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 8.0 M HCl(aq) to 200.0 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 Mass of filter paper + AgCl(s) precipitate after drying (a) Calculate the number of moles of AgCl(s) that precipitated. (The molar mass of AgCl is 143 g/mol). (b) Assuming that all of the Ag'(aq) ions precipitated, calculate the original molarity of Ag (aq) in the solution before HCl(aq) was added. 0.10 M NaCl O = Na* OF AR 0.851 g 2.311g 7M ARNO, -NO₂ (c) lons in a certain volume of 0.10 M NaCl(aq) are represented in the box above on the left. In the box above on the right, draw a particulate diagram that represents the ions in the same volume the original molarity of Ag*(aq) in the solution before HCl(aq) was added
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 8.0 M HCl(aq) to 200.0 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 Mass of filter paper + AgCl(s) precipitate after drying (a) Calculate the number of moles of AgCl(s) that precipitated. (The molar mass of AgCl is 143 g/mol). (b) Assuming that all of the Ag'(aq) ions precipitated, calculate the original molarity of Ag (aq) in the solution before HCl(aq) was added. 0.10 M NaCl O = Na* OF AR 0.851 g 2.311g 7M ARNO, -NO₂ (c) lons in a certain volume of 0.10 M NaCl(aq) are represented in the box above on the left. In the box above on the right, draw a particulate diagram that represents the ions in the same volume the original molarity of Ag*(aq) in the solution before HCl(aq) was added
Transcribed Image Text:A student investigates various properties f 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 8.0 M HCl(aq) to 200.0 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
Mass of filter paper + AgCl(s) precipitate after drying
(a) Calculate the number of moles of AgCl(s) that precipitated. (The molar mass
of AgCl is 143 g/mol).
(b) Assuming that all of the Ag' (aq) ions precipitated, calculate the original molarity
of Ag*(aq) in the solution before HCl(aq) was added.
0.10 M NaCl
Ⓒ = Nat O Ag
0.851 g
2.311g
7M AgNO3
Cr
NO₂
(c) lons in a certain volume of 0.10 M NaCl(aq) are represented in the box above on
the left. In the box above on the right, draw a particulate diagram that represents the
ions in the same volume the original molarity of Ag*(aq) in the solution
before HCl(aq) was added
(d) The calculated concentration of Ag*(aq) from the student's data is higher than the
actual concentration of the original solution. The student claims that the calculated
concentration is too high because the original solution contained
some Na* (aq) impurities that resulted in some NaCl(s) precipitating along with
the AgCl(s). Do you agree or disagree? Justify your answer.
The student then conducts an experiment to determine the solubility of AgCl in
a 2.5 M NaCl solution at various temperatures. Some AgCl(s) remains in the container
at all temperatures studied. The data are plotted on the graph below.
0.9
Mass of AgCl Dissolved
(g/1000 g solution
0.8-
0.7
0.6-
0.5
0.4+
70
75 80 85 90 95 100
Temperature (°C)
(e) A 1000. sample of a saturated solution at 95°C is cooled to 85°C. Determine the
mass of AgCl(s) that would precipitate out of the solution.
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