Which of the following steps MUST be done prior to titration of an analyte? I. Prepare a standardized solution II. Wash the burette with a standardized solution III. Fill the burette to the 50-mL mark IV. Prepare a contrast paper to determine burette volume and titration endpoint O I, Il and IV only O I, III and IV only O II, III and IV only 1, II, and III only

Which of the following steps MUST be done prior to titration of an analyte? I. Prepare a standardized solution II. Wash the burette with a standardized solution III. Fill the burette to the 50-mL mark IV. Prepare a contrast paper to determine burette volume and titration endpoint O I, Il and IV only O I, III and IV only O II, III and IV only 1, II, and III only

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.43QAP

See similar textbooks

Similar questions

A 1.8M HCl solution was standardized against 1.4g sodium carbonate Na2CO3 (MW = 106g/mol) . The Na2CO3 standard required 13.5 mL of the HCl solution to completely react up to the indicator endpoint. Two chemists prepared their samples by taking 12.0-mL aliquots of each household ammonia solution and diluting it to 25.0 mL. With the same titrant and indicator, Chemist #1’s ammonia solution required 15 mL of the standardized titrant, whereas, Chemist #2's ammonia solution required 35 mL of the same titrant. Write the balanced equation for the analyte and the titrant Solve for the exact concentration of the HCl titrant in molarity. What are the respective concentrations of ammonia of Chemist #1's sample and Chemist #2's samples in Molarity?
A 1.8M HCl solution was standardized against 1.4g sodium carbonate Na2CO3 (MW = 106g/mol) . The Na2CO3 standard required 13.5 mL of the HCl solution to completely react up to the indicator endpoint. Two chemists prepared their samples by taking 12.0-mL aliquots of each household ammonia solution and diluting it to 25.0 mL. With the same titrant and indicator, Chemist #1’s ammonia solution required 15 mL of the standardized titrant, whereas, Chemist #2's ammonia solution required 35 mL of the same titrant. Write the balanced equation for the analyte and the titrant Solve for the exact concentration of the HCl titrant in molarity.
Which of the following steps MUST be done prior to titration of an analyte? I. Prepare a standardized solution II. Wash the burette with a standardized solution III. Fill the burette to the 50-mL mark IV. Prepare a contrast paper to determine burette volume and titration endpoint
0.5 M of stock solution is given to be used for Titrant 1. Titrant 2 is going to be created by diluting 0.5 M stock solution to 0.1 M. How much stock solution (volume) will be needed to create 25 mL of the 0.1 M Titrant solution.
For titration, what is the purpose of a dropwise rate?
A serum sample of 3mL is analyzed for nitrogen by modified Kjeldahl. The sample is digested, distilled, and 14mL of standard of HCl is needed to titrate the ammonium borate. The HCl was standardized using 0.30g (NH4)2SO4. 30mL acid was required in titrating for standardization. What is the concentration of nitrogen in the serum (weight/volume)?
We want to make 400 ml of 1 d running buffer from the 20x stock , you will add ——-ml Of 20c stock to ——- ml water
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
True or False Titration that are not feasible in aqueous solvent can be feasible in non-aqueous solvents.
A 5.50 mL sample of an H3PO4H3PO4 solution of unknown concentration is titrated with a 1.050×10−2 MNaOH solution. A volume of 7.32 mL of the NaOH solution was required to reach the equivalence point. What is the concentration of the unknown H3PO4H3PO4 solution? Express your answer with the appropriate units. value/units
Define the term. Titration Error:
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?