Answered: A 0.2356 g sample containg only NaCl…

A 0.2356 g sample containg only NaCl (58.44 g/mol) and BaCl, (208.23 g/mol) yielded 0.4637 g of dried AgCl (143.32 g/mol). Calculate the percent of each halogen compound in the sample.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.23QAP

See similar textbooks

Related questions

Q: Determination of a chemical formula, mass of crucible is 14.9234g, crucible + hydrated sample is…

A: Given Mass of Crucible = 14.9234 Mass of hydrated sample = 1.6618 gram Mass of crucible + Mass of…

Q: Covert 0.00823 moles of HCL to g Convert 0.00911 moles Mg to g

A: Using formula: No Of moles (n)= given mass/molar mass No of moles of HCl is 0.00823mole No. Of…

Q: From the following, pick those that are empirical forme

A: Simplest whole number ratio of constituent elements in a compound is called empirical formula…

Q: What is the empirical formula for a compound that is comprised of 54.0% Sodium, 8.50% boron and…

A: The simplest formula or the empirical formula provides the lowest whole number ratio of atoms…

Q: A 2.37 gram sample of a KCI and KCIO3 mixture was found to contain 0.01611 mol of KCIO3. What is the…

A: Mass of mixture of KCl and KClO3 = 2.37 g Number of moles of KClO3 = 0.01611 mol Molar mass of KClO3…

Q: Suppose a student starts with 2.4185 g of a sand mixture and separates the components into 1.3012 g…

A: The mass percentage is the simplest way of representing the mass of the components present in the…

Q: 10. A 2.00g strip of Mg is reacted with oxygen inside a flash bulb by pressing the shutter. The…

A: Magnesium reacts with oxygen to form magnesium oxide. Reactants always react with each other in a…

Q: The number of moles in 37.80 g of C2H6O (molar mass = 46.1 g/mol) is?

A: Given information, Mass of C2H6O is 37.80 g. Molar mass of C2H6O is 46.1 g/mol.

Q: An elemental analysis of a 0.3285 g of a compound containing C, H, O and S undergo combustion and…

Q: 0.333 g of a hydrocarbon (CxHy) was analyzed by combustion analysis and 1.009 g of CO2 (MM = 44.01…

A: Mole concept: The number of molecules or atoms present in the one mole of the substance is equal to…

Q: A sample of nickel ore, which has nickel as the only metal present, is treated with an excessnof…

A: a) Please find below the balanced reaction Ni + H2SO4 ----> NiSO4 + H2

Q: A sample of copper wire with a mass of 1.659g is heated with excess powdered sulfur until the copper…

A: Weel know that , Empirical formula represent the simplest ratio of all atom present in the molecule…

Q: A chemist is given a sample of the CuSO4 hydrate and asked to determine the empirical formula of it.…

A: Given, Mass of hydrated CuSO4 = 42.75 g Mass of Unhydrated salt = 27.38 g Formula of hydrate = ?

Q: 22 A compound consists of 40.00% carbon, 6.71% hydrogen and 53.29% oxygen and has a molecular mass…

Q: The characteristic odor of pineapple is due to ethyl butyrate,a compound containing carbon,…

Q: 0.30g of an unknown organic compound containing C, H and O gave 0.733g of carbon dioxide and 0.30g…

A: The combustion equation for an organic compound may be written as:

Q: What is the maximum number of moles of Al203 that can be produced by the reaction of 0.40 mol of Al…

Q: A compound containing the elements C , H , N , and O is analyzed. When a 1.2359 g sample is burned…

A: Given L The compound contains elements C, H, N and O only. Mass of compound = 1.2359 g Mass of H in…

Q: Calculate tge empirical and molecular formula

A: From the question we get:- Carbon = 24.27% Hydrogen = 4.07% Chlorine = 71.65% Molar Mass = 99 g/mol.…

Q: If you added 231.9 grams of HF to an excess of Mg(OH),, how many moles of HF have you added?

Q: Calculate the molar mass of a sample containing 34 molecule that weighs 7X 10^-22 g.

A: Given : Number of molecules = 34 Mass of sample = 7 × 10-22 g To calculate :- Molar mass of…

Q: A white-colored solid contains 75.26% Ag by mass, and the rest is chlorine. Enter the empirical…

Q: Determination of a chemical formula, mass of crucible is 14.9234g, crucible + hydrated sample is…

A: Mass of hydrated sample =( Mass of crucible + hydrated sample) - Mass of crucible

Q: How many moles of Fe203 will be produced from 10.0 moles FeS and 20.0 moles of0?

A: 4 moles of FeS reacts with 7 moles of O2 10moles of FeS reacts with 7 x 10/4 = 17.5 moles so,…

Q: Predict what mass of carbon dioxide is produced from 10.0 g of butane and 30.0 g of oxygen.

A: The number of moles for a given chemical species refers to the ratio of mass of the species to that…

Q: How many g of C4H4S2 are equivalent to 5.40 moles of this compound?

A: Answer: 627.48 g

Q: f 37.0 g of MgSO4⋅7H2O is thoroughly heated, what mass of anhydrous magnesium sulfate will remain?…

A: On strong heating, water molecules get removed and turn hydrated salt into anhydrous salt.The…

Q: A sample of an oxide of vanadium weighing 4.589 g was reduced with hydrogen gas to form water and…

A: Solution : The empirical formula gives the simple whole-number ratio of elements present in a…

Q: Question attached

A: Empirical formula refers to the formula of a compound in which the elements are present in the…

Q: N2(g) + 3 H,(g)→2 NH;(g) How many moles of NH, can be formed from 3.0 mol of N, and 6.0 mol of H,?

A: Given reaction is : N2 (g) + 3H2 (g) ---------> 2NH3 (g) Moles of N2 = 3.0 mole Moles of H2 =…

Q: A new organic material is to be examined by combustion analysis. Burning 0.09303 g of this sample in…

A: The sample contains the percentage of, C = 40.63 % H = 5.08 % O = 54•28%

Q: (a) One molecule of the antibiotic penicillin G has a massof 5.342 * 10-21 g. What is the molar mass…

A: (a) Given information, One molecule of the antibiotic penicillin G has a mass of 5.342 * 10-21…

Q: Determine the empirical and molecular formulas of each ofthe following substances:(a) Styrene, a…

Q: Describe the compositions of Compound?

A: On the basis of chemical composition,matter is divided into three types ; elements,compounds and…

Q: A mixture of KClO₃ and KCl with a mass of 0.950 g was heated to produce O₂. After heating, the mass…

A: The balanced equation is as follows: 2KCIO3 (s) --> 2KCI(s) + 302 (g) The mass of the mixture (…

Q: The principal component of mothballs is naphthalene, a compound with a molecular mass of about 130…

A: Record the given information,

Q: 1. Given: Na + Cl, → NaCl Is the equation balanced? if NO, balance it! a. b. If 3.0 moles of Na are…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Write The Molecular Fotmula For The Following 1-Copper Sulfate 2-Phospours Pentabromide 3-Calicum…

A: Hello, since your question has multiple parts, we will solve the first question for you. If you want…

Q: Calculate the percent carbon by mass in phenol (C6H5OH). Show calculations, please

Q: The koala dines exclusively on eucalyptus leaves. Its digestivesystem detoxifies the eucalyptus oil,…

A: Empirical formula- The formula of compound which represent simplest whole number ratio of elements…

Q: Calculate the number of grams Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen

A: The reaction taking place will be 6 Li + N2 -----> 2 Li3N hence from the above reaction we can…

Q: 2. How many grams of Cu,S can be produced from 1.2 g Cu if the percentage yield of the reac- tion is…

A: As per bartlyby's policy, only first question can be solved in case of multiple questions.

Q: A certain blue solid contains 36.84% N. What is the empirical formula of this compound?

A: Solving only first question in accordance with guidelines. Oxide of nitrogen is blue coloured solid.…

Q: A 16.35mg sample of unknown compound A produced 48.05mg of CO2 and 14.05mg of H2O when subjected to…

Q: Mass % of H in ammonium bicarbonate

A: Given Name of Compound = Ammonium bicarbonate Mass % of H = ?

Q: A 0.235 g sample of Manganese (Mn) was heated in a crucible and produced 0.372 g of a compound…

A: Given: Mass of Manganese= 0.235 g Mass of compound, MnxOy= 0.372 g To estimate: Empirical formula of…

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

100%

A 0.2356 g sample containg only NaCl (58.44 g/mol) and
BaCl, (208.23 g/mol) yielded 0.4637 g of dried AgCl
(143.32 g/mol). Calculate the percent of each halogen
compound in the sample.

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

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

A 0.2356 g sample containing only NaCl (58.44g/mol) and BaCl2 (208.23 g/mol) yielded0.4637 g of dried AgCl (143.32 g/mol).Calculate the percent of each halogencompound in the sample.
An impure sample of table salt that weighed 0.8421 g when dissolved in water and treated with excess AgN03 formed 2.044 g of AgCl. What percentage of NaCl is in the impure sample?
How to calculate theoretical and percent yield. My values are: .152 g magnesium turnings, 1.10 g of bromobenze, 5 g of dry ice. mass of obtained product = .515 g
What mass of AgI can be produced from a 0.532 g sample that assays 20.1% of AlI3?
a 0.2356g sample containing only NaCl (58.44 g/mol) and bacl2 (208.23g/mol) yielded 0.4637 g of dried AgCl (143.32 g/mol). calculate the percent of each halogen compound in the sample
Seashells are made up of mostly CaCO3 (100.09 g/mol) and a substance called chitin which contains C, H, O and N. To determine the percentage of CaCO3present in a seashell, gravimetric analysis is performed by dissolving a shell in acid followed by treatment with NaC2O4 (134 g/mol) to produce solid CaC2O4 (128.1 g/mol). If a 514 g seashell found in Ocean City, MD undergoes this analysis to produce 598 g of CaC2O4, what is the percentage of CaCO3 in the shell? Assume 100% yield for the reaction. Report your answer to the tenths place and do not include the % sign.
An impure sample of table salt that weighed 0.8421grams when dissolved in water and treated with excess AgNO3 formed 2.044 grams of AgCl. What percent of NaCl is in the impure sample?
A 0.2356 g sample containing only NaCl ( 58.44g/mol ) and BaCl 2 (208.23g/mol) yielded0.4637 g of dried AgCl (143.32g/mol). Calculate the % of each halogen compound in thesample. Let x be the mass of NaCl in grams and y be the mass of of BaCl 2 in grams.
In the preparation of Alum, we used (3 mole) reacted with (25 ml) of (1 M) KOH solution and the resulting mass of Alum was (8.5 gm). Caleulate the percent (%) of Alum yield? (M.wt: K=39, Al-27, S-32, H=1).
1.) If I mixed 50g of aluminum sulphate and 50g of calcium hydroxide, which is the limiting reagent? Determine the amount of excess reagent if any. If the percent yeild is only 75%, how much is the actual yeild? 2.) What is the value in K of 400 R? 3.) How many grams of nickel are in a 3.4x10^27 nickel atoms? 4.) Why is there a need to balance chemical equations? Support your answer with a scientific basis.
Phosphoric acid can be prepared from phosphorus triiodide according to the reaction: Pl3 (s) + H2O(l) -> H3PO4(aq) + HI(g) If 150 g of PI3 (MM = 411.7 g/mol) is added to 250 mL OF H2O (g/mol), d = 1.00 g/mL), Identify which will be limiting and excess reagents. How many grams of H3PO4 (MM = 97.99 g/mol) will be produced theoretically?
Pb(C2H3O2)2(aq) + H2O(l)+CO2(g)---PbCO3(s)+HC2H3O2(aq) suppose a aqueous solution containing 1.40 g of lead(ii) acetate is treated with 5.80(g) of carbon dioxide. Calculate the theoretical yield of lead carbonate