Statement 1: Mohr titration is usually performed in an acidic medium. Statement 2: This is because under acidic conditions, the chromate ion is protonated to form chromic acid which leads to immediate precipitation at the end point. Statement 1 is incorrect and Statement 2 is correct Both statements are correct Both statements are incorrect Statement 1 is correct and Statement 2 is incorrect

Statement 1: Mohr titration is usually performed in an acidic medium. Statement 2: This is because under acidic conditions, the chromate ion is protonated to form chromic acid which leads to immediate precipitation at the end point. Statement 1 is incorrect and Statement 2 is correct Both statements are correct Both statements are incorrect Statement 1 is correct and Statement 2 is incorrect

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

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.97QE: According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as...

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The grid has six lettered boxes, each of which contains an item that may be used to answer the questions that follow. Items may be used more than once and there may be more than one correct item in response to a question. Place the letter(s) of the correct selection(s) on the appropriate line. Could dissolve Zn(OH)2 _____________ Could be used to prepare a buffer from __________ Halfway to the equivalence point in the titration of a weak, monoprotic acid with strong base ________ SO2-related atmospheric phenomenon __________ Species formed by a Lewis acid-base reaction ________ General condition required for precipitation to occur ________ [conj. base] = [conj. acid] in a buffer ___________
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
Samples containing iron(II) ion can be titrate with solutions containing dichromate ion under acidic conditions.
In the experiment, the amount of acetic acid in vinegar was determined by titrating with 0.1 M NaOH solution. In the analysis, three trials were performed to obtain more precise result. The table shows the initial and final burette readings for three titrations: Initial Burette Reading (mL) Final Burette Reading (mL) Trial 1 2.9 10.6 Trial 2 10.6 18.1 Trial 3 18.1 25.7 According to the given data, calculate molarity of acetic acid in the commercial vinegar. Please be sure that your answer includes followings; a) moles of NaOH for each trial b) average mole of NaOH c) average mole of acetic acid in 50 mL solution d) average mole of acetic acid in 250 mL solution e) molarity of acetic acid in vinegar.
Molarity of titrant (NaOH): 0.4550 M Trial # First Second Third Fourth Initial buret reading 0.15 mL 2.43 mL 1.32 mL 0.58 mL Final buret reading 18.62 mL 20.87 mL 20.03 mL 19.14 mL Volume of titrant used 18.47 mL 18.44 mL 18.71 mL 18.56 mL Write the balanced neutralization reaction that occurs when you titrate the acetic acid (HC2H3O2) with sodium hydroxide (NaOH). Hint: It’s in the background. HC2H3O2 (aq) + NaOH (aq) → NaC2H3O2 (aq) + H2O (l) Using data from all 4 titrations, calculate the average volume of standard NaOH solution required to titrate 10.00 mL of the vinegar solution (Show your work). Average volume to titrate 18.47+18.44+18.71+18.56/4= Average Volume = 18.545 mL Calculate the average number of moles of NaOH used in the titrations (show your work). Average Moles NaOH = moles Calculate or determine (give reasoning) the number of moles of acetic acid in the 10.00 mL…
Samples containing iron (II) ion can be titrated with solutions containing dichromate ion
Precipitation is the opposite of dissolution. Group of answer choices True False
A titration is used to determine the concentration of a specific substance in solution. O True O False
By reading the scientific literature, you discover that sodium dodecyl sulfate (SDS), a surfactant emitted by one of the factories, can be detected using a colorimetric method. If SDS is present in the sample, it will react with specific chemicals added to the sample and blue color will appear. What instrument could you use to measure the blue color intensity? A colorimeter A turbidity meter A scale A titrator
A student was titrating a solution of hydrazine, H₂NNH2, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. 1 NEXT 40.0 mL of a 0.200 M H₂NNH₂ solution was titrated with 80 mL of 0.100 M HNO3 (a strong acid). Fill in the ICE table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base.. Before (mol) Change (mol) After (mol) 6.00 × 10³ -6.00 × 10³ 0 Initial (M) Change (M) Equilibrium (M) 0.100 + x 0 H₂NNH₂(aq) 0.100 7.00 x 10" 0.100 - x H₂NNH3*(aq) + Question 8 of 23 2 0.100 0.200 + x 0.200 -7.00 x 10³ + 0.200 A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by…
If 0.045 g of KHP is used for titration, calculate the molarity (concentration) of the wood ash solution. Initial volume of the buret with wood ash is 5.75 mL and the final volume of wood ash after titration is 23.45 mL.
A pink solid has the formula CoCl3·5NH3·H2O. A solution of this solid is also pink in color and when titrated with silver nitrate quickly forms 3 mol of AgCl. Upon heating the pink solid, it loses 1 mole of water and forms a purple solid with the same NH3:Cl:Co ratio. Dissolving and titrating with AgNO3, the purple solid slowly releases one of its chlorides. a) Derive the formulas of the two octahedral complexes.b) draw and name them.c) write the chemical equations of all described reactions.

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		Statement 1 is incorrect and Statement 2 is correct
		Both statements are correct
		Both statements are incorrect
		Statement 1 is correct and Statement 2 is incorrect