12:42Schoology1 /4 >O 157% OA student investigates various properties of silver compounds in the lab. First, the student carries outthe following procedure to determine the concentration of Ag* (aq) in a solution of AgNO3(aq). Thestudent adds an excess of 2.0 M HCl(aq) to 300.0 mL of the solution, causing AgCl(8) to precipitate.The precipitate is separated from the solution by filtering it through a pre-weighed piece of filter paper.The precipitate and filter paper are rinsed with distilled water, dried, and weighed. The data from theexperiment are given in the table below.Initial mass of filter paper0.650 gMass of filter paper + AgCl(s) precipitate after drying0.793 g(a) Calculate the number of moles of AgCl(s) that precipitated. (The molar mass of AgCl is143 g/mol).O Please respond on separate paper, following directions from your teacher.(b) Assuming that all of the Ag* (aq) ions precipitated, calculate the original molarity of Ag* (aq) inthe solution before HCl(aq) was added.O Please respond on separate paper, following directions from your teacher.(c) The calculated concentration of Ag+ (ag) from the student's data is lower than the actualconcentration of the original solution. The student claims that the calculated concentration is too lowbecause some of the AgCl(s) passed through the filter paper. Do you agree or disagree? Justify youranswer.O Please respond on separate paper, following directions from your teacher.After the experiment, the student learns that the precipitate, AgCl(s), is slightly soluble in water. Todetermine the solubility, the student mixes a sample of the precipitate with warm, distilled water tomake a saturated solution. The student finds the following equation for the dissolution of AgCl(s) inCapyrighe 201. The Cullepe nd. These mterials we pan of a Colu unl prgrm. Uor disikien of thee mrials oline in pri heyand yorwhel's paticipwien in the pogrm i prohibtedPage 1 of 9AP OCollegolloardAP ChemistryTest BookletFinalwater and a Kap value at the temperature of the water.AgCl(s) 2 Ag*(aq) + Cl¯(aq)K, = 9.0 x 10–10(d) Calculate [Ag+] in the student's solution.O Please respond on separate paper, following directions from your teacher.(e) The value of Kp of another silver salt, AgF(s), is 2.0 × 10². If separate, saturated solutions ofAgF(8) and AgCI(s) are prepared, which solution will have the greater [Ag*]? Justify your answer.O Please respond on separate paper, following directions from your teacher.(f) The student finds the following particulate model of AgCl(s). Assuming the crystal structures aresimilar, how should the student modify the model to represent AgF(s)? Justify your answer in terms ofthe radius and arrangement of electrons in the ions.Ag*Ag+Ag+Ag+CF

Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

A student investigates various properties of silver compounds in the lab. First, the student carries out the following procedure to determine the concentration of Ag* (aq) in a solution of AgNO3 (aq). The student adds an excess of 2.0 M HC1(aq) to 300.0 mL of the solution, causing AgCl(s) to precipitate. The precipitate is separated from the solution by filtering it through a pre-weighed piece of filter paper. The precipitate and filter paper are rinsed with distilled water, dried, and weighed. The data from the experiment are given in the table below. Initial mass of filter paper 0.650 g Mass of filter paper + A£CI(a) precipitate after drying 0.793 g (a) Calculate the number of moles of AgCl(s) that precipitated. (The molar mass of AgCl is 143 g/mol). Please respond on separate paper, following directions from your teacher. (b) Assuming that all of the Ag* (aq) ions precipitated, calculate the original molarity of Ag* (aq) in the solution before HCI(aq) was added. Please respond on separate paper, following directions from your teacher. (e) The calculated concentration of Ag* (aq) from the student's data is lower than the actual concentration of the original solution. The student claims that the calculated concentration is too low because some of the AgCl(s) passed through the filter paper. Do you agree or disagree? Justify your answer. Please respond on separate paper, following directions from your teacher. After the experiment, the student learns that the precipitate, AgCI(s), is slightly soluble in water. To determine the solubility, the student mixes a sample of the precipitate with warm, distilled water to make a saturated solution. The student finds the following equation for the dissolution of AgCl(a) in

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...