4. When a 0.2565-g sample of impure potassium chloride was treated with an excess of AgNO30.2912 g of AgCl was produced. Calculate the percentage of KCl in the sample. 3. The mercury in a 1.0023-g soil sample was precipitated with an excess of paraperiodic acid,HŞIO6:SHg* (») 2H:IO6 (a) → Hgs(IO6)26) + 10OH“ (9)The precipitate was filtered, washed free of precipitating agent, dried, and weighed, and 0.4996 gwas recovered. Determine the %w/w of Hg.Cl2 in the sample.

Answered: Image /qna-images/answer/55f41433-e1fd-4ef9-8747-ae9bb622af2a.jpg

Answered: . When a 0.2565-g sample of impure…

. When a 0.2565-g sample of impure potassium chloride was treated with an excess of 0.2912 g of AgCl was produced. Calculate the percentage of KCI in the sample.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Suppose 74.0 mL of 0.370 M CoCl2 solution is added to 35.0 mL of 0.820 M NiCl2 solution. Calculate…

A: The molarity of CoCl2 solution is = 0.370 M The volume of CoCl2 solution is = 74.0 mL The molarity…

Q: a) Does a reaction occur when aqueous solutions of manganese(II) sulfate and barium bromide are…

A: Dear student! as per honor code, we only answer up to 3 sub-parts, we'll answer the first three.…

Q: Calculate the volume (mL) of 1.0 M metal nitrate solution required to prepare 5.0 g of the COPPER…

A: The balanced chemical equation is, Cu(NO3)2 ---> Cu2+ + 2NO3- From this reaction we can conclude…

Q: A sample of 0.3207 g of an ionic compound containing the bromide ion (Br) is dissolved in water and…

A: Number of moles is calculated by dividing given mass with molecular mass.

Q: yttrium (III) nitrate, prepared a solution of the metal salt by dissolving .7168 g of yttrium (III)…

A: Given that, Mass of Yttrium (III) nitrate = 0.7168 grams Volume of dissolution = 200 mL…

Q: A 0.5683 g sample of a pure soluble bromide compound is dissolved in water, and all of the bromide…

Q: In a neutralization reaction, 50.00 mL of 0.8500 M phosphoric acid reacts with 2.500 g of magnesium…

A: The answers to the first three questions can be given as - Given Data -

Q: Treatment of a 0.3500-g sample of impure potassium chloride with an excess of AgNO3 resulted in the…

A: Mass of impure potassium chloride (KCl) = 0.3500 g Mass of AgCl formed = 0.3640 g Excess reactant:…

Q: How many molecules of hydrosulfuric acid could be reacted by 2.330 g scandium (III) hydroxide?

A: This problem can be solved by comparing stoichiometric ratio of hydrosulfuric acid and scandium(iii)…

Q: How many grams of PbBr2 will precipitate when excess BaBr2 solution is added to 78.0 ml of 0.524 M…

A: Recall the reaction that will occur here PbNO32 + BaBr2 →PbBr2 + BaNO32 Given that 78.0 ml of 0.524…

Q: percentage KCl

Q: What mass of Fe(OH)3 would be produced by reacting 75.0 mL of a 0.0734 M Fe(NO3)3 solution with 125…

A: Given: Concentration (molarity) of Fe(NO3)3 = 0.0734 M Volume of Fe(NO3)3 = 75.0 mL Concentration…

Q: A student wishes to determine the mass percentage of barium in a 2.016g sample. The student…

A: Given : Molarity of H2SO4 = 0.20M Volume of H2SO4 = 20mL

Q: .. When 125 mL of 0.150 M Pb(NO3)2 is mixed with 145 mL of 0.200 M bBr. is collected. Calculate the…

Q: How many grams of chlorine gas can be produced from the electrolytic decomposition of 874 g of…

A: The reaction of electrolytic decomposition of calcium chloride - CaCl2aq →Cas + Cl2g

Q: A 12.3 g sample of an alloy of Mg and Al produces 1.66 mol of H2 when added to excess HCl. What…

A: Given: Total mass of alloy = 12.3 g. And moles of H2 produced = 1.66 mol. Assuming that there are…

Q: Chemistry Question

A: Given: Mass of BeCO3 = 44.0 g Molar mass of BeCO3 = 69.0211 g/mol Molar mass of CO2 = 44.01 g/mol

Q: Determine the mass of sulfate in the powder (in grams) if 2.47 g of barium sulfate (BaSO4) formed.…

A: The question is based on the concept of quantitative estimation of sulphate present in the given…

Q: Masses : Ca = 40.08 g S= 32.07 g O= 16.00 g A 35.0 mL sample of CaSO4 was evaporated to…

Q: Write a balanced chemical equation for this reaction. Hydrogen sulfide gas and aqueous iron(II)…

A: A balanced chemical equation has equal number of atoms for each element involved in the reaction are…

Q: When an aqueous solution of 6.71 g of barium chloride was added to an aqueous solution of 7.77 g of…

A: The reaction between barium chloride and potassium chromate is shown below, The given grams are…

Q: 0.8838-g sample of an ionic compound containing bromide ions and an unknown metal cation is…

A: Weight of ionic compound = 0.8838 gm Weight of precipitate (AgBr) = 1.573 gm

Q: A 0.764-g sample containing barium ions is completely dissolve in water and treated with excess…

A: The question is based on the concept of quantitative analysis. we need to calculate percentage…

Q: The molar mass of potassium hydrogen phthalate is 204.22 grams per mole. To determine the molarity…

A: Reaction:' KHP (aq) + NaOH (aq) --> KNaP (aq) + H2O (l) Given:' mass of KHP = 1.32 g molar mass…

Q: Determine the mass of sodium nitrate produced when 0.73 g of aqueous nickel(II) nitrate reacts with…

A: NOTE : There is a typing error in question. The solid will be of nickel (II) hydroxide and and…

Q: A sodium sulfate solution is added to a 25.0 mL sample of a solution containing Ba2+ ions until no…

A: To calculate the molarity of the Ba2+ ions, first of all, we calculate the moles of barium sulfate.

Q: A 25.0-g sample of garden compost was analyzed for chloride content. The sample was dissolved in…

A: Given, Mass of garden sample = 25.0 g Mass of dried precipitate = 1.58 g

Q: How many grams of PbBr2 will precipitate when excess AlBr3 solution is added to 66.0 mL of 0.754 M…

A: Given: Concentration (molarity) of Pb(NO3)2 = 0.754 M Volume of Pb(NO3)2 = 66.0 mL molar mass of…

Q: . Barium-contaminated soil can be remediated by immobilization of the barium as alforsite,…

A: A) To calculate the weight percent of alforsite in the soil sample, you need to find the mass of the…

Q: IReferences Use the References to access important values if needed for this question. A 0.5684 g…

Q: A 0.8830 g sample of a mixture of NaCl and KCl is dissolved in water, and the solution is then…

A: Given : Mass of mixture = 0.8830 g And mass of AgCl produced = 1.913 g Molar mass of AgCl = Atomic…

Q: and

A: reaction occur when aqueous solutions of manganese(II)sulfate react with potassium carbonate.…

Q: 1. H2SO4. The resulting solution contained excess acid and required 15.85 mL of 0.09850 M NaOH for…

A: The balanced equations are CaCO3 + H2SO4 ----------> CaSO4 + CO2 + H2O H2SO4 + 2 NaOH…

Q: Write a balanced equation for the precipitation reaction that occurs when aqueous solutions of…

A: The objective of the question is to write a balanced chemical equation for the precipitation…

Q: When 75.0 mL of a magnesium nitrate solution of unknown concentration had an excess of sodium…

A: Magnesium nitrate reacts with sodium hydroxide to form the precipitate of magnesium hydroxide and…

Q: Zinc and magnesium react with hydrochloric acid to produce the metal chlorides and hydrogen gas. A…

Q: What mass of precipitate (in g) is formed when 20.5 mL of 0.300 M Ni(NO₃)₂ reacts with 23.5 mL of…

Q: Calculate the mass of calcium phosphate that will precipitate when excess sodium phosphate solution…

A: you have given - Calcium Nitrate concentration = 0.0132 M Calcium Nitrate Volume = 100 mL

Q: A sample of 0.3291 g of an ionic compound containing the bromide ion (Br) is dissolved in water and…

A: Given Mass of sample = 0.3291 g Mass of AgBr = 0.6905 g Moles of AgBr = mass of AgBrmolar mass of…

Q: After titration, 25 mL of a vinegar solution was found to contain .03 moles of acetic acid. Using a…

A: Volume = 25 ml Moles of acetic acid = 0.03 M

Q: In an experiment, you used 4.00 mL of 0.100 M Copper (II) Nitrate and converted it into Copper (II)…

A: Theoretical yield :- The maximum amount of product that can be produced as per balanced chemical…

Q: Pure platinum is too soft to be used in jewelry because it scratches easily. To increase the…

Q: a) What is the maximum amount of salt (in molecules) that can be produced when 35 mL of 0.102 M of…

A: 1.a) The reaction between strontium hydroxide and nitrous acid is an acid base reaction that leads…

Q: Write the balanced NET ionic equation for the reaction when aqueous manganese(ll) chloride and…

Q: Barium can be analyzed by precipitating it as BaS04 and determining the mass of the precipitate.…

A: Molar mass of Barium = 137.33 g/mol Molar mass o BaSO4 = 233.38 g/mol Given that: Mass of sample =…

Q: sample of an alloy containing only platinum and cobalt is reac Calculate the mass percent of…

Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

4. When a 0.2565-g sample of impure potassium chloride was treated with an excess of AgNO3
0.2912 g of AgCl was produced. Calculate the percentage of KCl in the sample.

3. The mercury in a 1.0023-g soil sample was precipitated with an excess of paraperiodic acid,
HŞIO6:
SHg* (») 2H:IO6 (a) → Hgs(IO6)26) + 10OH“ (9)
The precipitate was filtered, washed free of precipitating agent, dried, and weighed, and 0.4996 g
was recovered. Determine the %w/w of Hg.Cl2 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.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 3 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

Define how Solid lead (II) sulfide reacts with aqueous hydrochloric acid to produce solid lead (II) chloride and hydrogen sulfide gas.
20.0 mL of a 0.617 M lithium phosphide and 25.0 mL of a 0.592 M molybdenum (IV) chloride. What mass of solid, in grams, is formed?
Determine the limiting reactant and theoretical yield of the solid when 10.00 mL of a 1.00 M sodium sulfate solution is mixed with 18.00 mL of a 1.25M barium chloride solution to give solid barium sulfate and aqueous sodium chloride.
3. What mass of NaCl can be produced from 0.55 mol Cl2 in the following reaction? 2 Naa + Cle) → 2 NaCle) d. 88 g a. 0.55 g b. 1.1 g с. 64 g С.
A sample of 0.5220 g of an ionic compound containing the bromide ion (Br-) is dissolved in water and treated with an excess of AgNO3. If the mass of the AgBr precipitate that forms is 0.8965 g, what is the percent by mass of Br in the original compound?
Suppose that a solution prepared by dissolving 0.554 g of MgCl2 in about 30 mL of water is mixed with a solution that contains excess K2CO3 dissolved in about 30 mL of water. What is the theoretical yield (in grams) of MgCO3 in the precipitation reaction that occurs?
A sodium sulfate solution is added to a 25.0 mL sample of a solution containing Ba2+ ions until no more precipitate formed. The precipitate (BaSO4) is collected, dried, and weighed. If 1.59 g of the precipitate are obtained, what is the concentration (in M) of Ba2+ ions in the 25.0 mL sample? Your answer should have 3 sig. figs. Molar Masses: (Na2SO4: 142.05 g/mol) (Ba2+: 137.3 g/mol) (BaSO4: 233.37 g/mol)
2. Calculate the mass of the precipitate formed when 2.00 g of Barium Nitrate is mixed with an excess of Sodium Phosphatein water. Write out the balanced Molecular Equation .
What mass of copper II hydroxide precipitate is produced by the double displacement reaction in a solution of 2.67 g of potassium hydroxide with excess aqueous copper II nitrate?
1) Lead (I) nitrate reacts with sodium chloride. A) Write a balanced chemical equation to describe this reaction B) 100.0 mL of a lead (I) nitrate solution reacts with excess sodium chloride solution and produces 6.95 grams of precipitate. 2) Calculate the moles of the precipitate produced by the reaction. A) Calculate the moles of lead in the original solution. B) Calculate the molarity of the 100.0 mL lead (I) nitrate solution.
Masses : Ca = 40.08 g S= 32.07 g O= 16.00 g A 35.0 mL sample of CaSO4 was evaporated to dryness, leaving 0.967 g of residue. What was the molarity of the original solution? step by step please
A 0.4455 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCI by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 0.9496 g. What is the mass percentage of chlorine in the original compound? %