13. Anhydrous sodium carbonate is used as the primary standard to determine the exact concentration a the HCI titrant. Which of the following IS NOT a desirable property of a primary standard? O hygroscopic easily weighed chemical purity of greater than 99+% does not decompose or gain weight under normal atmospheric conditions
Q: Look at Figure 2.17. If you did this titration using TRIS instead of phosphate, how would the…
A:
Q: of the following statements is incorrect O A standard solution should react completely with the…
A: Incorrect statement is:
Q: Given the following data for the titration of chromate ion with silver ion, write the titration…
A: Since we only answer up to 3 subparts, we'll answer the first 3. Please resubmit the question and…
Q: What is the correct order of performing EDTA titration? I. Titrate milk sample aliquot with standard…
A: Steps for performing EDTA titration Weighing Preparation of standard solution Standardization of…
Q: Use a spreadsheet to generate a titration curve for 10.0 mL of 0.100 M Cro titrated with 0.100 M Ag*…
A:
Q: One of the following statements is incorrect: O A standard solution should react completely with the…
A: The solution is given below -
Q: 0,0585g Na2C2O4 10 mL 'to adjust KMnO4 solution prepared as 0,1M distilled water, 2 M H2SO4 was…
A:
Q: 12Electrodes of the first kind have poor precision The answer is either true or false 16Voltammetry…
A:
Q: One of the following statements is incorrect: O A primary standard should be highly pure, has…
A: Introduction: Primary standards are the compounds that are generally used to determine the unknown…
Q: next question The following evidence was obtained during the titration of chromium (1) nitrate with…
A: Write the expression to find the unknown values from known values. M1V1=M2V2 where M1 and M2 are the…
Q: A colorimetric titration was carried out to determine the amount of ascorbic acid in a 15.00 mL…
A: When potassium iodate in presence of iodide ions forms the redox titration with ascorbic…
Q: All of the following regarding Argentometric titration are correct except: a. Chromate indicator is…
A: All of the following regarding Argentometric titration are correct except:a. Chromate indicator is…
Q: All of the following regarding Argentometric titration are correct except: a. Chromate indicator is…
A: Argentometric titration :
Q: A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask.…
A: On reaction with sulphuric acid, urea produces ammonia. One mole of urea produces one mole of urea.…
Q: How many mL of 0.1200 M KSCN will be needed in the back titration after addition of 30 mL 0.110 M…
A: Given that - Molarity of KSCN = 0.1200 M Molarity of AgNO3 = 0.110 M Volume of AgNO3 = 30 mL…
Q: 5. A 300.0 mg sample containing Na¿CO3, NaHCO, and NaOH and inert material either alone or in some…
A:
Q: A limestone sample weighing 400 mg was dissolved in acid treated with excess sodium oxalate. The…
A:
Q: Determine the % w/w chloride in the sample. A 0.3285 g sample containing chloride and inert…
A: The % w/w chloride in the sample has to be given, Given : The mass of the solute is 0.3285 g. The…
Q: Calculate the % w/w Cl– (35.45 g/mol) in the sample. Provide your answer to 2 places after the…
A:
Q: A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask.…
A: When Urea reacts with sulphuric acid then ammonia is produced. Now this ammonia is treated with…
Q: All of the following regarding Argentometric titration are correct except a. Chromate indicator is…
A: fajan method An adsorption indicator shows two different colour in adsorbed or desorbed from is…
Q: From the following data, find the % (w/w) cream of tartar (KHC4H406. MM=188): Wt of sample = 1.4160…
A: Tartar (KHC4H4O6; MM=188) is a mono protic acid.
Q: A solution containing Mg2+ was buffered to pH 9.97 and titrated with EDTA. Eriochrome black T, with…
A: Eriochrome black T is a diprotic acid, represented as H2E.
Q: Calculate the concentration of the Na2S2O3.
A: Given, Mass of primary standard KIO3 0.1238 g Volume of sodium thiosulfate (Na2S2O3) = 41.27 mL =…
Q: Before you proceed with the titration proper, you must first determine the exact concentration of…
A: In general before titration we first determine the exact concentration of titrant it against a…
Q: B. Titration Data A 100 mL Kool-Aid solution was made: 0.3210 g of Kool-Aid powder was…
A:
Q: One of the following statements is incorrect: O Titration error is the difference between…
A: Out of the given statements , one statement is wrong . We have to select that incorrect statement.
Q: Q2// (A) Calculate the number of meq. involved in a titration that required 15.4 ml of 0.3N KMNO4…
A: Given data; a) Normality of KMnO4 = 0.3 N ; Volume of KMnO4 = 15.4 mL b) Total Volume of EDTA added…
Q: A 10 mL of a chloride sample was treated with 15 mL of 0.1182 M AgNO3 The excess silver was titrated…
A: Given: The volume of AgNO3 = 15 mL = 15 x 10-3L The molarity of AgNO3 = 0.1182 M The volume of SCN-…
Q: 10mL of a 10% by weight MgCl2 solution (density = 1.1 g / mL) is precipitated as magnesium ammonium…
A:
Q: Which of the following statements does NOT explain why KHP is a suitable primary standard in an…
A: KHP is a suitable primary standard in an acid-base titration. Here we have to find out the…
Q: For the complexometric titration of Ca (II) ions in the shell of the egg sample weighing 59.427 g,…
A: Molar ratio in which calcium ions bind EDTA is 1:1
Q: A 1.067g sample of magnesium oxide of 84.736% were treated with 50mL of 1.017 N Sulfuric Acid, and a…
A: Given: mass of MgO = 1.067 g Volume of H2SO4 = 50 mL Normality of H2SO4 = 1.017 N Volume of NaOH =…
Q: A 0.574-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the…
A: Given data: Molarity of AgNO3 = 0.28 M Volume of AgNO3 = 26.21 mL Molarity of KSCN = 0.122 M Volume…
Q: 25.0 mL aliquots of acidified tin(II) iodide are titrated with 0.396 mol/L of potassium dichromate.…
A: Working formula: volume*Molarity = no of mmol the balanced chemical reaction is as follows: 2…
Q: A 0.4482 g sample of impure NaCN is titrated with 0.1018 M AgNO3 requiring 39.68 mL to reach the end…
A: The reaction is, NaCN + AgNO3 ---> AgCN + NaNO3 From the reaction, we can conclude that 1 mol of…
Q: 23A 0.20 g sample of primary standard Na2C204 (134 g/mol) needed 37.22 mL of of KMNO4 solution to…
A: 1) Mass of Na2C2O4 = 0.2g Molar mass of Na2C2O4 = 134g/mol Volume of KMnO4 = 37.22ml Molarity of…
Q: A 20 mL solution containing both Ca2+ and Mg2+ cations is diluted in to 100 mL. When 10 mL of this…
A:
Q: Standard Sodium Chloride Weighed mass of NaCl g in 250.0 mL Purity of NaCl = 100.03 % Molar…
A: Concentration of solution refers to amount of solute present in a given amount of solution or…
Q: pls ans. asap The titration reaction: 2Ce4+ + 3I- ⇌ 2Ce3+ + I3- is an example of: a.…
A: In iodometric titration , Iodide ion is reacted with oxidizing agent
Q: 9.6 ml of a standard NaOH was consumed in the titration of 5.0 mL CH3COOH sample. Calculate for the…
A: Given: 1.0 mL of NaOH is equivalent to 0.1071 g of KHP. Volume of NaOH solution required = 9.6 mL.…
Q: 1.What the difference between primary and secondary standard substances? 2.Calculate the volume of…
A:
Q: Repeats of 12.64 mL samples of a 0.2937 M primary standard zinc ion solution were titrated with an…
A: Given that - Volume of standard zinc ion Solution = 12.64 mL Molarity of standard zinc ion…
Q: Silver nitrate can be standardized using primary standard KCl. A dried sample of analytical grade…
A: When Titration between potassium Chloride and silver nitrate take place, then Following balanced…
Q: A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask.…
A: Given information, Mass of sample = 1.0 g Molarity/Concentration of HCl = 0.0500 M Volume of HCl =…
Q: Titration of 0.2121 g of primary standard Na, C,04 (133.999 g/mol) required 21.66 mL of KMnO4…
A: Given balanced equation of reaction of Na2C2O4 with KMnO4: 2 MnO4- + 5 C2O42- + 16 H+ → 2 Mn2+ + 10…
Q: As a chemist, you know that when analyzing a 50-ml sample for total hardness, every milliliter (1.00…
A: General chemistry
Q: 5.00 mL aqueous sample containing hydrogen peroxide was diluted to 25 mL and analyzed by titration…
A: The balanced Chemical equation for Titration between permanganate ions and Hydrogen peroxide in…
Q: For the complexometric titration of Ca (II) ions in the shell of the egg sample weighing 59.427 g,…
A: At first we will determine the concentration of Ca2+ in the given 100mL solution. Then we'll extend…
Q: Sulfur containing compound weighing 4.8670 grams was digested and purified to form H,SO4. A 25.00-mL…
A: Moles = Molarity * Volume (L) Mass = Moles * Molar mass
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
- All of the following criteria must be met for a titrimetric analysis to be feasible EXCEPT: Select one: a. Reaction between the standard and analyte must be known. b. There should be a substance for endpoint detection c. Reaction must proceed quantitatively to completion. d. Reaction between the reactants must be slow.A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCl, evaporated to incipient dryness, and quantitatively transferred to a 250 mL volumetric flask and diluted to mark. A 10 mL of aliquot was then transferred to an Erlenmeyer flask, together with 5mL buffer and 5 drops of EBT indicator, and was used to standardize the EDTA titrant. The solution turned blue after the addition of 24.10 mL of EDTA. A blank correction was made and was determined to be 0.4 mL. [Analysis] A 30 mL unknown water sample was treated with 37.6 mL of EDTA. A blank correction was made and was determined to be 0.4 mL. What is the concentration of Ca2+ (40.0780 g/mol) in ppm?A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCl, evaporated to incipient dryness and quantitatively transferred to a 250 mL volumetric flask, and diluted to mark. A 10 mL of aliquot was then transferred to an Erlenmeyer flask, together with 5mL buffer and 5 drops of EBT indicator, and was used to standardize the EDTA titrant. The solution turned blue after the addition of 24.10 mL of EDTA. A blank correction was performed and was determined to be 0.4 mL. What is the concentration of EDTA obtained (MW CaCO3 = 100.0869 g/mol)?
- In the Assay of Sodium Chloride, what is the purpose of adding nitric acid in the solution? It is used to prevent precipitation of silver as carbonate It is used to hasten chemical reaction It is used to precipitate silver bromide It is used to form a film over silver nitrate precipitate What is the permanent color expected at the end point in the standardization of 0.1 N Ammonium Thiocyanate? * Orange red Blue Red Yellow In the Standardization of 0.1 N Silver Nitrate, what is the purpose of allowing the mixture to stand in the dark? * It is used to aid in the formation of precipitate with large particles It is used to prevent the production of free silver It is used to acquire a purplish color in the precipitate It is used to maximize the reduction of silver chloride In the standardization of 0.1 N Silver Nitrate, what is the most suitable temperature to dry the Silver Chloride precipitate to constant weight? * 115° C 110° C 100° C 120° C Which is NOT…As a chemist, you know that when analyzing a 50-ml sample for total hardness, every milliliter (1.00 mL) of EDTA titrant removes an equivalent of 20 ppm CaCO3. What would be the total hardness of a sample if a total of 24.57 mL titrant was used? Based on the preceding question, if 0.25 mL was used in the blank titration to achieve the same end-point color, what will be the correct total hardness of the sample?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 Determination of water hardness using complexometric titration. During sample analysis (ppm CaCO3), the volume for blank correction was not subtracted to the volume of titrant. EX Blank 1 ET
- List the advantages and disadvantages of a potentiometric titration relative to a direct potentiometricmeasurement.A 0.1093-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back-titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the endpoint. Report the purity of the Na2CO3 sample. [Ans. 90.9 % (w /w )]1. These are balances that have a maximum loading of 10 to 30 g with a precision of 60.01 mgA. semi-microanalyticalB. MicroanalyticalC. MacrobalancesD. Triple Beam Balance2. Which type of curve is normally produced when plotting the change in the concentration of a specie of some function and the amount of reagent added?A. Titration curveB. Sigmoidal CurveC. Phase Transition curveD. Calibration curve3. In the dead dear case study, silver diethyldithiocarbamateforms a colored solution when it binds with arsenic, what do we call substance like silver diethyldithiocarbamate?A. Secondary standard reagentB. Precipitating agentC. Chelating agentD. Primary standard reagent
- A piece of Gold weighing 12,359 Kg is suspected of being contaminated with Iron. To perform an instrumental analysis and To confirm whether or not it contains Fe, a portion of the sample (0.954 g) is taken from the piece and dissolved with 25 mL of aqua regia. Heats up For its complete dissolution, it is cooled and made up to 100 mL. A 10 mL aliquot is taken from this solution and made up to 50 mL. From This last solution is given the appropriate treatment to visualize Fe+2, for which the 1,10-phenanthroline reagent is added. (it forms a complex that is red in color) and is taken to a visible spectrophotometer and with a 12 mm cell a absorbance of 0.45. Previously, a calibration curve of Fe+2 was obtained under the same instrumental conditions obtaining the following data: (view table) Calculate the purity of the gold piece, assuming impurities only due to Fe.10mL of a 10% by weight MgCl2 solution (density = 1.1 g / mL) is precipitated as magnesium ammonium phosphate after necessary processes, filtered and washed. The precipitate is dissolved in 50mL 1M HCl and excess acid is titrated with 2.0M NaOH solution in the presence of methyl orange. Find the NaOH consumption (Mg = 24,3g / mol, Cl = 35,5g / mol)The Kjeldahl procedure was used to analyze 244 µL of a solution containing 38.1 mg protein/mL. The liberated NH3 was collected in 5.00 mL of 0.0375 M HCl and the remaining acid required 5.98 mL of 0.00998 M NaOH for complete titration. What is the weight percent of nitrogen in the protein?