25ml AgNo3 react with 5mM NaCl 35 ml of (AgNo3) silver solution is required to titrate sample of ZnCl2 How many mill mole of ZnCl2 are present in the sample
Q: A sample of vinegar is to be analyzed for its acetic acid content. A volume of 50.0 mL is measured…
A: The volume of 1000.0 mL is equal to 1.0 L. The number of moles of NaOH or OH- in the 31.66 mL of…
Q: The molarity of an EDTA solution is 0.0114 M. A 25.0 mL sample of water with unknown Ca+2…
A: Molarity is number of moles of solute present in 1 liter of solution. Mass of substance = molar mass…
Q: 1) 25 mL Ag Nos of (AgNos ) silver Selution is required to titrate react witth 5mM Nacl; 35 ml…
A: Silver nitrate solution required = 35 mL Millimoles of NaCl required = 5 mM
Q: 0.4723-g sample of primary-standard-grade Na2CO3 required 34.78 mL of an H2SO4 solution to reach the…
A: Given information: Mass of sample = 0.4723 g Volume = 34.78 mL
Q: A solution was prepared by dissolving 5.76 g of KCI MgCl2.6H2O (277.85 g/mol) in sufficient water to…
A: Mass of solute = 5.76 g Molar mass of solute = 277.85 g/mol Volume of solution = 2.000 L We need…
Q: A 30.00 ml sample of sulfuric acid is titrated to the endpoint with a 0.1000 M lithium hydroxide…
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Q: Lläi 4 If 20mL of a 0.40M Mg(OH)2 solution is used to titrate 25mL of HCI solution, * ? the molarity…
A: The chemical reaction for this will be Mg(OH)2 + 2HCl - - - - - - - > 2H2O+ Mgcl2 According to…
Q: A Ba(OH)2 solution is standardized against potassium hydrogen phthalate (KHP). The titration of…
A: Given: Mass of KHP used = 0.5781 g. Volume of Ba(OH)2 required = 30.50 mL = 0.03050 L…
Q: Given the following data during the potentiometric titration of 75.00 mL unknown NaCl solution by…
A: Given Data:
Q: A Ba(OH)2 solution was standardized against potassium hydrogen phthalate (KHP). The titration of…
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Q: What volume of 0.2 M AGNO3 is required to react exactly with 120.0 mL of 0.3 M Na,SO4 solution?…
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Q: You want to analyze a cadmium nitrate solution. What massof NaOH is needed to precipitate the Cd2+…
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Q: What mass of NaCl is needed to precipitate all the silver ions from 20.0 mL of 0.100 M AgNO3…
A: We know the reaction, Ag+ + Cl- ---------> AgCl AgCl is precipitated product. One mole of Ag+…
Q: What volume of 0.200 M NaOH solution will react with 50.0 mL of 0.200 M Al(NO3)3
A: Concept is based on Molarity.
Q: O 8 https://online.vitalsource.com/reader/books/9781792484490/pageid/77 4. In a titration of KOH…
A: Given, Potassium hydrogen phthalate (KHP) Chemical formula of Potassium hydrogen phthalate : C8H5KO4…
Q: A 15.00 mL sample of a solution of H2SO4 of unknown concentration was titrated with .3200 N NaOH.…
A: The balanced reaction H2SO4 + 2NaOH = Na2SO4 + 2H2O Mass of NaOH = Normality x equivalent weight x…
Q: 12.5mL
A: We wil use neutralisation concept
Q: Calculate the grams of Acetic Acid ( M. W. 60.05g/ mole) in a unknown sample. A sample of Acetic…
A: Molarity of a solution is used to express the concentration of the solution. It can be calculated by…
Q: The reaction of KOH with HNO2 is presented by the unbalanced chemical reaction below: ___ KOH(aq)+…
A: In the given reaction by balancing reaction and equating number of moles we can find molar…
Q: An actacide tablet containing Mg(OH)2 (MM=58.3 g/mol) is titrated with a 0.100 M solution of HNO3.…
A: Given : concentration of HNO3 used = 0.100 M volume of HNO3 used = 20.00 mL = 0.020 L…
Q: A student titrates 25.00mL of H3PO4 with 0.0987 M KOH. She uses 54.06 mL to complete the chemical…
A: C1V1=C2V2 Expression is used.
Q: Titration of the I2 (254 g/mol) produced from 0.1142 g of primary-standard KIO3 (214 g/mol) required…
A: Titration is a laboratory method where the volume of a solution of known concentration is used to…
Q: How many mL of 0.105 M AgNO3 are needed for an experiment that requires 0.00510 mol of AgNO3?
A: Molarity is the number of moles of solute present in one litre solution.
Q: 35.0 mL sample of 0.225 M HBr was titration with 42.3 mL of KOH. What is the concentration of the…
A: First we write the balanced equation between HBr and KOH. This is given as; KOH (aq) + HBr (aq) →…
Q: A stock standard concentration of 101.25ppm was prepared of Cu. What are the actual concentrations…
A: The formula used to prepare working solution from the stock solution is: M1V1=M2V2 Here, M1=initial…
Q: 17.72 Suppose that a 10-mL sample of a solution is to be tested for I ion by addition of 1 drop (0.2…
A: 1) Calculate the concentration of Pb2+ of Pb(NO3)2 in the mixture of solution. 2)As PbI2 is a…
Q: Suppose that a 10-mLmL sample of a solution is to be tested for Cl−Cl− ion by addition of 1 drop…
A:
Q: What volume of a 0.0225 solution of potassium permanganate are required to titration 0.461 g sample…
A: The concentration of potassium permanganate (KMnO4), M = 0.0225 M Given mass of sodium oxalate…
Q: Q4) Name of the technique that is used for Standardization of sodiums bydroxide solution is a)…
A: acid-base titration It is an acid-base titration. The sodium hydroxide is an alkali whose…
Q: How many liters of pure water will be required to disslove 0.885g of solid lead iodate, if the water…
A: First the moles of Pb(IO3)2 present in given grams is calculated as below,Water already contains…
Q: 50.00 mL of a solution containing 0.080 M H2SO4, and 0.20 M KIO3 Calculate the mass of potassium…
A: Given Molarity of KIO3 solution = 0.20 mol/L Volume of Solution = 50 mL…
Q: Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000157 mol…
A: Given that: Number of moles of KIO3 added = 0.0000157 mol Volume of Na2S2O3 solution at endpoint =…
Q: Titration of the 12 (254 g/mol) produced from 0.1142 g of primary-standard KIO3 (214 g/mol) required…
A: The given information is: Mass of KIO3 = 0.1142 g Volume of Na2S2O3 = 27.95 ml Molar mass of KIO3 =…
Q: Calculate the concentration of all ions present in each of the following solutions ofstrong…
A: Since you have posted multiple sub-parts, the answer for first three sub-parts are given below.…
Q: A student mixes 100.0mL of .500 M AgNO3 with 25.3g CaCl2. What is the concentrations of Ag, NO3,…
A: Given: 1) Volume of AgNO3 is (V) =100.0 mL 2) Concentration of AgNO3 is (M) = 0.500 M 3) Mass of…
Q: 1) 25 (AgNoz ) silver Solution is required to titrate Sample o ZnClz How many millimole o mL Ag Nos…
A:
Q: On a separate piece of paper, complete the following calculations. A 50.0 mL sample of ocean water…
A: AgNO3 reacts with Cl- ions present in the water according to the equation: AgNO3+Cl-→AgCl+NO3- So, 1…
Q: balanced equation for the neutralization reaction of aqueous H₂SO4 with aqueous KOH is shown.…
A: Given Reaction :- H2SO4 + 2KOH -----> K2SO4 + 2H2O Molarity of KOH = 0.220M Molarity of H2SO4 =…
Q: b) A 60.00 ml of a sample of river water was titrated with 0.0016 M of sodium dichromate and I…
A: The volume of the sample = 60 mL Molarity of dichromate = 0.0016 M Volume of dichromate =…
Q: it took 32.47 mL of 0.123M NaOH to reach the endpoint when titrating a sample containg 0.2372g of…
A: Since the acid is given as triprotic hence the moles of NaOH required to reach the endpoint = moles…
Q: 1) 25 mL Ag No3 react with 5mM Nacl; 35 mk of (AgNoz ) silver Solution is required to titrate Sample…
A: 3.5 millimoles of ZnCl2 is present in the sample
Q: 45.32 mL of 0.1046 M AgNO3 is spent in Fajans titration of 0.7908 gram sample. So which of the…
A:
Q: A 350 ml phosphate buffer solution contains 0.84 mg NaH2PO4 and 2.48 mg Na2HPO4, respectively.…
A: Given : Volume of buffer solution = 350 ml Mass of Na2HPO4 = 2.48 mg Mass of NaH2PO4 = 0.84 mg…
Q: A 26.05mL of HNO3 reacts with 32.24 mL of 0.076M Ba(OH)2. Calculate the molar concentration of the…
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Q: A 0.205 g sample of a monoprotic acid was dissolved in 25 mL of water. The acid solution was…
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Q: 5.00 mL of acetic acid required 37.28 mL of 0.0999 M NaOH to be neutralized in a titration.…
A: Volume of acetic acid= 5 ml Volume of NaOH= 37.28ml Concentration of NaOH=0.0999M
Q: 5. A student used 23.21 mL of titrant to reach the endpoint of a titration of 0.2000 g sample of…
A: Given ,volume of titrant = 23.21 mLmass of sample = 0.2000 gVolume of titrantmass of sample =…
Q: A 19.56-mL of potassium permanganate solution is required to titrate 25.0 mL of 0.04637 M sodium…
A: Given: 2MnO4-+5H2C2O4+6H+→2Mn2++10CO2+8H2O Volume of MnO4- is 19.56 mL Volume of sodium oxalate is…
Q: How many miles of Na2S will be required to completely react with 40.0 mL of .200 M Fe(NO3)3
A: The reaction between Na2S and Fe(NO3)3 is as follows,
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- calculate the mass of Sn when 50 mL of a sample containing Sn2+ is titrated with 42.00 mL of 0.0150M MnO4- to reach endpoint0.2219 g of pure iron wire was dissolved in acid nd iron reduced to+2 state. Then the solution required 34 65ml of cerium(4) in a titration . Calculate molar concentration of ce4+???The arsenic in a 1.22-g sample of a pesticide was converted toAsO43- by suitable chemical treatment. It was then titratedusing Ag+ to form Ag3AsO4 as a precipitate. (a) What is theoxidation state of As in AsO43-? (b) Name Ag3AsO4 by analogyto the corresponding compound containing phosphorusin place of arsenic. (c) If it took 25.0 mL of 0.102 M Ag+to reach the equivalence point in this titration, what is themass percentage of arsenic in the pesticide?
- What mass of solid Lanthanum (III) oxalate nonahydrate { La2 ( C2O4 )3 ∙ 9 H2O } can be obtained from 650 mL of 0.0170 M aqueous solution of LaCl3 by adding a stoichiometric amount of sodium oxalate ? with solution/explanationThe level of dissolved oxygen in a water sample can be determined by the Winkler method. In a typical analysis, a 100.0-mL sample is made basic, and treated with a solution of MnSO4, resulting in the formation of MnO2. An excess of KI is added, and the solution is acidified, resulting in the formation of Mn2+ and I2. The liberated I2 is titrated with a solution of 0.00870 M Na2S2O3, requiring 8.90 mL to reach the starch indicator end point. Calculate the concentration of dissolved oxygen as parts per million of O2.A 1.963-g sample of an alloy is dissolved in HNO3 and diluted to volume in a 100-mL volumetric flask. Titrating a 25.00-mL portion with 0.1078 M KSCN requires 27.19 mL to reach the end point. What is the %w/w Ag in the alloy?
- A 0.64 g sample containing KCl ( mw = 74.6 ) is dissolved in 50mL of water and titrated to the Ag2CrO4 end point, requiring 26.2 mL of 0.15 M AgNO3 .The %w/w KCl in the sample is ?An unknown sample weighing 0.2583g is titration to the end point with 47.28mL of a 0.10M AgNO3 solution. What is the weight percent of Cl- in the sample?25 mL of a bleach (NaOCl) sample is diluted to 500 mL. An excessive amount of KI is added to the 20 mL solution taken from here and the I2 released is titrated with 35.5 mL of 0.0409 M NaS2O3. Accordingly, calculate the weight percent by volume of NaOCl in the sample. (MaNaOC:74,4 g/mol)
- The mass of K3PO4 needed to prepare 250.0mL of an aqueous solution in which PO4-3 concentration is 0.0550M. The answer is ……………………… How many grams of silver sample is equal to 0.0417 mole of silver The answer is ……………………… When 38.0 mL of 0.1250 M H2SO4 is added to 100 mL of a solution of PbI2, a precipitate of PbSO4 forms. The PbSO4 is then filtered from the solution, dried, and weighed. If the recovered PbSO4 is found to have a mass of 0.0471g, what was the concentration of iodide ions in the original solution The answer is ……………………………… Express 96.342 m using 2 significant figures The answer is ………………………………. The oxidation number of sulfur in (Na2S2O5) is? The answer is ………………………………A solid sample containing some Fe2+ion had a total mass of .9791 g. It required 18.2 ml of 0.02304 M KMnO4 to titrate the Fe2+ in the dissolved sample to a pink endpoint. How many moles of Fe2+ were in the the sample? How many grams of irion were present in the sample and what was the mass percent iron in the sample?0.0585 g Na2C2O4 10 mL to adjust KMnO4 solution prepared in 0.1 M'pure water, 2 M H2SO4 added, heating process and 8.4 mL titrant as a result of titration it's spin out. Calculate the actual concentration of potassium permanganate accordingly
