### Precipitation of Lead IonsLead ions can be precipitated from a solution with KCl according to the reaction:\[ \text{Pb}^{2+} \text{(aq)} + 2\text{KCl(aq)} \rightarrow \text{PbCl}_2 \text{(s)} + 2\text{K}^+ \text{(aq)} \]### Reaction DetailsWhen 34.3 g of KCl is added to a solution containing 25.8 g of \(\text{Pb}^{2+}\), PbCl₂(s) forms. The solid is filtered and dried, and it is found to have a mass of 30.9 g.### Calculating Percent Yield**Part C: Determine the percent yield for the reaction.**Express your answer in percent to three significant figures.#### Formula for Percent Yield\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \]#### Given Data- Actual Yield: 30.9 g- **Theoretical Yield** (provided above): 25.8 g**Calculation:**1. **Identify the masses of reagents and products:** - Actual yield of PbCl₂(s): 30.9 g - Theoretical yield of PbCl₂(s): 25.8 g2. **Determine the percent yield:** \[ \text{Percent Yield} = \left( \frac{30.9 \, \text{g}}{25.8 \, \text{g}} \right) \times 100 \approx 119.77\% \]3. **Round to three significant figures:** \[ \text{Percent Yield} \approx 119.8\% \]**Inputs for Calculation:**\[\text{\% yield} = \boxed{ \quad } \%\] Magnesium oxide can be made by heatingmagnesium metal in the presence of the oxygen. Thebalanced equation for the reaction is:2Mg(s) + O2(g) → 2MgO(s)When 12.9 g Mg reacts with 14.0 g O2, 12.5 g MgOis collected.The theoretical yield is determined from the limiting reactant. The mass of Mgmoles of MgO to grams of MgO.- Part CDetermine the percent yield for the reaction.Express your answer as a percent.[ΨΕΙ ΑΣΦÚ?%2

Solution :-“Since you have posted multiple questions, we will provide the solution only to the…

Lead ions can be precipitated from solution with KCl according to the reaction: Pb²+ (aq) + 2KCl(aq) → PbCl₂ (s) + 2K+ (aq) When 34.3 g KCl is added to a solution containing 25.8 g Pb2+, PbCl2 (s) forms. The solid is filtered and dried and found to have a mass of 30.9 g. theoretical yield of PbCl2 = 25.8 g Ph Part C % yield = X Determine the percent yield for the reaction. Express your answer in percent to three significant figures. ΠΫΠΙ ΑΣΦ 1 mol Pb2+ 1 mol 1 met X 207.2 g Pb²+ 2 ? %

Lead ions can be precipitated from solution with KCl according to the reaction: Pb²+ (aq) + 2KCl(aq) → PbCl₂ (s) + 2K+ (aq) When 34.3 g KCl is added to a solution containing 25.8 g Pb2+, PbCl2 (s) forms. The solid is filtered and dried and found to have a mass of 30.9 g. theoretical yield of PbCl2 = 25.8 g Ph Part C % yield = X Determine the percent yield for the reaction. Express your answer in percent to three significant figures. ΠΫΠΙ ΑΣΦ 1 mol Pb2+ 1 mol 1 met X 207.2 g Pb²+ 2 ? %

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

Similar questions

TReferences] A student titrates an unknown amount of potassium hydrogen phthalate (KHCgH,O, often abbreviated KHP) with 22.07 mL of a 0.1800-M N&OH solution. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution? Mass
How many grams of Cu(OH)2 will precipitate when excess Ba(OH)2 solution is added to 74.0 mL of 0.786 M CuSO4 solution? CuSO4 (aq) + Ba(OH)2 (aq) → Cu(OH)2 (s) + BaSO4 (aq) g
A quality control technician needs to determine the percentage Arsenic (As) in particular pesticide.The pesticide is dissolved and all of the arsenic present is converted to arsenate ions (AsO43-). Then the amount of AsO43- is determined by titrating with a solution containing silver ions (Ag+). The silver reacts with the arsenate according to the net ionic equations: 3 Ag+ + AsO43- → Ag3AsO4 When a 1.22 g sample of pesticide was analyzed this way, it required 25.0 mL of 0.102 M Ag+ solution to precipitate all of the AsO43-. What was the mass percentage of arsenic in the pesticide?
One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 200.mL sample of groundwater known to be contaminated with iron(III) chloride, which would react with silver nitrate solution like this: FeCl3 (aq) + 3AgNO3 (aq) →3AgCl (s) + (FeNO3)3 (aq) The chemist adds 48.0mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 7.5mg of silver chloride. Calculate the concentration of iron(III) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits.
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s) + CuSO4 (aq) → Cu (s) + FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 73.mg . Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.
esc 100. mL of 0.10 M CaCl₂ is mixed with 50.0 mL of a 0.10 M solution of either Al₂(SO4)3, Na₂SO4, or AgNO3. 1.36 g of precipitate is produced. Is the solution Al₂(SO), Na₂SO, or AgNO₂? Fn Al₂(SO)₂(aq) + 3CaCl(aq) → 3CaSO4(s) + 2 AICI₂ (aq) 3 Select the single best answer. Na₂SO (aq) + CaCl₂(aq) 2AgNO3(aq) + CaCl₂(aq) → ⒸAL₂(SO4)3 O Na₂SO4 O AgNO3 Continue 61°F Partly cloudy CaCl₂(aq) → CaSO (s) + 2 NaCl(aq) 4 F1 3 F2 F3 2AgCl(s) + 2AgCl(s) + Ca(NO3)₂ (aq) X Ś DII F4 Search F5 S F6 F7 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A P 8 F8 > H F9 DOLL prt sc F10 home Submit Assig F11 end F12 in
A 1.50 g sample of KCl is dissolved in 36.0 mL of water. The resulting solution is then added to 32.0 mL of a 0.470 M CaCl2 (aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution. Concentration of K* ions = M Concentration of Ca2+ ions = M Concentration of Cl ions = M
One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate, Suppose an EPA chemist tests a 200 mL sample of groundwater known to be contaminated with iron(III) chloride, which would react with silver nitrate solution like this: FeCl,(aq) + 3 AgNO,(aq) 3 AgCl(s) + Fe(NO₂),(ag) The chemist adds 21.0 mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 3.3 mg of silver chloride. Calculate the concentration of iron(III) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits. e -12 D.P C P
Classify each chemical reaction: Ba (CIO,),(s) → BaCl,(s) + 30, (8) KOH(aq) + HBrO (aq) 1 reaction CuSO4 (aq) + Zn CrO4 (aq) K BrO (aq) + H₂O (1) CH₂OCH₂ (1) + 30₂(g) → 2CO₂(g) + 3H₂O(g) ZnSO4 (aq) + Cu Cro(s) type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition 000 000 000 precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base
For each of the reactions, calculate the mass (in grams) of the product formed when 15.67 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant. 2K(s)+Cl2(g)−−−−−→2KCl(s) 2K(s)+Br2(l)−−−−−→2KBr(s) 4Cr(s)+3O2(g)−−−−−→2Cr2O3(s) 2Sr(s)−−−−+O2(g)→2SrO(s)
Sodium bicarbonate reacts with hydrochloric acid in a gas-forming reaction to produce aqueous sodium chloride, water, and carbon dioxide gas NaHCO3(s) + HCl(aq)→NaCl(aq) + H2O(l) + CO2(g) Determine the mass of CO2 gas produced when 8.89 g of NaHCO3 is added to a solution that contains 5.15 g of HCl.
Hydrobromic acid dissolves solid iron according to the following reaction: Fe(s)+2HBr(aq)→FeBr2(aq)+H2(g) A.) What mass of HBr (in g) would you need to dissolve a 2.6−g pure iron bar on a padlock? Express your answer using two significant figures. B.)What mass of H2 would be produced by the complete reaction of the iron bar? Express your answer using two significant figures.