) crystals to the solution and then mercury(I) nitrate (HgNO₃) results in a white precipitate followed by a yellow precipitate, confirming the presence of SO₄²⁻ (sulfate ions).
-
Confirmatory Test (C.T.) for Ba²⁺
Identification of Anions
-
Confirmatory Test (C.T.) for NO₃⁻
- Adding copper fillings to the solution and then concentrated sulfuric acid (H₂SO₄). Heating the mixture causes the evolution of brown fumes, leaving a blue colored solution, confirming the presence of NO₃⁻ (nitrate ions).
- Adding concentrated H₂SO₄ and a freshly prepared FeSO₄ solution (added slowly to the side of the test tube) results in the formation of a brown ring at the junction of the two solutions, confirming the presence of NO₃⁻.
Practical Significance of Electrode Potential of Copper Metal
- Determining the electrode potential of a metal helps identify its position in the electrochemical series. This series ranks metals based on their electrical behavior.
- Understanding this ranking is crucial for designing structures that utilize the principle of galvanic corrosion to protect the structure from corrosion damage.
Industry/ Employer Expected Outcomes of Electrode Potential Experiment
- Handling glassware.
- Handling reagents.
- Observation.
Practical Learning Outcomes of Electrode Potential Experiment
- Determining the electrode potential of copper metal by setting up an electrochemical cell.
- Measuring the electrode potential of copper metal using a voltmeter.
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Description
This quiz covers the concepts of acids, bases, and salts and how they dissolve in water to form cations and anions. You will learn about the formation of these ions, their charges, and the required resources for conducting a related experiment. Important safety precautions will also be addressed.
