An 800.0 mg sample containing sulfate was treated with a slight excess of Bac vielding a precipitate that contained 4.3 mg of co-precipitated BaCO3. After i and cooling, the precipitate (BaSO4+ BaCO3) weighed 377.0 mg. Calculate th following:

An 800.0 mg sample containing sulfate was treated with a slight excess of Bac vielding a precipitate that contained 4.3 mg of co-precipitated BaCO3. After i and cooling, the precipitate (BaSO4+ BaCO3) weighed 377.0 mg. Calculate th following:

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.35QAP

See similar textbooks

Related questions

Q: An attempt is made to analyse barium gravimetrically by precipitating of BaF, with NaF2. Assuming…

A: Answer: Precipitation of a sparingly soluble salt takes place only when its ionic product becomes…

Q: The KSP for BaCro4 is 1.2X10-10. Will BaCrO4 precipitate when 10mL of 1.0X10-5M Ba(NO3)2 is mixed…

A: First we have to find moles of barium ions, Then find the concentration of barium ions after…

Q: 11. A 0.8000-g sample of iron ore containing 21.00% Fe is analyzed gravimetrically. If the final…

Q: f 145 mL of a 0.0078 mol/L solution of CuNO3 was mixed with 195 mL of a 1.48 x 10-3 mol/L solution…

A: Solution -

Q: B. Molar Solubility of Calcium Hydroxide in the Presence of a Common Ion Trial 1 Trial 2 Trial 3 1.…

A: 5.) Volume of HCl added is calculated using formula : Volume of HCl added (mL ) = Final buret…

Q: A 0.8000-g sample of iron ore containing 21.00% Fe is analyzed gravimetrically. If the final…

Q: f 27.5 mL of 1.63x10-9M of FeCl3 is added to 98.6mL of 2.58x10-9 M NaOH, will a precipitate of…

A: The question is based on the concept of solubility product principle. it states that a weak…

Q: 1. A bottle containing an alkaline earth chloride was removed due to uncareful handling. The sample…

Q: 100. mL of 0.015 mol L- Pb(NO3)2 and 1500. mL of 0.0020 mol L-1 Nal (sodium iodide) are combined.…

A: Answer:- This question is answered by using the simple solubility product constant expression and…

Q: A sample of freshly precipitated silver chloride weighs 704.7 mg. Before the solution can be…

A: Mass of freshly precipitated AgCl ( M )= 704.7 mg Mass of sample loss before AgCl Solution is…

Q: 3. Calculate the [Ag"] and [CrO4<], and the solubility of Ag2CrO4 in a solution prepared by adding…

A: Solubility product is defined as the product of the solubilities of the individual ions present in a…

Q: Calculate the % w/w Cl– (35.45 g/mol) in the sample. Provide your answer to 2 places after the…

Q: 1. Will Agl03 precipitate when 20 mL of 0.010 M AgIO3 is mixed with 10 mL of 0.015 M NalO3? Ep of…

A: Solution -

Q: (a) Will Ca(OH)2 precipitate from solution if the pH ofa 0.050 M solution of CaCl2 is adjusted to…

A: a) The pH of the solution is first calculated. The dissolution equilibrium for CaCl2 is as follows,

Q: The Ksp for BaCrO4 is 1.2×10−10.1.2×10−10. Will BaCrO4 precipitate upon mixing 10 mL of…

Q: 0.986635g of BaCO3 is dissolved in 1.00dm3 water at 800C. the solution was then cooled down to 250C.…

A: Given: Ksp of BaCO3 at 25 °C =2.58 x 10-9

Q: 1. Outline methods for analysing [Co(NH:)»CIJCI; for the ionic chloride and for the total chloride…

A: Introduction: Ionic chloride reacts with AgNO3 and gives a white precipitate of AgCl. For example,…

Q: *SHOW COMPLETE SOLUTION* A solution contains 0.02 mol Cd2+, 0.02 mol Zn2+, and 1 M HCI is saturated…

A: Ka is the acid dissociation constant which measure the strength of the acid . As the solubility of […

Q: Evaluate

A: Fluoride ions serve as the limiting reagent in the chemical reaction. Two moles of fluoride ions…

Q: ₃ precipitate form if 150.0 mL of 0.002 M BX₃ is mixed with 250.0 mL of pH 9.0 Ba(OH)₂ solution at…

A: The concentration of B+3 from BX3=0.002MAfter mixing total volume of solution =250mL+150mL400mLThe…

Q: A 45.00 ml mixture containing 0.0596 M TI+ and 0.0596 M Hg2*2 is titrated with 0.0878 M Nal…

A: Let the volume of Tl+ and Hg22+ be equal. TlI dissociates in the solution as: TlI ⇌Tl+ + I-…

Q: a.) Concentrated HCl is added to the original solution. A solid precipitate forms. Ag*| Select) Pb2+…

Q: A 185.0 mL sample of 1.200 M Pb(NO3)2 is mixed with 118.50 mL of 1.500 M NaCl, and the P6CI2…

Q: 0.986635g of BaCO3Bace3 is dissolved in 1.00dm3 water at 800C. the solution was then cooled down to…

A: Given: Mass of BaCO3 = 0.986635 g Volume of solution = 1.00 dm3 = 1.00 L…

Q: How many grams of CaF2 (molar mass = 78.077) will dissolve in 750 ml of 0.70 M NaF solution? The Ksp…

A: Given: Concentration of NaF = 0.70 M Volume of NaF solution = 750 mL = 0.750 L…

Q: 50.0 ml of 0.01 M Cd(NO3)2 is added to 50.0 ml of 0.1 M H2S. Will a precipitate form? (the Ksp of…

A: All known compounds can be dissolve in certain solvents whereas they remain insoluble in other…

Q: A solution is prepared such that Li3+=3.0×10-3 M while PO43-=2.0×10-3 M. If the Ksp of Li3PO4 is…

A: A precipitate is an insoluble ionic solid which is formed when certain cations combine with anions.…

Q: What is the molar solubility of a. As2Cd3O8 (Ksp = 2.2E-33) b. Be(OH)2 (Ksp = 6.9E-22) c.…

Q: a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm…

Q: Does a precipitate form when 50.0 mL of 1.OM Ba(OH)2 solution and 86.4 mL of 0.494M H2S04 solution…

A: For precipitation, the Qsp value should be greater than or equal to Ksp value. Qsp≥Ksp If the Qsp…

Q: A solution contains 1.5 x 10-2 moldm-3 I- and 8.0 x 10-3 moldm-3 C2O42-. If aqueous Pb(NO3)2 is…

A: Given : [I-] = 1.5 x 10-2 mol dm-3 [C2O4-2] = 8.0 x 10-3 mol dm-3 Ksp of PbI2 = 9.8 x 10-9…

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: The solubility of Ag2CrO4 (Ksp = 1.2 x 10-12) is several times greater than that of AgCl (Ksp = 1.82…

A: Given: Mass of K2CrO4 = 1 mg Ksp Ag2CrO4 = 1.2 x 10-12 Ksp AgCl = 1.82 x 10-10 To determine: The…

Q: 123 mL of a 0.352 M Ca(NO3)2 solution is mixed with 251 mL of a 0.254 M solution of NaF at 25ºC.…

A: Given that, Volume of 0.352 M Ca(NO3)2 solution = 123 mL = 0.123 L Moles of 0.352 M Ca(NO3)2 in…

Q: 1- The mercury present in a sample with a mass equal to 0.8142 g was precipitated with an excess of…

A: Given information, Mass sample of mercury = 0.8142 g Mass of product i.e. Hg5(IO6)2 = 0.4114 g

Q: The molar solubility of MgCO3 (Ksp = 3.500 x 10°°) in distilled water at room temperature is M.…

Q: Effect of Common lons on the Solubility of Ca(OH)2 Answer the concentrations and solubility in 3…

A: Given the molarity of the standardized HCl solution = 0.1980 M

Q: (a) For the precipitation reaction: A+ + B–  AB(s)Calculate the value of the equilibrium constant…

A: The answer for part (a) is given below. Kindly repost the other questions as separate question. a)…

Q: The Ksp for silver chromate (Ag2CrO4) is 1.1x10-12. Using the same initial set up of 10mL of 1M…

A: The solubility of and CrO42- ions in the aqueous solution is considered to be s and the solubility…

Q: 0.500 M Ca(NO3)2 is added to 25.0mL of 0.250 M NaF at 25°C? (Ksp of CaF2 = 5.3 X 10^-9 at 25

A: Solubility equilibrium of CaF2 CaF2(s) <----> Ca2+(aq.) + 2F-(aq.) Condition for…

Q: 4.0 mL of 0.20 M HCI is added to 4.0 mL of 0.30 M Pb(NO3)2 to produce a precipitate of P6CI215)-…

Q: 0.986635g of BaCO3Baco3 is dissolved in 1.00dm3 water at 800C. the solution was then cooled down to…

A: Given: Mass of BaCO3 = 0.986635 g Volume of solution = 1.00 dm3 = 1.00 L…

Q: Using an experimentally determined value (2.4×10−10) of Ksp, determine the value for the reaction…

A: we need to calculate the value of Q for Ag2CrO4

Q: If 250.0 mL of 0.0010 M Sr(NO3)2 were added to 50.0 mL of 0.0000010 M Na2CO3 would a precipitate of…

Q: A 0.5g sample of CaCO3 is dissolved in an acidic solution. The calcium is precipitated as…

A: Given Mass of sample = 0.5 g Mass of dry precipitate = 0.72 g

Q: 3. A 10.0-mL sample of aqueous NaOCl is treated with excess KI in an acidic solution. The quantity…

A: Molarity of NaOCl can be calculated using the balanced reaction for iodine generation when NaOCl…

Q: Determine the minimum concentration of NaF required to precipitate BaF2 from a solution containing…

Q: Will a precipitate form when 3.0 L of 0.0016 M BaCl2 is added to 5.0 L of 0.0024 M KF? The Ksp of…

A: In a saturated solution, the molar solubility of salt is used to determine the solubility product.…

Q: A 45.0 mL sample of 0.0015 M BaCl2 was added to a beaker containing 75.0 mL of 0.0025 M KF. Will a…

A: The volume of 0.0015 M BaCl2 is 45.0 mL. The volume of 0.0025 KF is 75.0 mL. The solubility product…

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…

Question

An 800.0 mg sample containing sulfate was treated with a slight excess of Bac
vielding a precipitate that contained 4.3 mg of co-precipitated BaCO3. After i
and cooling, the precipitate (BaSO4+ BaCO3) weighed 377.0 mg. Calculate th
following:

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step by step

Solved in 4 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

The following solutions are mixed: 1.0 L of 0.00010 M NaOH and 1.0 L of 0.0014 M MgSO4. Is a precipitate expected? Explain.
A roll of 35-mm black and white photographic film contains about 0.27 g of unexposed AgBr before developing. What mass of Na2S2O35H2O (sodium thiosulfate pent hydrate or hypo) in 1.0 L of developer is required to dissolve the AgBr as Ag(S2O3)23- (Kf=4.71013)?
A 0.125-M solution of 0.075 Mn(NO3)2 is saturated with H2S([H2S]=0.10M). At what pH does Mns begin to precipitate?. MnS(s)Mn2+(aq)+S2(aq)Ksp=4.31022 H2S(aq)+2H2O(l)2H3O+(aq)+S2(aq)K=1.01026
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
The % (w/w) I- (MM = 126.9) in a 0.5812-g sample was determined by Volhard titration. After adding 50.00 mL of 0.06912 M AgNO3 and allowing the precipitate to form, the remaining silver was back-titrated with 0.07012 M KSCN, requiring 36.17 mL to reach the endpoint. Report the %(w/w) I- in the sample. 17.76 % 20.08 % 35.52 % 40.16%
5. A 300.0 mg sample containing Na,CO3, NaHCO, and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 ml to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
The % w/w I– in a 0.6712-g sample was determined by Volhard titration. After adding 50.00 mL of 0.05619 M AgNO3 and allowing the precipitate to form, the remaining silver was back titrated with 0.05322 M KSCN, requiring 35.14 mL to reach endpoint. AgNO3 + I– → AgI (s) + NO3– Ag+ + SCN– → AgSCN How many millimoles of AgNO3 reacted with I–?
The % (w/w) I- in a 0.6712-g sample was determined by Volhard titration. After adding 50.00 mL of 0.05619 M AgNO3 and allowing the precipitate to form, the remaining silver was back-titrated with 0.05322 M KSCN, requiring 35.14 mL to reach the endpoint. Report the %(w/w) I- in the sample. [Ans. 17.76 % (w /w)]
11. A 0.485 g sample containing chloride was titrated with 36.8 mL of 0.1060 M AgNO3 stock solution. Express the results of this analysis in:a) Percent by weight of Clb) Weight percent Cl2c) Percent by weight of CaCl2d) Weight percent of AlC13
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 detergent
Q2: A 3.275 g sample of K2CrO4 yielded a precipitate of Cr,03 which weighed 1.075 g. Calculate Cr % and the purity of the salt.

SEE MORE QUESTIONS

Recommended textbooks for you

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry