nat the purpose of the indicator is I the culculated value of the molarity of the NaOH solution be too high or too low hanged if the following errora were made? Explain your answeni. - beaker into which the student poured the NaOH solution from the fumo hood i some distilled water in it flask into which the student weighed the KHP wus wet

nat the purpose of the indicator is I the culculated value of the molarity of the NaOH solution be too high or too low hanged if the following errora were made? Explain your answeni. - beaker into which the student poured the NaOH solution from the fumo hood i some distilled water in it flask into which the student weighed the KHP wus wet

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.93QE

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This is about determinition of acid content in vinegar through titration, please answer the questions. Please answer only the items nummber 4-5. i only put other questions for guide. 1. What is the purpose of standardization? 2. What is the primary standard used (name and formula)? ANS: KHP 3. Suppose that the KHP is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be higher, lower, or unaffected? Explain. 4. In preparing the buret for titration the final rinse is with the NaOH titrant rather than with distilled water. Explain. 5. The procedure suggests the addition of only 2 drops of phenolphthalein. What will be the effect to the analysis if larger amount of phenolphthalein is added?
A student prepares a weak acid solution by dissolving 0.2400 g HZ to give 100. mL solution. The titration requires 30.0 mL of 0.1025 M NaOH. Calculate the molar mass of the acid. (a) Would the molar mass be too high, too low, or unaffected if the student accidentally used 0.1400 g in the calculation? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated (b) Would the molar mass be too high, too low, or unaffected if the student accidentally used 20.0 mL instead of 30.0 mL? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated
2 A student conducted an acid-base titration but neglected to condition the burette properly. As a result, the student began the titration but the stem of the burette was not filled with titrant. How will this error impact the experimental molarity determined from the titration data? Specifically discuss the effect on the measured values used to calculate the experimental molarity
Pls help me answer the following: The 2 options for each are buret or erylenmeyer Match the following reagents to their location in the titration apparatus.... Analyte ["",""] Titrant ["", ""] Indicator ["", ""] Solution of known concentration ["", ""] Solution of unknown concentration ["", ""]
Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3
d) please see attached question concentration KOH=20.8325mL pH solution=2.9 beginning of the titration, Vbase = 0.00 mL
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
1. Calculate the moles of KHP you titrated for each trial. (KHP is KHC8H4O4). MW = 204.23 g/mol. Determine the number of moles of NaOH required to neutralizw the KHP. Use the mole-mole ratio provided inthe balanced equation. Place answers in data table 2(second picture format) 2. Calculate the volume, in mililiters, of NaOH used to neutralize the KHP. Convert to Liters. Place answers in data table 2. 3. Calculate the molarity of the NaOH solution in units of moles/liter. Place answers in data table 2.
Q2 (a) Compare between redox titration and Acid-base titration. (b) A 0.12 N HNO3 solution is titrated with potassium hydroxide. 20 ml ofunknown KOH solution consume 15 ml of above HNO3. Calculateamount of KOH present in the solution in terms of g/lit. (c) Identify any three requirements of primary standard and give suitablejustification for the above selected points.
When 20.00 ml of sulfuric acid of unknown concentration is titrated with 0.1249 M NaOH, 32.50 ml of titrant are needed to reach the end point. What is the molarity of the sulfuric acid? Please give calculator answer and sig fig anwser
For an acid-base titration, the moles of the acid should be equal the moles of the base. 30 mL of aliquot of a 0.23N HCl is placed in an Erlenmeyer flask and 2 drops of phenolphthalein was added. It was titrated and had an intial reading of 15.8 The normality of the solution is found to be 0.52N. (a) How much of the NaOH solution is used for the titration? (b) What is the final reading on the buret?
One of your classmates (or you, perhaps!) forgot to add phenolphthalein indicator before starting the titration, and he/she already began adding sodium hydroxide from the buret! Uh oh...what should be done? a) Just restart. The trial is completely ruined. b) Add a couple drops of phenolphthalein into the acid flask. If it remains clear, nothing's wrong. If it changes to dark pink, record the final buret reading and call it a successful trial. c) Add a couple drops of phenolphthalein into the buret to turn the sodium hydroxide solution dark pink. That will really make your instructor happy.......right? d) Add a couple drops of phenolphthalein into the acid flask. If it remains clear, nothing's wrong. If it changes to dark pink, I guess you need to restart! e) Add a couple drops of phenolphthalein into the acid flask just for the heck of it. You need to restart anyways, but why not have some fun?