A 0.5427 g mixture of KCN (MW=65.116 g/mol) and NaCN (MW=49.005 g/mol) was dissolved in water....
A 0.5427 g mixture of KCN (MW=65.116 g/mol) and NaCN (MW=49.005 g/mol) was dissolved in water. AgNO3 was added to the solution, precipitating all of the CN− in solution as AgCN (MW=133.886 g/mol). The dried precipitate weighed 1.264 g. Calculate the weight percent of KCN and NaCN
in the original sample.
KCN wt%=
%
NaCN wt%=
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A 0.5427 g mixture of KCN (MW=65.116 g/mol) and NaCN (MW=49.005
g/mol) was dissolved in water....
A 0.6689 g mixture of KCN (MW = 65.116 g/mol) and NaCN (MW = 49.005 g/mol)...
A 0.6689 g mixture of KCN (MW = 65.116 g/mol) and NaCN (MW = 49.005 g/mol) was dissolved in water. AgNO, was added to the solution, precipitating all of the CN in solution as AgCN (MW = 133.886 g/mol). The dried precipitate weighed 1.518 g. Calculate the weight percent of KCN and NaCN in the original sample. KCN wt% = NaCN wt% =
A 0.2150 g sample is dissolved and treated with excess AgNO3. The precipitate is filtered, washed,...
A 0.2150 g sample is dissolved and treated with excess AgNO3. The precipitate is filtered, washed, dried, and weighed. The mass of the product (AgCl) is 0.4587 g. What is the wt% of Cl in the original sample? The molecular weight of AgCl is 143.32 g/mol.
A sample containing a mixture of SrCl2·6H2O (MW = 266.62 g/mol) and CsCl (MW = 168.36...
A sample containing a mixture of SrCl2·6H2O (MW = 266.62 g/mol) and CsCl (MW = 168.36 g/mol) originally weighs 1.9715 g. Upon heating the sample to 320 °C, the waters of hydration are driven off SrCl2·6H2O, leaving the anhydrous SrCl2. After cooling the sample in a desiccator, it has a mass of 1.6811 g. Calculate the weight percent of Sr, Cs, and Cl in the original sample. 1) wt% Sr 2) wt% Cs 3) wt% Cl
Suppose a 12.42g mixture of NaCl and CaCl2 is dissolved in water. To this solution, an...
Suppose a 12.42g mixture of NaCl and CaCl2 is dissolved in water. To this solution, an excess of AgNO3 solution is added resulting in the formation of 31.12g of the precipitate. Calculate the % by mass of NaCl and CaCl2 in the original mixture. Show all work.
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
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?
Suppose a 12.42g mixture of NaCl and CaCl2 is dissolved in water. To this solution, an excess of AgNO3 solution is added...
Suppose a 12.42g mixture of NaCl and CaCl2 is dissolved in water. To this solution, an excess of AgNO3 solution is added resulting in the formation of 31.12g of the precipitate. Calculate the % by mass of NaCl and CaCl2 in the original mixture. Show all work.
A 0.8690 g sample of a mixture of NaCl and KCl is dissolved in water, and...
A 0.8690 g sample of a mixture of NaCl and KCl is dissolved in water, and the solution is then treated with an excess of AgNO3 to yield 1.933 g of AgCl. Calculate the percent by mass of each compound in the mixture. % mass NaCl = ? % mass KCl = ?
A 2.31 g sample of a mixture of AgNO3 and NaNO3 is treated with excess Na2S(aq)....
A 2.31 g sample of a mixture of AgNO3 and NaNO3 is treated with excess Na2S(aq). The precipitate is filtered off, dried and weighed. The dried precipitate weighs 0.47 g. What is the percentage by mass of NaNO3 in the original mixture? Your answer must be accurate to two significant digits. Keep several extra digits in your calculations and round off only at the end. Do not include the percent sign (%) as part of your answer! Molar masses (in...
A 2.1342.134 g sample of a solid mixture containing only potassium carbonate (MM=138.2058 g/molMM=138.2058 g/mol) and...
A 2.1342.134 g sample of a solid mixture containing only potassium carbonate (MM=138.2058 g/molMM=138.2058 g/mol) and potassium bicarbonate (MM=100.1154 g/molMM=100.1154 g/mol) is dissolved in distilled water. A volume of 31.5231.52 mL of a 0.7440.744 M HCl standard solution is required to titrate the mixture to a bromocresol green end point. Calculate the weight percent of potassium carbonate and potassium bicarbonate in the mixture. K2CO3:_____ wt% KHCO3:_____ wt%
A 0.6689 g mixture of KCN (MW = 65.116 g/mol) and NaCN (MW = 49.005 g/mol) was dissolved in water. AgNO, was added to the solution, precipitating all of the CN in solution as AgCN (MW = 133.886 g/mol). The dried precipitate weighed 1.518 g. Calculate the weight percent of KCN and NaCN in the original sample. KCN wt% = NaCN wt% =
A 0.2150 g sample is dissolved and treated with excess AgNO3. The precipitate is filtered, washed, dried, and weighed. The mass of the product (AgCl) is 0.4587 g. What is the wt% of Cl in the original sample? The molecular weight of AgCl is 143.32 g/mol.
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?
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