The percent chloride in an unknown sample may be determined by gravimetric methods. Suppose a 0.6789g...
The percent chloride in an unknown sample may be determined by gravimetric methods. Suppose
a 0.6789g sample of an unknown chloride sample was dissolved and AgCl is precipitated by adding
AgNO3 solution. The precipitate was filtered, ignited, and found to weigh 0.3333g. What was the
percent chloride in the sample?
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The percent chloride in an unknown sample may be determined by
gravimetric methods. Suppose
a 0.6789g...
A chloride unknown sample weighing 0.4213 g is dissolved in acidic solution and is treated with...
A chloride unknown sample weighing 0.4213 g is dissolved in acidic solution and is treated with the precipitating solution. The silver chloride precipitate that forms is filtered, washed, dried and weighed. The mass of the silver chloride obtained is 0.5915 g. Calculate the % Cl in this unknown sample. Molar Masses: AgCl = 143.35 g/mol, Cl– = 35.45 g/mol
Chloride in a water sample can be determined indirectly by atomic absorption spectrometry by precipitating chloride...
Chloride in a water sample can be determined indirectly by
atomic absorption spectrometry by precipitating chloride as AgCl(s)
with a measured amount of AgNO3 that is excess of the chloride
content of the sample. The AgNO3 is added and the sample is
centrifuged. The remaining Ag+ in the solution (supernatant) is
quantified and the chloride is measured by assuming that chloride
was quantitatively precipitated.
Chloride in a water sample can be determined indirectly by atomic absorption spectrometry by precipitating chloride...
1. A 0.4187 g sample of a pure soluble chloride compound is dissolved in water, and...
1. A 0.4187 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 0.9536 g. What is the mass percentage of chlorine in the original compound? ________% 2. A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide...
12.0 mL of a 437.1 mM AgNO3 solution is added to a 20.0 mL sample containing...
12.0 mL of a 437.1 mM AgNO3 solution is added to a 20.0 mL sample containing an unknown chloride ion concentration to precipitate Cl- as AgCl. The AgCl solid is removed and excess Ag+ is titrated with a standard 137.0 mM KSCN solution in the presence of Fe3+. After 2.5 mL of the standard solution have been added, all Ag+ has precipitated as AgSCN and the red complex FeSCN2+ forms. What is the chloride ion concentration in the sample to...
5. Suppose that a 0.2045g Unknown sample is analyzed using the procedure for this lab experiment....
5. Suppose that a 0.2045g Unknown sample is analyzed using the procedure for this lab experiment. If the initial crucible weight is 3.0531g and the final crucible weight is 3.5016g. what is the%Cl by mass of the Unknown sample? Show all work. PRELAB: Experiment 5: Gravimetric Analysis is the most common method for isolating and analyte for gravimetric analysis 2. Nucleations sites are important to insure the formation of large This is achieved more efficiently by mixing slowly and keeping...
16. A solid sample contains only NaCl and KCI. A 0.5623 g sample of this material...
16. A solid sample contains only NaCl and KCI. A 0.5623 g sample of this material was dissolved in water. An excess of 0.10 M AgNO3 solution was added to precipitate out AgCl: Agt(aq) + Cl(aq) → AgCl(s) The AgCl was filtered, dried, and weighed. 1.2691 g of AgCl was obtained. What was the wt% of NaCl and the wt% of KCl in the sample?
Gravimetric Analysis of a Chloride Salt QUESTIONS 1. The following percentages of chloride were found: 32.52%,...
Gravimetric Analysis of a Chloride Salt QUESTIONS 1. The following percentages of chloride were found: 32.52%, 32.14%, 32.61%, and 32.75% (a) Find the mount, the standard deviation, and the relative standard deviation (b) Can any result be discarded? 2. Barium can be analyzed by precipitating it as BaSO, and determining the mass of the precipitate. When a 0.269 g sample of a barium compound was treated with excess H,SO, 0.0891 g of BaSo, formed. What percentage of barium is in...
The chloride ion concentration in a solution may be determined by the precipitation of lead chloride....
The chloride ion concentration in a solution may be determined by the precipitation of lead chloride. Pb2+(aq) + 2CI+(aq) —>PbCl2(s) A student finds that 23.52 mL of 0.6250 M lead nitrate is needed to precipitate all of the chloride ion in a 25.00-mL sample of an unknown. What is the molarity of the chloride ion in the student's unknown? M
GRAVIMETRIC ANALYSIS Gravimetric Analysis-A type of analysis in which a sample is subjected to some treatment...
GRAVIMETRIC ANALYSIS Gravimetric Analysis-A type of analysis in which a sample is subjected to some treatment that causes a change in the physical state of the analyte that permits its separation from the other components of the sample. Mass measurements of the isolated analyte used along with the known stoichiometry of the compounds involved, permit calculation of the analyte concentration. Commonly, the analyte is separated by subjecting it to a precipitation reaction. -EXAMPLE a) A 0.4550-g solid mixture containing MgS0,...
A gravimetric analysis was preformed on an unknown chloride sample in the laboratory to try and...
A gravimetric analysis was preformed on an unknown chloride sample in the laboratory to try and determine the identity of the solid. if the results of the experiment were 32.52%, 32.14%, 32.61 and 41.29 what is the mean, standard deviation and relative standard deviation of these experiments? finally, can any of these results be discarded and if so why?
Chloride in a water sample can be determined indirectly by
atomic absorption spectrometry by precipitating chloride as AgCl(s)
with a measured amount of AgNO3 that is excess of the chloride
content of the sample. The AgNO3 is added and the sample is
centrifuged. The remaining Ag+ in the solution (supernatant) is
quantified and the chloride is measured by assuming that chloride
was quantitatively precipitated.
Chloride in a water sample can be determined indirectly by atomic absorption spectrometry by precipitating chloride...
5. Suppose that a 0.2045g Unknown sample is analyzed using the procedure for this lab experiment. If the initial crucible weight is 3.0531g and the final crucible weight is 3.5016g. what is the%Cl by mass of the Unknown sample? Show all work. PRELAB: Experiment 5: Gravimetric Analysis is the most common method for isolating and analyte for gravimetric analysis 2. Nucleations sites are important to insure the formation of large This is achieved more efficiently by mixing slowly and keeping...
16. A solid sample contains only NaCl and KCI. A 0.5623 g sample of this material was dissolved in water. An excess of 0.10 M AgNO3 solution was added to precipitate out AgCl: Agt(aq) + Cl(aq) → AgCl(s) The AgCl was filtered, dried, and weighed. 1.2691 g of AgCl was obtained. What was the wt% of NaCl and the wt% of KCl in the sample?
Gravimetric Analysis of a Chloride Salt QUESTIONS 1. The following percentages of chloride were found: 32.52%, 32.14%, 32.61%, and 32.75% (a) Find the mount, the standard deviation, and the relative standard deviation (b) Can any result be discarded? 2. Barium can be analyzed by precipitating it as BaSO, and determining the mass of the precipitate. When a 0.269 g sample of a barium compound was treated with excess H,SO, 0.0891 g of BaSo, formed. What percentage of barium is in...
The chloride ion concentration in a solution may be determined by the precipitation of lead chloride. Pb2+(aq) + 2CI+(aq) —>PbCl2(s) A student finds that 23.52 mL of 0.6250 M lead nitrate is needed to precipitate all of the chloride ion in a 25.00-mL sample of an unknown. What is the molarity of the chloride ion in the student's unknown? M
GRAVIMETRIC ANALYSIS Gravimetric Analysis-A type of analysis in which a sample is subjected to some treatment that causes a change in the physical state of the analyte that permits its separation from the other components of the sample. Mass measurements of the isolated analyte used along with the known stoichiometry of the compounds involved, permit calculation of the analyte concentration. Commonly, the analyte is separated by subjecting it to a precipitation reaction. -EXAMPLE a) A 0.4550-g solid mixture containing MgS0,...
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