To solve stoichiometry problems, you must always calculate numbers of moles. Recall that molarity, M, Is equal to the concentration in moles per liter: M= mol/L. When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of solution according to the equation AGNO3 (aq) + KCI(aq)→AgCl(s) + KNO3(aq) Part A What mass of silver chloride can be produced from 1.47 L of a 0.156 M solution of silver nitrate? Express your answer with the appropriate units. • View Available Hint(s) HẢ mass of AgCI = Value Units Submit Part B P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy I Permissions I Contact Us | A 10:05

To solve stoichiometry problems, you must always calculate numbers of moles. Recall that molarity, M, Is equal to the concentration in moles per liter: M= mol/L. When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of solution according to the equation AGNO3 (aq) + KCI(aq)→AgCl(s) + KNO3(aq) Part A What mass of silver chloride can be produced from 1.47 L of a 0.156 M solution of silver nitrate? Express your answer with the appropriate units. • View Available Hint(s) HẢ mass of AgCI = Value Units Submit Part B P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy I Permissions I Contact Us | A 10:05

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

Complete (where necessary) and balance the following equation. Write the stoichiometric equation, then write the equation in ionic and net ionic form. __ Cu(NO3)2 (aq) + __ NaOH (aq) → Cu(OH)2 (s) + __________
1. For each of the following reactions, identify the category of reaction, balance reaction, and describe how you knew a reaction took place. To indicate an already balanced reaction, write balanced above the reaction. Reaction 1 Balance: H2O(1) + NO2(g) Cu(s) Cu(NO3)2(aq) + HNO3(aq) + Reaction Category: How did you identify a reaction took place? Reaction 2 Balance: Cu(NO3)2(aq) + NaOH(aq) – Cu(OH)2(s) + NaNO3(aq) Reaction Category: How did you identify a reaction took place? OhoW Reaction 3 Balance: Cu(OH)2(s) → CuO(s) + H2O(1) Reaction Category: How did you identify a reaction took place? Reaction 4 Balance: CuO(s) + H2SO4(aq) – CuSO4(aq) + H2O() Reaction Category: How did you identify a reaction took place? Reaction 5 Balance: CuSO4(aq) + Zn(s) → ZNSO4(aq) + Cu(s) Reaction Category: How did you identify a reaction took place?
Potassium iodide reacts with lead(II)(II) nitrate in the following precipitation reaction: 2KI(aq)+Pb(NO3)2(aq)→2KNO3(aq)+PbI2(s)2KI(aq)+Pb(NO3)2(aq)→2KNO3(aq)+PbI2(s) What minimum volume of 0.218 MM potassium iodide solution is required to completely precipitate all of the lead in 145.0 mLmL of a 0.150 MM lead(II)(II) nitrate solution?
Students in a chemistry lab are making the compound cobalt (II) carbonate. It can be made byreacting sodium carbonate solution with cobalt (II) chloride solution.Calculate the volume of 1.0 mol/L cobalt (II) chloride solution required to completely reactwith 250 mL of 1.5 mol/L sodium carbonate.Na2CO3 (aq) + CoCl2 (aq) → CoCO3 (s) + 2 NaCl (aq)
QUESTION 11 A student titrates 26.5 mL of a sulfuric acid solution with 0.750 M NaOH. The color change indicates that it takes exactly 47.9 mL of the NaOH solution for the reaction to go to completion. What was the concentration of the original H₂SO4 solution? (Write your answer in 3 significant figures)? The balanced equation is: H₂SO4 (aq) + 2 NaOH (aq) → 2 H₂O (1) + Na2SO4 QUESTION 12 Metals frequently adopt solid-state structures which can be described is terms of cubic, face-centered cubic or body-centered cubic unit cells with metal atoms located at the lattice points. Ni is face-centered cubic, Fe is body-centered cubic and Ga is simple cubic. Which description below correctly indicates the number of metal atoms per unit cell? OA. Fe 4 OB. Fe 1 OC. Fe 2 OD. Fe 9 OE. Fe 14 NN NN N Ni Ni Ni 4 Ni 14 Ni 9 Ga 1 Ga 4 Ga 1 Ga 8 Ga 8 save all answers.
If 37.70 mL of HCl is required to titrate 2.180 g of Na2CO3 according to the following equation, what is the concentration (mol/L) of the HCl solution? Na2CO3(aq) + 2 HCl(aq) → 2 NaCl(aq) + CO₂(g) + H₂O(l) Concentration = M
While working in a lab, Ronan reacts 50.0 mL of 0.320 mol/L Na2CO3 (aq) with 85.0 mL of 0.210 mol/L AlCl3 (aq). Calculate the mass of Al2(CO3)3 precipitate that forms when the reaction is complete 3 Na2CO3 (aq) + 2 AlCl3 (aq) → Al2(CO3)3 (↓) + 6 NaCl (aq)
Toxic chromate can be precipitated from an aqueous solution by bubbling sulfur dioxide through the solution. How many grams of sulfur dioxide are required to treat 1.1 L of 0.12 M chromate? 2 CrO42-(aq) + 3 SO2(g) + 4 H+(aq) → Cr2(SO4)3(s) + 2 H2O(l) Your answer should have 2 sig figs. Molar Masses if needed: H2O 18.02 g/mol, Cr2(SO4)3 392.21 g/mol, SO2 64.07 g/mol
QUESTION 22 A student titrates 55.2 mL of a sulfuric acid solution which contains 1.40 M NaOH. The color change indicates that it takes exactly 37.4 mL of the NaOH solution for the reaction to go to completion. What was the concentration of the original H₂SO4 solution? (Write your answer in 3 significant figures)? The balanced equation is: H2SO4 (aq) +2 NaOH(aq) → 2 H20 (1) + Na2SO4 U (atomic mass 235.0439) is 45.84% and the QUESTION 23 A sample of waste from a nuclear reactor contains an unnatural distribution of isotopes of uranium. The abundance of 235 ( abundance of 238 (atomic mass 238.0508) is the remainder. What would the average atomic mass of uranium be in this sample? (Write your answer in 4 significant figures. Do not include units.)
Write an ionic equation and a net ionic equation for the following molecular equation.BaCl2 (aq) + K2SO4 (aq) → BaSO4 (s) + 2KCl (aq)
Which equation best represents the net ionic equation for the reaction that occurs when aqueous solutions of potassium phosphate and manganese(II) nitrate are mixed? 3Mg2+(aq) + 2PO43–(aq) → Mg3(PO4)2(aq) 2K3PO4(aq) + 3Mg(NO3)2(aq) → Mg3(PO4)2(s) + 6KNO3(aq) 2K3PO4(aq) + 3Mg2+(aq) → Mg3(PO4)2(s) + (K+)6(aq) 2K+(aq) + Mg(NO3)2(aq) → 2KNO3(aq) + Mg2+(aq) 3Mg2+(aq) + 2PO43–(aq) → Mg3(PO4)2(s)
In the following reaction, 35.0 mL of 0.150 M magnesium bromide solution reacts with excess silver nitrate to form a precipitate. What is the expected mass of AgBr in grams? (molar mass of AgBr = 187.77 g/mole) MgBr2(aq) + 2AgNO3(aq) --> 2AgBr(s) + Mg(NO3)2(aq) Question 11 options: 0.985 g 0.493 g 1.97 g 986 g none of these