Ex. A sample that may contain NaOH, Na₂CO3, NaHCO3, and inert matter alone or in compatible combination is titrated with 0.1000 N HCI with phenolphthalein as the indicator and the solution became colorless after the addition of 48.8 mL. Methyl orange is then added and 14.55 mL more of the acid are needed for the color change. If the sample weighs 2.345 grams, it contains a.5.842% NaHCO3 and 6.577% Na₂CO3 b.6.577% Na2CO3 and 5.842% NaOH c. 65.77% Na₂CO3 and 5.842% NaHCO3 d. 65.77% Na₂CO3 and 5.842% NaOH
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- A 250.0mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and titrated with 0.091M NAOH , requiring 29.5ml to reach end point. Determine equivalent weight500 mL of 0.1019 M NaOH solution is preparedIt is immediately forgotten with the cap open and absorbs 0, 652 g of CO2. Calculate the relative carbonate error made in acetic acid titration with this solution with phenol-phthalate indicator.While preparing the samples for analysis, you forgot that you already added phenolphthalein indicator so you added some more. What will be its effect in the volume of the titrant needed to reach the endpoint? Select one: A. Increase B. Decrease C. No effect D. Cannot be determined Primary standards are used to determine the exact concentration of the titrant. Based on the criteria of primary standards, which of the following cannot be used as a primary standard? Select one: A.Oxalic acid B. Sodium hydroxide C. Sodium carbonate D. Potassium dichromate During titration, you notice that the retention of the faint pink color is longer than earlier. Your lab partner suggested that you add a “half-drop” to prevent over-titration of the analyte solution. Is it ethical to do the “half-drop” technique? Select one: A. NO. It will cause error in calculations if you forgot to record the volume reading before adding the half-drop. B. YES. No error in calculations will be encountered provided…
- Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided TOPIC: Standardization of Titrant Question 7 Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX __ ET TOPIC: Determination of Molar Concentration of each component (Double Indicator Titration) Question 8 No blank correction Ex ___ ET Question 9 Bubbles trapped in the tip of burette: EX ___ ET Question 10 Measuring the sample volume using a volumetric pipet while looking downwards at the meniscus: EX ___ ETplease stop rejecting. we pay for this service, so we deserve getting our answer! I do not want to have to put a claim in and report Use acid-base titration to determine theconcentration of:– A strong acid: HCl 0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOH Phenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10A 250.0-mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and titrated with 0.0663 M NaOH, requiring 35.18 mL to reach the end point. Determine the compound’s equivalent weight
- A solid 0.4550 g sample contains only barium carbonate (MW, 197.34) and sodium carbonate (MW, 105.99). 37.60 mL of 0.1500 M HCl is required in the titration of the sample using red indicator as of methyl. Find the percentage of each of the components in the solid sample.Im doing a lab for chemistry and need help answering numers 1 and 2 below using the data provided. The molar concentration of the sodium for both is .100M. For your coarse titration, record the following results. initial burette volume reading of NaOH titrant at the start (mL) 0.00 final burette volume reading of NaOH titrant before the color change (mL) 29.05 volume of NaOH solution dispensed (mL) 29.05 volume of HCl solution in the flask (mL) 5.00 1) Calculate the molar HCl concentration using your coarse titration results. For your fine titration, record the following results. initial burette volume reading of NaOH titrant at the start (mL) 0.00 burette volume reading of NaOH titrant at the color change (mL) 30.05 volume of NaOH solution dispensed (mL) 30.05 volume of HCl solution in the flask (mL) 5.00 2)Calculate the molar HCl concentration using your fine titration results.Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution. 2MnO4- + 5C2O4-2 +16H+ -> 2Mn2+ + 10CO2(g) + 8H2O Calculate the molar concentration of the KMnO4 solution. Pls show step by step. What type of molecules will interfere in this analysis ?
- How to distinguish between an Acidic Buffer and Acidic Solution as well as Basic Buffer and Basic Solution? Is it based on the color exhibited sol. w/ indicator or pH level of a solution? Ex. Solution 1: 30.0 mL 0.10 M CH3COOH Solution 2: 15.0 mL 0.20 M CH3COOH – 15.0 mL 0.20 M NaCH3COO Both used methyl orange as indicator Solution Observed Color & Estimated pH range Classification (acidic/basic & buffer/solution) 1 a 1.0 M HCl Red pH < 3.1 (2.01pH) b 1.0 M NaOH Orange 3.1 < pH < 4.5 (3.98pH) c Control Red pH < 3.1 (2.91pH) 2 a 1.0 M HCl Yellow pH > 4.5 (4.73) b 1.0 M NaOH Yellow pH > 4.5 (4.82) c Control Yellow pH > 4.5 (4.76)Double indicator titration of 1.000g powdered sample containing either alone or any compatible mixture of NaOH/Na2CO3/NaHCO3 and the rest are inert components. The sample was dissolved in 20 ml water then titrated with 0.50 M HCl and reach phenolphthalein endpoint at burette volume of 25.55 ml. Continuing titration, it reached methyl orange endpoint at burette volume of 9.45 ml. Calculate the percentage mass of the possible alkaline component/s.Why are the standard reagents used in neutralization titrations generally strong acids and bases ratherthan weak acids and bases? Explain.