30.00 mL of K2Cr2O7 , 0.1900 M, Is used as a titrant in a 25mL solution of Sn2+ Below is the balanced equation. 3Sn2+ + Cr2O2-7+14H+ -> 3Sn4++2Cr3++ 7H2O What is the Final Molarity of K2Cr2O7 & Sn2+
Q: Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000519 mol…
A: The overall net reaction between sodium hypochlorite and KIO3 under acidic condition is written…
Q: A titrant solution of KMNO4 was standardized with 0.2g of Na2C2O4 amd consumed 27.75 mL to reach…
A: Given that, a titrant solution of KMnO4 was standardized with 0.2 g of sodium oxalate (Na2C2O4) and…
Q: SO2 + 2 MnO4- + H2O ---> 5 SO42- + 2 Mn2+ + 4 H+ The MnO4- solution is poured in a burette and then…
A: When equivalent points reached then both molecules should have equal equivalent We should equal…
Q: A base (B) that is dibasic is titrated with a strong acid. At what added volume (V) is the pH of the…
A: Equivalence point can be determined using equivalence point volume.
Q: Consider the titration 40mL of 0.10M NaI with 0.05M Ag+. What is the major species present in the…
A: The correct option would be:
Q: Titration of the I2 produced from 0.1142g of primary standard KIO3 required 27.95 mL of sodium…
A: The mole of KIO3 is calculated as,
Q: Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant…
A: The reaction of Na2CO3 with HCl is, Na2CO3 + 2HCl = 2NaCl + CO2 + H2O Given Formula mass of Na2CO3 =…
Q: 4. A 0.1036-g sample containing only BaC2 and NaCl is dissolved in 50 mL of distilled water.…
A: Given data Mass of sample mixture [BaCl2 + NaCl] = 0.1036 g Volume of distilled water= 50 mL…
Q: Calculate the % w/w Cl– (35.45 g/mol) in the sample. Provide your answer to 2 places after the…
A:
Q: A 25.0025.00 mL solution of 0.033000.03300 M Na2CO3Na2CO3 is titrated with 0.026300.02630 M…
A: Using molarity equation as shown below- M1: molarity of Sodium Carbonate. V1: volume of Sodium…
Q: A solution contains NaHCO3, Na2CO3, and NaOH, either alone or in permissible combination. Titration…
A:
Q: Direct titration: 10.00 ± 0.02 ml of an unknown KHP solution required 11.54 + 0.02 ml of 0.1010…
A: The concentration of an unknown KHP is calculated as shown below.…
Q: A chemist titrates 30.0 mL of a sample solution containing CI-(aq) ions with a 0.0489 mol/L…
A: The balanced reaction taking place is given as, Given : Concentration of KMnO4 = 0.0489 M Volume of…
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: 1. How many ml of 0.30M solution of H2SO4 will react with 20ml of a 0.30M solution of NaOH?…
A: Solved only first question in accordance to guidelines. You can repost remaining questions.
Q: You are performing an experiment in lab that involves the titration of 25.0 mL of H2SO4 solution.…
A: According to the neutralization reaction between NaOH and H2SO4, the stoichiometric ration between…
Q: arsenic in a 1.010 g sample of pesticide was converted to H3ASO4 by appropriate means. The acid…
A:
Q: A sodium thiosulfate solution is standardized using pure copper as the primary standard. A sample of…
A: Given data, Mass of Cu = 0.2624 g Volume of sodium thiosulfate =…
Q: IO3– + 8I– + 6H+ ⇌ 3I3– + 3H2O. The 50-mL of I3 or triiodide (0.0014 mol) was used to standardize…
A:
Q: accordingly
A: Mass of Na2C2O4 = 0.0585 g Molar mass of Na2C2O4 = 134 g/mol At equivalent point, Geq. of KMnO4 =…
Q: Titration of the I2 produced from 0.1142 g of primary-standard KIO3 required 27.95 mL of sodium…
A: Given, Mass of primary standard KIO3 0.1142 g Volume of sodium thiosulfate (Na2S2O3) = 27.95 mL =…
Q: It is desired to determine the concentration of chlorides in a powdered milk following the method of…
A: Given data,Mass of milk sample=1.5gMolarity of AgNO3=1MVolume of AgNO3 added=20mLMolarity of…
Q: Imagine a titration of 38.77 mg of a solid dissolved in water. If the titration is stopped when…
A: The amount of solid dissolved in water is 38.77 g. The amount of 0.1000 M AgNO3 required for…
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 10.0 mL aliquot of H2 SO4 solution was diluted to 100.0 mL. Then 25.0 mL aliquot of the diluted H2…
A: Here we are required to find the molar concentration of original sulphuric acid
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: Molarity of (NH3) solution (M) from bottle- 5.0 Initial reading of buret (NH3) (mL)- .27 Final…
A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…
Q: 0.5 gr of a diprotic acid is dissolved in water and titrated with 10 mL 1 M KOH to phenolphthalein…
A:
Q: 0.753-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the…
A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…
Q: A How many mL of 0.40 M NaOH would be fequired to titrate 22.50 mL of 0.250 M H2C2O4 to the…
A:
Q: You want to measure the concentration of carbonate (CO32-) in a mildly basic solution by using an…
A: The concentration and the number of moles of Ca2+ ion in the filtered solution is;…
Q: 0.5 gr of a diprotic acid is dissolved in water and titrated with 10 mL 1 M KOH to phenolphthalein…
A: The mass of diprotic acid is = 0.5 g The molarity of KOH solution = 1M The volume of KOH solution =…
Q: 0.5 gr of a diprotic acid is dissolved in water and titrated with 10 mL 1 M KOH to phenolphthalein…
A:
Q: Consider the titration of the weak acid, benzoic acid, HC7H5O2. Its acid dissociation reaction is:…
A: The question is based on the concept of titration. We have to calculate acid dissociation constant…
Q: Titration of 0.2121 g of primary standard Na2C204 (133.999 g/mol) required 21.66 mL of KMN04…
A: Given: The mass of the primary standard is 0.2121 g. The molar mass of sodium oxalate is 133.999…
Q: 2) Mohr's method uses the potassium chromate (K2CIO:) as indicator and this indicator makes the…
A:
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: 175.0 mL of 0.2015 M nitric acid was added to 1.4213 g of impure calcium carbonate sample. The…
A: The balanced equations are 2 HNO3 + CaCO3 ----------> Ca(NO3)2 + CO2 + H2O NaOH + HNO3…
Q: A 100.0-mL sample of brackish water was made ammoniacal, and the sulfide it contained was titrated…
A: Answer: This question is based on stoichiometric calculation where moles of silver nitrate will be…
Q: EXAMPLE: Chromium(III) is slow to react with EDTA (HAY) and is therefore determined by…
A: The question is based on the concept of quantitative estimation. We have to determine amount of…
Q: 3. A weak acid was titrated using 0.20 M KOH. The pH at several volumes added was recorded and…
A: Given: Mass of acid (assuming it monoprotic like HA) = 175 mg = 0.175 g. Concentration of KOH = 0.20…
Q: Molarity of the standard solution of sodium hydroxide = 0.1010 mol/L %3D Volumes of NaOH(aq): First…
A: Titration is a laboratory quantitative technique in chemistry that is used to determine the…
Q: Titration of 0.2120 g of pure Na,C204 (134.0 g/mol) required 43.31ml of KMNO4 solution according to…
A: The reaction that takes place during titration is :2 MnO4-+5Cr2O42-+16H+→2 Mn2+10 CO2 +8H2OMass of…
Q: 0.5 gr of a diprotic acid is dissolved in water and titrated with 10 mL 1 M KOH to phenolphthalein…
A:
Q: Titration of 53.00 mL of 0.04746 M Na2 C2 O4 required 39.33 mL of a potassium permanganate solution.…
A: During titration at equivalence point the number of moles of titrant = number of moles of analyte
Q: Titration of a 0.492-g KH₂PO4 used 25.6 mL of 0.112M NaOH. What is the percent purity of KH₂PO4? MW…
A: The number of moles of a substance is determined as the mass of the substance upon its molar mass.…
Q: 102A 0.2295-g sample of sodium oxalate (Na₂C₂O4-134g/mol; 97.8%) required 35.12mL of a potassium .…
A: Gram milliequivalent weight can be figure out by considering n factor for the sodium oxalate.
Q: 50 mL sample solution containing Na2CO3 and NaOH is titrated with 0.2 M HCl solution. Acid…
A: In the presence of a strong base (NaOH) in the mixture of Na2CO3 and NaOH, HCl first reacts with…
Q: A titration of 50.00 mL of 0.1100 M Fe3+ with 0.07750 M Sn2+ is carried out. The analytical reaction…
A: Equivalance point is the point where all moles of one reactant is neutralized by another compound.…
30.00 mL of K2Cr2O7 , 0.1900 M, Is used as a titrant in a 25mL solution of Sn2+
Below is the balanced equation.
3Sn2+ + Cr2O2-7+14H+ -> 3Sn4++2Cr3++ 7H2O
What is the Final Molarity of
K2Cr2O7 & Sn2+
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 4 images
- 1ml of 1mg/ml of diluted aspirin powder solution is titrated by 0.005M NaOH. Before titration, 5 ml ethanol, 14 ml CO2 free water, and 4 drops bromothymol blue indicator is added into diluted aspirin powder solution. Mass of 0.005M NaOH used is obtained by weight titration = 1.1384g . [Molar mass of aspirin =180.15]; for solution, 1g=1mL at 25 degree Celcius. Calculate the purity of the powder.If 1.000 ml. of a solution of KMn04 is equiva- lent to 0.1000 millimole of NaCHO2 (sodium formate) in the fol- lowing titration: 3CHO2- + 2MnO- + H2O -> 3CO2 + 2MnO2 + 5OH-, what is the value of the KMnO4 in terms of grams of CaO in the volumetric method for calcium in which that element is precipitated as CaC2 4 .H2O and the precipitate is filtered, dis- solved in dilute H2S04 , and the oxalate titrated with permanganate?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?
- The arsenic in a 1.010 g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, and exactly 40.00 mL of 0.06222M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag in the filtrate and in the washings from theprecipitate was titrated with 10.76 mL of 0.1000MKSCN; the reaction wasAg+ + SCN-→ AgSCN(s) Calculate the percent AsO3 in the sample.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 endpointA 370.00 mL solution of 0.00185 M A3B4 is added to a 390.00 mL solution of 0.00100 M C3D4. What is pQsp for A3D4?
- Using basic conditions, MnO4- can be used as titrant for the analysis of Mn2+, with both the analyte and the titrant ending up as MnO2. In the analysis of a mineral sample for manganese, a 0.5165-g sample is dissolved, and the manganese is reduced to Mn2+. The solution is made basic and titrated with 0.03358 M KMnO4, requiring 34.88 mL to reach the endpoint. Calculate the %w/w Mn in the mineral sample. Answer: % Mn =a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm (m:v) in Fe? b) Using this stock solution, what aliquot must be used to prepare calibration solutions, 100 mL volume, of the following concentrations: 0.100 ppm, 0.500 ppm, 2.00 ppm, 4.00 ppm, and 7.00 ppm.The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 5SO2 + 2MnO4- + 2H2O ---> 5SO42- + 2Ms2 + 4H+ Calculate the number of grams of SO2 in a sample of air if 4.90mL of 0.00700M KMnO4 solution are required for the titration. Be sure your answer has the correct number of significant digits.
- A saturated solution of magnesium hydroxide is prepared and the excess solid magneisum hydorixed is allowed to settle. A 25.0 mL aliquot of the saturated solution is withdrawn and transfered to a flask, two drops of inficator are added. A 0.00053 M HCL is dispensed from a buret into a solution. The solution changes color after the addition of 13.2 mL. What is the Ksp of magnesium hydroxide?A shipment of containing NaOH (40 g/mol) and Na2CO3 (106 g/mol) was declared to contain less than 10 % impurity. However, Noel is suspicious that the declared impurity is higher. Being the best and brightest employee of the year, Noel weighed 1.000 g sample, dissolved in 50.0 mL of distilled water and titrated with cold 0.5000 M HCl. With Phenolphthalein as indicator, the solution turns colorless after the addition of 30.00 mL of the acid. Methyl Orange is then added, and 5.00 mL more of the acid is required before this this indicator changes color. Calculate the following: a. Determine the volume of the acid to fully neutralize NaOH (final answer up to one decimal place) =400 g sample containing chloride ions (MW=35.45 g/mol) was dissolved in 50.0mL of distilled water. A 15.0 mL aliquot was taken, and was further diluted to 50.0 mL using distilled water. The diluted solution was then titrated using a 0.0989 M AgNO3 solution, and it consumed a total of 31.9 mL of the titrant in order to reach the end point. What is the concentration of the undiluted chloride solution? Round off to three (3) significant figures. What is the % (w/v) concentration of the undiluted chloride solution? Round off to two (2) decimal points. What is the % (w/w) of Cl- composition of the sample? Round off to two (2) decimal points.