Row A. B. C. D. Use the following information to answer questions 38 and 39. A Sample Titrated with HCl(aq) 14.0 Row A. B. C. D. 7.0- 38. Which of the following rows identifies the indicator that would accurately detect the equivalence point and the colour change that would indicate the endpoint? Indicator Phenol red Phenol red Volume of HCl(aq) added (mL) Chlorophenol red Chlorophenol red Colour Change Yellow to red Sample Being Titrated Aqueous ammonia Aqueous ammonia Aqueous sodium hydroxide Aqueous sodium hydroxide 102 Red to yellow Yellow to red Red to yellow 39. Which of the following rows identifies a possible sample being titrated and the number of buffer regions on the titration curve? Number of Buffer Regions 1 2 1 2

Row A. B. C. D. Use the following information to answer questions 38 and 39. A Sample Titrated with HCl(aq) 14.0 Row A. B. C. D. 7.0- 38. Which of the following rows identifies the indicator that would accurately detect the equivalence point and the colour change that would indicate the endpoint? Indicator Phenol red Phenol red Volume of HCl(aq) added (mL) Chlorophenol red Chlorophenol red Colour Change Yellow to red Sample Being Titrated Aqueous ammonia Aqueous ammonia Aqueous sodium hydroxide Aqueous sodium hydroxide 102 Red to yellow Yellow to red Red to yellow 39. Which of the following rows identifies a possible sample being titrated and the number of buffer regions on the titration curve? Number of Buffer Regions 1 2 1 2

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 107AP

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Figure 15-3 outlines the classic scheme for separating a mixture of insoluble chloride salts from one another. Explain the chemistry involved in the various steps of the figure.
please 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: 8.3-10
Define pH indicator. The amount of pH indicator added are normally kept as small aspossible in a titration process. Explain on the reason why we should not add excessive pHindicator into sample during titration.
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)
Define the end point of a titration: a) It is a synonym for equivalence point b) It is when a change that indicates equivalence is observed in the analyte solution c) It is the point at which the pH no longer changes
A suitable target for the titration is 30.0 cm3 of 0.025 moldm-3 Br2(aq) Justify why a much smaller target titre would not be appropriate Calculate the amount in moles of bromine in the target titer Justification? calculate a suitable massof alive oil to transfer to the volumetric flask using your answer to of above question and the structure of Y Assume that the olive oil contains 85/- of Y by mass (If you were unable to calculate the amount of bromine in the target titer,you should assume it is 6.25×10^-8 mol .this in not the correct amount)
1. The reaction of ??? with ???3 is presented by the unbalanced chemical reaction below: ___ KOH(aq)+ ___ HNO3 (aq) ---> ___ KNO3 (aq)+ ___ H2O(l)Calculate the molar concentration of Nitric acid (???3) when 40.5−?? of 0.674 ? ???is required to quench 101.0?? of Nitric acid over phenolphthalein indicator.
Consider the Heat of Solution Practical that was conducted. Temperature (oC) Amount of NaOH ( 0.015M) used to reach end point of titration (ml) 40 42 35 35 30 26 25 23 20 16 Use the data provided above in order to determine the heat of solution. Include any necessary graphs.
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 ___ ET
6. What do we call reagents of known concentration that is used to carry out a volumetric titration?A. standard titrateB. standard analyteC. standard titrantD. standard reagent7. What has the analyte reached when the amount of added titrant is chemically equivalent to the amount of the analyte in the sample?A. equivalence pointB. end-pointC. titration pointD. Dilution point8. In an acid-base titration, what indicator does an analytical chemist add to indicate chemical equivalence?A. bromophenol greenB. phenolphthaleinC. iodineD.methyl orange9. These are factors in the environment that causes exposure to the emission of electromagnetic waves.A. BiologicalB. ChemicalC. PhysicalD. Radiation10. What concentration unit measures the number of chemical equivalents of reagent in the same volume?A. MolalityB. FormalityC. MolarityD. Normality
which indicator is best used for the titration of aqueous ammonia and benzoic acid?
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