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Thank you for your insightful observation! The difference in preparation methods for methyl orange and phenolphthalein primarily stems from their solubility properties: Methyl orange is water-soluble, so it is initially dissolved in distilled water before ethanol is added to reach the final volume. Phenolphthalein on the other hand, is poorly soluble in water and requires alcohol as the primary solvent. Once dissolved, distilled water is added to complete the volume. As for the references used: The procedure for preparing these indicators is widely documented in standard analytical chemistry texts, such as Vogel's Textbook of Quantitative Chemical Analysis, Guidelines from ASTM standards, such as ASTM D1209-05 for chemical solutions, also provide similar details. Flinn Scientific also provides similar procedures.

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In this case, I think the problem you re experiencing is an "indicator error". Methyl orange can degrade over time or be affected by light leading to incorrect colour changes. I will advice you also double check the concentration of the acid and the base, and most importantly prepare a fresh methyl orange indicator from the methyl orange powder or purchase another methyl orange powder and prepare a fresh solution from it. Use this link below to learn how to prepare methyl orange indicator ua-cam.com/video/lKVDzocGHuU/v-deo.html

@@ChemEasy_Eko Thank you very much sir

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You are welcome. You can use any one. I used Peak powder milk

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No, you don't have to Could be a problem with your reagent or chemicals or method of preparation

@@ChemEasy_Eko i noticed it's from the indicator. I've changed it. Thanks for your response

@preciousogbonna2420 Oh! That's great. You are welcome. Success in advance

Good day I tried this titration but I didn't get the deep orange colour, the color was the same just lighter

Your methyl orange indicator might be the caused. Try preparing or using a different methyl orange indicator. Watch the video below on how to prepare methyl orange by clicking on the link ua-cam.com/video/lKVDzocGHuU/v-deo.html

If it is volume, answers should be written to 4 significant figure or 2 decimal places such as 20.43 instead of 20.4 because of systematic errors in reading an equipment. If it's any other calculations e.g involving concentration, you limit the significant figure of the final answer to the digit with the fewest significant figure. E.g assuming you want to add 23.456 + 21.1235 + 21.10 = Your final answer should have the same significant figure with the digit with the fewest significant figure (i.e 21.10) Hence, when you add the above to get 65.6795 you should approximate the final answer to 65.78. inorder words you have limited the significant figure in the final answer to the digit in your calculation with the fewest significant figure.

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For the QUALITATIVE analysis of CuSO4 and Zn(NO3)2, the ions present are 1. Cu²+ (Copper ion) 2. Zn²+ (Zinc Ion) 3. SO4²- (Sulphate ion) 4. NO3- (Nitrate ion) 1. To Qualitatively analyze copper, the reagents used are caustic soda (NaOH) and aqueous ammonia. PROCEDURE: Dissolve a small amount of copper sulfate in water. OBSERVATION: The solution will be blue, indicating the presence of Cu²⁺ ions. I. Addition of Sodium Hydroxide (NaOH):Procedure: Add a few drops of sodium hydroxide solution to the copper sulfate solution. Observation: A light blue gelatinous precipitate of copper(II) hydroxide (Cu(OH)₂) forms which is insoluble in excess Reaction: Cu²⁺ + 2OH⁻ → Cu(OH)₂ (blue precipitate) II. Addition of Ammonia (NH₃): Procedure: Add dilute ammonia solution to the copper sulfate solution dropwise. Observation: Initially, a light blue precipitate of copper(II) hydroxide forms, which dissolves upon adding excess ammonia, forming a deep blue complex [Cu(NH₃)₄]²⁺. Reaction: Cu(OH)₂ + 4NH₃ → [Cu(NH₃)₄]²⁺ + 2OH⁻ 2. To Qualitatively analyze zinc ion, the reagents used are caustic soda (NaOH) and aqueous ammonia. I. Adding caustic soda in drops give a white gelatinous precipitate, in excess the precipitate is soluble to give a clear solution II. Adding ammonia in drops give a white gelatinous precipitate which is soluble is excess to give a clear solution. 3. To Qualitatively analyze sulphate ion (SO42-), the reagents used are Barium Chloride and dilute HCl I. Make an aqueous solution of the sample. To the solution add barium Chloride, a white precipitate of barium sulphate is form II. Proceed by adding HCl, the precipitate is insoluble in dilute HCl 4. To Qualitatively analyze NO3- the reagents used are freshly prepared FeSO4 solution and concentrated H2SO4. I. Make an aqueous solution of the sample. To the solution of the sample, add few drops of freshly prepared FeSO4 solution followed by concentrated H2SO4 acid along the side of the rest tube in a slant position. A brown ring is formed just at the junction of the acid and the solution. 5. Also, you can test for nitrogen (IV) oxide gas (NO2) by placing Zn(NO3)2 salt in a boiling tube and heat strongly Observation: the salt decomposes with a crackling sound , the gas evolved is reddish brown that turns moist blue litmus paper red. Confirmatory Test with Copper Turnings and Concentrated Sulfuric Acid: Procedure: Add a few copper turnings to the zinc nitrate solution and then add concentrated sulfuric acid. Observation: Brown fumes of nitrogen dioxide (NO₂) will be released, indicating the presence of nitrate ions

It depends on your intended use. Most times I prepare 1M concentration or 0.1M concentration

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Do you mean qualitative analysis?

@@ChemEasy_Eko yes sir the qualitative analysis

Yes you can

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Amen 🙏 You are welcome

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I don't see it's relevance in this analysis as it tis used in absorbing CO2 gases, drying gases and sometimes in water purification. Anyway, if you still need the requirements I will send you a detailed procedure for it.

@@ChemEasy_Eko thank you so much, please I really need it, I will appreciate if you will send me the procedure for it.

NaOH + CaO= soda lime ..that's all

@@AbughSamsonHough how many grams for each

In 250cm3 of water

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No! The calibration of the burette typically includes the volume within the entire burette, including the tip. Therefore, any liquid remaining in the tip is part of the total volume dispensed as long as it was initially filled into the burette. You should not tap off or attempt to remove the remaining acid from the tip of the burette after the final reading. The volume that has been read from the burette scale includes the liquid in the tip as part of the burette calibration. Tapping off the remaining liquid would alter the actual volume dispensed, leading to inaccuracies in your titration result

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Thanks Sir

Hydrogen peroxide Manganese (IV) oxide Liquid soap Colourant

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Become a member of my channel and you will have access to my WhatsApp channel page where we can have one on one interaction

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God bless you sir

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Of course you can Molar mass = mass/mole Mass = 6g Mole = 0.0566mol (per dm³) Molar mass = 6g/0.0566mol Molar mass = 106g/mol

@@ChemEasy_Eko okay sir thank you

@@ChemEasy_Eko sir please there is a question I saw I don't know if I send it to you maybe it can serves as preparatory questions also

Ok send it. Reach me via this link facebook.com/governorjerry?mibextid=ZbWKwL

You re welcome Thanks!!! Definitely

10ml. But if u have 5ml measuring cylinder I ll advice you use it for more accuracy.

What if I did my titration ND d color does not changed, wat can be wrong with d titration?

So many factors could be responsible for it: 1. Check your indicator 2. Check the solutions concentration 3. Check the purity of the solution etc

Reach out to me via facebook.com/governorjerry?mibextid=ZbWKwL Thanks

Very soon. Thanks for reaching out🙏

@@ChemEasy_Eko okay sir weldone sir

1. Chemistry Alternative A is a practical examination where students perform actual laboratory experiments. This practical component typically involves using laboratory equipment and chemicals to carry out specific tasks outlined in the exam. While: 2. Chemistry Alternative B is designed for schools or candidates that may not have access to fully equipped laboratory facilities. Instead of a hands-on practical exam, Alternative B features a "practical paper" that is theoretically based. This paper often includes alternative-to-practical questions where students are tested on their understanding of practical concepts without having to perform actual experiments.

No. Calculating the number of atoms of MnO4- and the amount of moles of MnO4- are two related but distinct concepts. 1. To find the number of moles of MnO4- we use: Mole = mass/molar mass 2. To find the number of atoms, you first need to calculate the number of moles and then use Avogadro's number to convert moles to atoms Number of atoms = number of moles×6.022×10²³ atoms/mol