Q1. What is complexometric titration? Explain the reactions occurring during a complexometric titration citing the volumetric determination of nickel in a solution. (Do not write the step-by-step procedure)
Q: A student in conducting molecular weight determination of an uninown diprotic acid. He first…
A: KHP dissociates completely to form K+ and HP-. HP- then acts as weak acid. KHP and NaOH are…
Q: Titration of a 0.7513-g sample of impure NazB,07 required 30.79 mL of 0.1129 M HCI. B40,2+ 2H3O*…
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Q: A 250.0-mg sample of an organic weak acid was dissolved in an appropriate solvent and titrated with…
A: Assuming the equivalent weight of acid is E. Given : mass of acid = 250 mg = 0.25 g…
Q: A 0.5131-g sample that contains KBr (MM: 119.0023) is dissolved in 50 mL of distilled water.…
A: When we need to find the concentration of ions like Cl-, Br- of a solution by titration with silver…
Q: A 5.850-g sample containing KCl and KClO4 was dissolved in sufficient water to give 250.00 mL of…
A: Given , Reaction : 8V3+ (aq) + ClO4- (aq) + 12H2O (l)→Cl- (aq) + 8VO2+ (aq) + 8H3O+ (aq) Volume of…
Q: 7. Define back-titration. What is the concept behind this method?
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Q: 1. Titration of 0.485g sample by the Mohr method required 38.8mL of standard 0.1060 M AgNO3…
A: Given, Weight of sample= 0.485 g Concentration of AgNO3 = 0.1060 M Volume = 38.8mL = 38.8/1000 =…
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: A 4.0520g sample of hydrochloric acid, sp. Gr. 1.18, required 44.15ml of 0.9035N sodium hydroxide in…
A: Note - “Since you have posted a question with multiple sub-parts, we will solve the first three…
Q: concentration
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Q: In order to adjust the Potassium Permanganate solution, 0.0544g Na2C2O4 was taken and necessary…
A: 2 moles of potassium permanganate reacts with 5 moles of oxalate.
Q: Titration of 0.1756 g primary standard Na2C2O4 required 32.04 mL of a potassium permanganate…
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Q: Enumerate at least 2 specific medical applications of complexometric titration and discuss each.
A: This titration is used to analyse the urinary samples in medical field by calculating the presence…
Q: Calculate the pAg when 29.25 mL of 0.1140 MF is titrated with 27.00 mL of 0.1250 M AGNO3 titrant.…
A: pAg =3.14
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: A 0.2386-g sample contained only NaCI and KBr. It was dissolved in water and required 48.40 mL of…
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Q: 50.00 mL of 0.1000 M Ti2+ solution is titrated with 0.1000 M Sn4+ solution. Find the concentration…
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Q: . What do we call reagents of known concentration that is used to carry out a volumetric titration?…
A: Usually in a volumetric titration, a solution of known concentration is treated as reference. With…
Q: After solubilization, 150 mg of a silver sample is titrated with 25 mL of a solution containing 48.5…
A: Introduction: Molarity is often used to express the concentration of the solution. It is defined as…
Q: A 0. 238 g sample contained only NaCı and KBr. It was dissolved in water and required 48. 40 ml of…
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Q: 1) What is the different between volumetric titration and condumetric titration?
A: “Since you have asked multiple question, we will solve the first question for you. If you want any…
Q: Which of the following can be used to determine the turning point in a complexometric titration? A.…
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Q: 4) A series of titrations gave the following concentration (M) values: 0.517,0.528, 0.521, 0.523.…
A: Molarity is defined as “the mole of the solute per unit volume of the solution”. It is represented…
Q: Enter your answer in the provided box. Use information from a table of solubility products and a…
A: We know that Ksp for Cr(OH)3 is 6.3 × 10 -31
Q: Why are Ce4+solutions never used for the titration of reductants in basic solutions?
A: The reason why Ce4+ solutions are not used for the titration of reductants in basic solutions have…
Q: 1. How many ml of 0.30M solution of H2SO4 will react with 20ml of a 0.30M solution of NaOH?…
A: Given values: n1 = 2 M1= 0.30M V1 = ? n2= 1 V2= 20ml M2= 0.30M n1, M1 and V1 are the…
Q: if a 1.25g sample of magnesium oxide (98.9%) were titrated with 70ml of 1.04N of sulfuric acid, what…
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Q: In water analysis using back-titration technique, 1) What are the names of the anions that form…
A: 1. Chloride (Cl-) and sulfate (SO42-) are the anions that form water-insoluble salt with Ag (aq). 2.…
Q: 1. What is the role of chromate ions in chloride determination? 2. Why pH range is important in…
A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: A 0.2386-g sample contained only NaCI and KBr. It was dissolved in water and required 48.40 mL of…
A: Given data, Mass = 0.2386 g 48.40 mL of 0.04837M AgNO3 for complete titration Calculating the weight…
Q: The Zn in a 0.6185 g sample of foot powder was titrated with 23.74 mL of 0.01485 M EDTA. Calculate…
A: In a complexometric titration a complex is formed .Here metal ion are estimated with the help of…
Q: 25.00 mL of a sample containing Hg2²+ was titrated with 0.05789 M of KIO3, requiring 35.69 mL to…
A: In this question we have to calculate the concentration of Hg22+ in the sample.
Q: 100.0 cm3 water is titrated with 0.0049 M ascorbic acid solution. What is the analytical…
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Q: Complexometric titrations are particularly useful for the determination of a mixture of different…
A: titration in which the formation of colored complex formed when complexing agent that is EDTA…
Q: C Complexometric Titration
A: One of the main problems in laboratory soil analysis is the selection of the determination system of…
Q: A 492-mg sample containing KH2PO4 (136.09 g/mol) is titrated with 0.112 M NaOH requiring 25.60 mL.…
A: Number of moles of NaOH should be calculated to determine the moles of KH2PO4 . Number of moles =…
Q: What is the calculated equivalence point volume when 21.2 mL of 0.250M HI are titrated with 0.350M…
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Q: A 5.30 mLmL sample of an H3PO4H3PO4 solution of unknown concentration is titrated with a 1.050×10−2…
A: Solution: We have balanced reaction for given titration is: 3NaOH + H3PO4→ Na3PO4 +3H2O. Therefore,…
Q: What volume of 0.317 M KOH solution will be required to titrate 25.00 ml of 0.285 MHNO3?
A: Recall the reaction between KOH and HNO3 KOH+HNO3→KNO3+H2O As basicity of HNO3 is 1 we can…
Q: 9. A 0.2700 g of impure Na₂CO3 required 24.12 ml Of 0.1684 M HCl and a back titration with 2.96 ml…
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Q: What is the acid/base ratio? Why is it important in the titrimetric process?
A: Acid base ratio is the exact amount of acid and base required to obtain a desired pH. This value can…
Q: A 370.00 mL solution of 0.00185 M A3B4 is added to a 390.00 mL solution of 0.00100 M C3D4. What is…
A: Assuming the salts A3B4 and C3D4 are soluble in water completely as no information is given about…
Q: Complexometric titration must be performed at pH 10.0
A: Complexometric Titration is basically a type of volumetric titration where a colored complex is…
Q: The excess K2Cr207 was back-titrated with 8.53 ml of 0.00949 M Fe2* şolution. Calculate the molar…
A: Answer is 1.12×10-²M
Q: 2. A 0.5131-g sample containing KBr is dissolved in 50 mL distilled water. Titrating with 0.04614 M…
A: Given Mass of sample = 0.5131 g Dissolved in 50ml of water M (AgNO3) = 0.04614 Volume = 25.13 ml At…
Q: 0.316 grams of a sample containing chloride is taken and treated with an excess of 48.5 mL of 0.11 M…
A: Here we are required to find the percentage of chloride present in the sample
Q: A 25 ml of an HCIO4 solution was titrated with 0.1032 M NaOH solution, 28.06 ml was added in excess,…
A: When the concentration of the hydrogen ion (H+) is increased in an aqueous solution by a substance,…
Q: A 0.4263 g solid sample containing NaCl and KBr only was dissolved in 50 mL of water and titrated to…
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Q: Identify the differences between a primary and secondary standard in titration process? state…
A: Titration: it is common laboratory method of quantitative chemical analysis to determine the…
Q: Acidimetric titrant can be: H,SO4 solution; KOH solution; H;PO4 solution; CH;COOH solution;
A: Acidimetric titration are also known as acid base titration, in which concentration of base find out…
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- In complexation volumetry, classify the statements below as true or false.Justify the one(s) that you judge to be “false”.a) When preparing an EDTA solution, to be used as a titrant of Ca2+ ions, it is necessary to add a small amount of Mg2+ in the solution.b) A metallochromic (Ind) indicator is a substance that forms colored complexes with metallic ions. The colors of these complexes are always the same as the colors of the free forms of these indicators.c) In order for the titration of a metal (Me) with EDTA to be carried out, it is necessary that the Me-EDTA complex has a stability constant greater than that of the Me-Ind complex.d) In determining the partial hardness of a hard water sample with EDTA solution, murexide is used as an indicator at pH 10.You are given a table of [CN-] standard solutions of different concentration. A 25 mL aliquot of each standard solution was added with Fe(NO3)3 to form a colored complex[Fe(CN)6]3-(aq). Each standard solution was then diluted to a total volume of50.0 mL. [CN–] prior to dilution, M [CN-] final M 0 0 0.04 0.1 0.16 0.24 0.32 0.4 What are the new concentrations for the standard solutions? Please show solutions.What is the basis of the ‘40000’ in the equation? Note: this is about "DETERMINATION OF WATER HARDNESS BY EDTA TITRATION"
- Write all the reactions involved in the Mohr's method, if an unknown solution containing chloride ions is titrated against silver nitrate solution. Suggest an indicator and what is its colourin the unknown chloride solution ? and Why is KSCN solution used as burette solution and not in conical flask in Volhard's method?Chloride in a brine solution is determined by the Volhard method. A 10.00 mL aliquot of the solution is treated with 15.00 mL standard 0.1182 M AgNO3 solution. The excess silver is titrated with standard 0.1010 M KCNS solution, requiring 2.38 mL to reach the endpoint. Calculate the concentration of chloride in g NaCl/liter.1. Titration of 0.485g sample by the Mohr method required 38.8mL of standard 0.1060 M AgNO3 solution. Calculate the percentage of chloride in the sample.
- Which of the following statements about the indicators used in Edta titrations is false?A. The strength of the complex made with the metal ion should be less than the complex of the same metal with EDTA.B. Metal indicators are used to determine the turning point in complexometric titrations.C. They should form water-soluble colored chelate complexes with metals.D. The complex formation constant of the complex made with metal ions must be very low.Which of the following statements is true regarding permanganimetry? a) Permanganate solution can oxidize water which is catalyzed by the presence of manganese dioxide or manganese ion. b) The light pink endpoint color for permanganimetry tends to fade with time due to the catalytic reaction. c) Standardization of the permanganate titrant is carried out at elevated temperature with sodium oxalate. d) all of these e) none of theseChromel is an alloy composed of nickel, iron and chromium.A 0.6472 g sample was dissolved and diluted to 250 mL. When a50 mL aliquot of 0.05182 M EDTA was mixed with an equal volumeof the diluted sample and all the three ions were chelated, a 5.11 mLback titration with 0.06241 M copper (II) was required.The chromium in a second 50 mL aliquot was masked through theaddition of hexamethylenetetramine, titration of the Fe and Nirequired 36.28 mL of 0.05182 M EDTA.Iron and chromium were masked with pyrophosphate in a third50 mL aliquot and the nickel was titrated with 25.91 mL of theEDTA solution.Calculate the percentage of nickel, chromium and iron in thealloy.
- After solubilization, 150 mg of a silver sample is titrated with 25 mL of a solution containing 48.5 mg KCNS in 10 mL in the presence of Fe3+. Calculate the purity of Ag in the sample.Chloride in a brine solution is determined using Volhard method. A 10.00 mL aliquot of the solution is treated with 25.00 mL standard 0.1182 M AgNO3 solution. The excess silver is titrated with standard 0.1010 M KSCN solution, requiring 12.38 mL to reach the red Fe(SCN)2+ end point. Identify the (a) indicator (b) end point color (c) molarity of the Cl- in sample.Which of the following causes the sharpest change in the equivalence point of a complexometric titration? A. Increasing the concentration of the EDTA solution B. Decreased concentration of the analyte C. Increasing the concentration of the EDTA solution D. Increasing the stability of the [metal-EDTA] complex
