Precipitation Titration (Argentimetry) All of the following is true regarding Argetometric titration method except: a) The method can be used for determination of Br and I b) AgNO, is the titrant and it is not a primary standard c) In Fajan's method excess amount of AgNO, is added then back titrated with Thiocyanate d) Different methods can be used for detecting the end point e) Fajan's method depends on using fluorescence indicators such as Dichlorofluorescine Experiment 4: Precipitation Titration (Argentimetry)All of the following is true regarding Argetometric titration methodexcept:a) The method can be used for determination of Br and Ib) AgNO, is the titrant and it is not a primary standardc) In Fajan's method excess amount of AgNO, is added then backtitrated with Thiocyanated) Different methods can be used for detecting the end pointe) Fajan's method depends on using fluorescence indicators such asDichlorofluorescine

Argentometric titration method The correct statements are-- a) The method can be used for…

Precipitation Titration (Argentimetry) All of the following is true regarding Argetometric titration method except: a) The method can be used for determination of Br and I b) AgNO, is the titrant and it is not a primary standard c) In Fajan's method excess amount of AgNO, is added then back titrated with Thiocyanate d) Different methods can be used for detecting the end point e) Fajan's method depends on using fluorescence indicators such as Dichlorofluorescine

Precipitation Titration (Argentimetry) All of the following is true regarding Argetometric titration method except: a) The method can be used for determination of Br and I b) AgNO, is the titrant and it is not a primary standard c) In Fajan's method excess amount of AgNO, is added then back titrated with Thiocyanate d) Different methods can be used for detecting the end point e) Fajan's method depends on using fluorescence indicators such as Dichlorofluorescine

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 10P

See similar textbooks

Similar questions

1.Given that the solubility products (Ksp) of silver chloride(AgCl),silver iodide(AgI) and silver bromide (AgBr) are 1.82×10^-10,1×10-16,5.2×10^-13 and 1.82×10^-10 respectively.Plot an arbitrary titration curve of pAg versus volume of AgNO3 for each of the above on the same set of axis.You may assume that the concentration and volume of starting materials the same. 2.Using the information above,predict the order in which each species would precipitate from first to last
CrO42- can be used as an indicator when Br- is titrated with Ag+. What concentration of CrO42- should be used so that Ag2CrO4(s) just starts to form at the equivalence point? If a concentration of 0.0010 M CrO42- is used instead, at what concentration of Br- will Ag2CrO(s) just start to precipitate? Do you think this is likely to introduce significant error? The Ksp for Ag2CrO4(s) is 1.2x10-12.
PART 2: A solution is prepared by mixing 150.0 mL of 0.0010 M magnesium nitrate and 250.0 mL of 0.100 M sodium fluoride (Ksp = 7.4x10-11). Is Ksp greater than , equal to, or lower than Qsp? Will a precipitate form, Y/N? What is the fluoride ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3). What is the magnesium ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3).
A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed fourtrials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22 g/mol) as standard to determine the exact concentration of the NaOHtitrant. The results of the student are summarized in the table below:Note: The stoichiometric relationship of KHP to NaOH is 1:1Standardization Trial 1 Trial 2 Trial 3 Trial 4KHP Mass, g 0.5033 0.5066 0.6989 0.6843Volume NaOH used, mL 24.32 25.61 24.67 24.56After the standardization, the student weighed different amounts of the unknown acid. In a similar fashion, the student performed acid-base titrationusing phenolphthalein as indicator. The results of the molecular weight determination are summarized below:Note: The stoichiometric relationship of Unknown acid to NaOH is 1:2Molecular WeightDeterminationTrial 1 Trial 2 Trial 3 Trial 4Unknown Mass, g 0.1234 0.1034 0.1178 0.1322Volume NaOH used, mL…
A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed fourtrials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22 g/mol) as standard to determine the exact concentration of the NaOHtitrant. The results of the student are summarized in the table below:Note: The stoichiometric relationship of KHP to NaOH is 1:1Standardization Trial 1 Trial 2 Trial 3 Trial 4KHP Mass, g 0.5033 0.5066 0.6989 0.6843Volume NaOH used, mL 24.32 25.61 24.67 24.56After the standardization, the student weighed different amounts of the unknown acid. In a similar fashion, the student performed acid-base titrationusing phenolphthalein as indicator. The results of the molecular weight determination are summarized below:Note: The stoichiometric relationship of Unknown acid to NaOH is 1:2Molecular WeightDeterminationTrial 1 Trial 2 Trial 3 Trial 4Unknown Mass, g 0.1234 0.1034 0.1178 0.1322Volume NaOH used, mL…
A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed fourtrials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22 g/mol) as standard to determine the exact concentration of the NaOHtitrant. The results of the student are summarized in the table below:Note: The stoichiometric relationship of KHP to NaOH is 1:1Standardization Trial 1 Trial 2 Trial 3 Trial 4KHP Mass, g 0.5033 0.5066 0.6989 0.6843Volume NaOH used, mL 24.32 25.61 24.67 24.56After the standardization, the student weighed different amounts of the unknown acid. In a similar fashion, the student performed acid-base titrationusing phenolphthalein as indicator. The results of the molecular weight determination are summarized below:Note: The stoichiometric relationship of Unknown acid to NaOH is 1:2Molecular WeightDeterminationTrial 1 Trial 2 Trial 3 Trial 4Unknown Mass, g 0.1234 0.1034 0.1178 0.1322Volume NaOH used, mL…
11. A 0.485 g sample containing chloride was titrated with 36.8 mL of 0.1060 M AgNO3 stock solution. Express the results of this analysis in:a) Percent by weight of Clb) Weight percent Cl2c) Percent by weight of CaCl2d) Weight percent of AlC13
pls complete the table using given dataEffect of Common Ions on the Solubility of Ca(OH)21. Add Ca(OH)2 to 250.0 mL of 0.010 M CaCl2 with stirring until equilibrium is achieved.2. Filter the undissolved precipitate. Measure out 50.0 mL of the filtrate in a 250-mL Erlenmeyer flask. 3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved. 4. Record the volume of HCl solution used. Perform two more trials.
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…
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 ?
You are going to analyze a substance with the following structure. What method will be best used? CHOICES: a. Neutralization b. Direct EDTA Titration c. Indirect and Residual d. EDTA Titration e. Residual Titration Precipitation
Question:- We performed a titration with EDTA to determine the presence of Calcium in a limestone sample. We used a calcium carbonate standard to standardize the EDTA. Calmagite was used as the indicator and 1.5 g of MgCl2 was added to the EDTA to allow the indicator to function. Wouldn't this addition of magnesium to the titrant cause the end point volume to be too high? Please explain.