The Sn in a 0.4352 g mineral specimen was reduced to the +2 state with Pb and titrated with 29.77 mL of 0.01735 M K2Cr2O7. Identify: 1) balanced chemical reaction 2) appropriate indicator and its type 3) color at the end point 4) % SnO2 in the sample
Q: Calculate the equilibrium concentration of Zn2 + in a solution that was prepared by mixing 75.0 mL…
A: Zinc is determined by EDTA titration in almost the same way magnesium is - in the pH 10 against…
Q: 1. Aluminum is determined gravimetrically by precipitating Al(OH)3 and isolating Al½O3. A sample…
A: “Since you have posted a question with multiple sub-parts, we will solve first three subparts for…
Q: The phosphate in a 3.00 g sample of industrial detergent was precipitated by the addition of 1.000 g…
A: Precipitation titration is that type of volumetric titration in which precipitates are formed. It is…
Q: A 3650-mg sample containing bromate and bromide was dissolved in sufficient water to give 250.0 mL.…
A:
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: In supposing that a linear relationship exists between the readings taken from the apparatus and…
A: We will first plot the calibration curve using turbidity (y axis) vs concentration (x axis) data.
Q: The arsenic in a 1.203-g sample was converted to H,AsO4 by suitable treatment. The acid was then…
A: Given data: Weight of pesticide = 1. 203 g Pesticide →H3AsO4→AgNO3 Ag3AsO4 Ag++SCN- →AgSCN(s)…
Q: A 0.64 g sample containing KCI (mw = 74.6 ) is dissolved in 50mL of water and titrated to the…
A: At end point milliequivalents of KCl and milliequivalents of AgNO3 are equal.
Q: The phosphate in a 3.000-g sample of industrial detergent was precipitated by the addition of 1.000…
A: Given Mass of sample - 3 g Mass of AgNO3 = 1g Volume of KSCN = 18.23 ml Molarity of KSCN = 0.1337 M
Q: The amount of iron in a meteorite was determined by a redox titration using KMnO4 as the titrant. A…
A: Redox titration involves the determination of concentration of a given analyte by using the concept…
Q: The alcohol content of a certain low alcohol beer was determined using volumetric analysis. In this…
A:
Q: A 0.2386-g sample contained only NaCI and KBr. It was dissolved in water and required 48.40 mL of…
A:
Q: A 600.0 mg sample consisting of only CaC2O4and Mg C2O4is heated at 500oC converting the two salts to…
A: Answer: This question is based on the stoichiometric calculation where ratio of the mass of a…
Q: A shipment of containing NaOH (40 g/mol) and Na2CO3 (106 g/mol) was declared to contain less than 10…
A: #(a): Given the shipment contains a mixture of NaOH (40 g/mol) and Na2CO3 (106 g/mol).
Q: A 0.512 g sample of CaCO3 is dissolved in 12 M HCl and the mixture is diluted to 250 mL. A small…
A: A 250 mL solution of CaCO3 is prepared by dissolving a sample of 0.512 g of CaCO3 in 12 M HCl and…
Q: A two-liter sample of mineral water was evaporated to a small volume, following which the potassium…
A:
Q: A 2.950 sample containing NH,CI, Rb,CO3 and inert material was dissolved to give 250.0 ml of…
A: Therefore,
Q: A 0.1214-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of…
A: The net ionic equation is given below
Q: The sulfur from 4.00g steel is evolved as dihydrogen sulfide gas and titrated with 1.60 mL of…
A:
Q: 6. The mercury in a 0.839 g sample was precipitated with an excess paraperiodic acid, H¿IO, SHg* +…
A: Given reaction is : 5Hg2+ + 2H5IO6 -------> Hg5(IO6)2 + 10 H+ Given mass of the sample = 0.839…
Q: The % w/w I– in a 0.6712-g sample was determined by Volhard titration. After adding 50.00 mL of…
A: Given reaction AgNO3 + I– → AgI (s) + NO3– Ag+ + SCN– → AgSCN We have to find milli moles of AgNO3…
Q: The sulfate in a247.1 mg sample was precipitated as BasO4 by addition of 25.00 mL of 0.03992 M…
A: Given: Mass of sulfate = 247.1 mg Volume of BaCl2 = 25.00 mL Molarity of of BaCl2 =…
Q: The arsenic in a 1.203-g sample of a pesticide was converted to H₃AsO₄ by suitable treatment. The…
A:
Q: The phosphate in a 3.000 g sample of industrial detergent was precipitated by the addition of 1.000…
A: Mass of phosphate sample = 3.0 gram Mass of AgNO3 added = 1.0 gram Required volume of Filterate =…
Q: A mineral in a fine state of division (0.6324 g) was dissolved in 25.0 mL of 4.0 mol / L boiling HCl…
A:
Q: А, В, С + NH3 1. + HNO3, 2. toluene white precipitate white precipitate yellow toluene layer,…
A: Given scheme is:
Q: Using basic conditions, MnO4- can be used as titrant for the analysis of Mn2+, with both the analyte…
A: A question based on quantitative analysis, which is to be accomplished.
Q: The arsenic in a 1.208-g sample of a pesticide was converted to H3 AsO4 by suitable treatment. The…
A:
Q: ml of a solution containing an 30.00 unknown amount of I ( iodide) was treated with 50 ml of 0.3650M…
A: Given : Volume of solution = 30.0 mL =0.03 L 50 ml of 0.3650 M AgNO3 = 0.050 L…
Q: An antihistamine sample, brompheniramine maleate, weighing 5.01234 g was dissolved in alcohol and…
A: Mass of an antihistamine sample, Brompheniramine maleate = 5.01234 g Molarity of AgNO3 = 0.3121 M…
Q: After titration, weight percent of oxalate in K3[Fe(C2O4)3] (MW: 437.2 g/mol) sample was determined…
A: Given; Actual weight % of oxalate ion=55.8% The molar mass of K3[Fe(C2O4)3]=437.2 g/mol. The molar…
Q: A dried sample of commercial salt was prepared by a coning and quartering. A 0.911-g sample of the…
A: NaCl (aq) + AgNO3(aq) -----> AgCl(s) + NaNO3(aq) 1 mole AgNO3(silver nitrate) neutralizes 1 mole…
Q: A mixture containing iodide is analyzed by the Volhard method. 0.6712 g of the sample is reacted…
A: mass of the sample = 0.6712 g Concentration of AgNO3=0.05619 M Volume of AgNO3=50.00mL Concentration…
Q: Q1/ What weight of pyrite ore (impure FeS2) must be taken for analysis so that the BaSO, precipitate…
A:
Q: The phosphate in a 3.000 g sample of industrial detergent was precipitated by the addition of 1.000…
A: Solution Given that Phosphate = 3.000g AgNO3 = 1.000g KSCN = 0.1377M…
Q: 5. 0.1500 g sample of chromium ore was dissolved and the chromium oxidized to chromate ion. The…
A: Answer: This question is based on the stoichiometric calculation where we have to convert the number…
Q: A colorless aqueous solution contains nitrates of two metals, X and Y. When it was added to a…
A: The question is based on the concept of qualitative analysis. We have to identify the cations…
Q: The %w/w Cl- (36.45 g/mol) in a 0.5785 g sample was determined by Volhard titration. After adding…
A:
Q: 6. The phosphorus content in a 0.3004-g sample was precipitated as (NH4);PO4 .12M0O3 a slightly…
A: Given: Mass of PbMoO4 precipitate formed = 0.3017 g. And mass of sample used = 0.3004 g. Molar mass…
Q: 3. For the determination of Zn (AW 65) gravimetrically in a sample it is precipitated and weight as…
A:
Q: ure KI is treated with 0.1942g of pure K2CrO4 and the solution is boiled to expel all of the…
A: Given: Sample is 0.35 g impure KI Pure K2CrO4 is 0.1942 g
Q: The Sn in a 0.4352 g mineral specimen was reduced to the +2 state and titrated with 29.77 mL of…
A: Redox titration is the titration used to determine the analyte concentration by carrying out a redox…
Q: The % w/w I– in a 0.6712-g sample was determined by Volhard titration. After adding 50.00 mL of…
A: Answer: These questions are based on stoichiometric calculation where we have to convert the moles…
Q: concentration and pH of the H2SO4 solution.
A:
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: A 1.2 g sample of mixture of NaOH and Na:CO, containing inert impurities s dissolved and titrated…
A: Given : Weight of sample = 1.2 g Concentration of HCl = 0.5 N Volume of HCl required to reach…
Q: 21. Some 1.0 g steel samples are believed to contain about 2.5% cobalt. Ifa 10% excess of the…
A: Molecular weight of cobalt = 59 Molecular weight of 1-nitroso-2-naphthol = 173
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
Q: A solution is made by mixing 500.0 mL of 0.02018 M Na, HASO, with 500.0 mL of 0.04078 M NaOH.…
A: Solution: From the given data one thing we have clear that this is the type of acid base reaction.…
Q: Ca in a 5.0 ml urine sample was precipitated, redissolved and required 16.17mL of standard MnO,…
A: Determination of Ca in urine Calcium content of urine is determined by the following procedure. In…
The Sn in a 0.4352 g mineral specimen was reduced to the +2 state with Pb and titrated with 29.77 mL of 0.01735 M K2Cr2O7. Identify:
1) balanced
2) appropriate indicator and its type
3) color at the end point
4) % SnO2 in the sample
Step by step
Solved in 2 steps
- The phosphate in a 3.000-g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO3. The solution was filtered and filtrate, upon addition of 1.00 mL of 0.01 M fecl3, required 18.23 mL of 0.1377 M KSCN for titration to the end point. (a) what type of precipitation titrimetry was used. (b) which served as the indicator (c) the color at the endpoint (d) the weight percent of phosphate in the detergent.The phosphate in a 3.000-g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO3. The solution was filtered and filtrate, upon addition of 1.00 mL of 0.01 M fecl3, required 18.23 mL of 0.1377 M KSCN for titration to the end point. (a) the weight percent of phosphate in the detergentThe phosphate in a 3.000 g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO3. The solution was filtered and the filtrate required 18.23 mL of 0.1377 M KSCN for titration to the FeSCN2+ end point. Calculate the percentage of phosphate in the detergent.
- The phosphate in a 3.00 g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO₃ (169.87 g/mol). The solution was filtered and the filtrate, upon addition of 1.00 mL of 0.01 M FeCl₃, required 18.23 mL of 0.1377 M KSCN for titration to the endpoint. Identify (a) what type of precipitation titrimetry was used (b) which served as the indicator (c) the color at the end point Calculate (d) the weight percent of phosphate (94.97 g/mol) in the detergent.1. 0.646 g of sample containing BaCl2.2H2O (244.26 g/mol) was dissolved and enoughpotassium chromate was added. After filtering, the precipitate was dissolved in acid andenough KI was added and titrated with thiosulfate. Since 48.7 mL of 0.137 M thiosulfateis used for this, what is the percentage of BaCl2.2H2O in the sample?K2Cr2O7 + 7H2SO4 + 6KI 4K2SO4 + Cr2(SO4)3 + 7H2O + 3I2Chloride 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.
- The arsenic in a 2.345g sample of a pesticide was converted to H 3 AsO4 by suitable treatment.The acid was then neutralized, and 60.00 ml of 0.06781M AgNO 3 was added to precipitate thearsenic quantitatively as Ag 3 AsO4. The excess Ag+ in the filtrate and washings from theprecipitate was titrated with 15.27 ml of 0.123 M KSCN; the reaction wasAg+ + SCN- → AgSCN(s)Calculate the percentage As 2 O 3 in the sample.A 1.7483-g sample containing Al(NO:)3, AICI, and inert material was dissolved in acid and divided into two equal portions. One portion was treated with 5.00 mmol of AGNO:. The excess Ag" required 28.89 mL of 0.1002 M KSCN for titration. The other portion required 26.02 mL of 0.1193 M NaOH for titration: Al* +3 OH → AI(OH):(s) Calculate the percentage composition of Al(NO:)s and AICl3s in the sample.A limestone sample weighing 400 mg was dissolved in acid treated with excess sodium oxalate. The solution was made basic and the resulting calcium oxalate was filtered, washed and redissolved in dilute acid. This solution required 14.0 mL of 0.00865 M KMnO4. What is the % Ca of the limestone.
- A 4.912-g sample of a petroleum product was burnedin a tube furnace, and the SO2produced was collectedin 3% H2O2.Reaction:SO2(g)+H2O2→H2SO4A 25.00-mL portion of 0.00873 M NaOH was introducedinto the solution of H2SO4, following whichthe excess base was back-titrated with 15.17 mL of0.01102 M HCl. Calculate the sulfur concentrationin the sample in parts per million.A sample containing phosphorus weighs 4.2580g. The phosphorus in the sample is converted into phosphate ion and precipitated as silver phosphate through the addition of 50mL of 0.0820M of silver nitrate. The excess silver nitrate was back titrated with 4.06mL of 0.0625M of potassium thiocyanate. Calculate the % phosphorus pentoxide in the sample.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 the precipitate was titrated with 10.76 mL of 0.1000M KSCN; the reaction was Ag+ + SCN-→ AgSCN(s) Calculate the percent AsO3 in the sample.