carbonate ions from a soluble metal carbonate (M2CO3) will be quantitatively isolated as CaCO3(s) by precipitation...
carbonate ions from a soluble metal carbonate (M2CO3) will be quantitatively isolated as CaCO3(s) by precipitation using CaCl2 (aq) followed by filtration according to the following reaction:
CaCl2(aq) + M2CO3(aq) CaCO3(s) + 2 MCl(aq)
Determine the exact mass of unknown you started with and the mass of precipitate produced from it and identity for the metal in your unknown,it is a group IA metal carbonate you were given.
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carbonate ions from a soluble metal carbonate (M2CO3) will be
quantitatively isolated as CaCO3(s) by precipitation...
Many metal ions are precipitated from a solution by the sulfide ion. As an example, consider...
Many metal ions are precipitated from a solution by the sulfide ion. As an example, consider treating a solution of copper(II) sulfate with sodium sulfide solution: CuSO4(aq) + Na2S(aq) → CuS(s) + Na2SO4(aq) What volume of 0.104 M Na2S solution would be required to precipitate all of the copper(II) ion from 13.4 mL of 0.120 M CuSO4 solution? Volume = mL Submit Answer Try Another Version 7 item attempts remaining Generally, only the carbonates of the Group 1 elements and...
It is of interest to decide if an analytical separation of the metal ions can be...
It is of interest to decide if an analytical separation of the metal ions can be effected by selective precipitation of carbonates from a solution that is 9.11×10-2 M in Cu2+ and 0.100 M in Ca2+. CaCO3 Ksp = 3.80×10-9 CuCO3 Ksp = 2.50×10-10 To analyze this problem, answer the following questions. (1) What carbonate concentration is needed to precipitate 99.9% of the metal that forms the least soluble carbonate? __M (2) When 99.9% of the least soluble carbonate has...
Calcium carbonate (CaCO3) reacts with stomach acid (HCl, hydrochloric acid) according to the following equation: CaCO3(s)...
Calcium carbonate (CaCO3) reacts with stomach acid (HCl, hydrochloric acid) according to the following equation: CaCO3(s) + 2HCl(aq) + CO2(g) + H2O(l) + CaCl2(aq) A typical antacid contains CaCO3. If such an antacid is added to 25.0 mL of a solution that is 0.300 M in HCl, how many grams of CO2 gas are produced? Express the mass to three significant figures and include the appropriate units. TI MÃ + + + a ? Value Units MCO: = Submit Previous...
How could you use a precipitation reaction to separate the two metal ions? We could add...
How could you use a precipitation reaction to separate the two metal ions? We could add HF (aq) to obtain a precipitate of AgF (s). We could add more H2O to obtain a precipitate of AgOH(s). We could add HCl (aq) to obtain a precipitate of AgCl (s). o We could add HCl (aq) to obtain a precipitate of NaCl(s).
04 (a) Calcium ions can be determined by precipitation of the oxalate according to the equation:...
04 (a) Calcium ions can be determined by precipitation of the oxalate according to the equation: Ca2+ (aq) + C2O42- (aq) = CaC204 (s) The solid may then be filtered off, washed and oxalic acid is regenerated by the addition of excess sulfuric acid. The amount of oxalic acid is then quantified by titration using potassium permanganate according to the equation: H2C204 + MnO4 + H+ = CO2 + Mn2+ + H20 (unbalanced) In an experiment to find the concentration...
All multiple parts to the same problem, thank you! :) Solution Stoichiometry: We need to make...
All multiple parts to the same problem, thank you! :)
Solution Stoichiometry: We need to make a 0.250 M sodium carbonate solution. We will use a 100.00 mL volumetric flask. How many grams of solid sodium carbonate should we add to the flask to make the solution? Use 105.99 as the molar mass, report correct sig figs, and use g as the unit. Solution Stoichiometry: We need to make a 0.200 M calcium chloride solution. We will use a 100.00...
DATA ANALYSIS Part 1 - Precipitation, Filtration, and Drying of Calcium Carbonate 1. Write a balanced chemical equ...
DATA ANALYSIS Part 1 - Precipitation, Filtration, and Drying of Calcium Carbonate 1. Write a balanced chemical equation for the reaction between calcium chloride and potassium carbonate. K2CO3 (aq) + CaCl2 (aq) > CaCO3 (s) + 2 KCl (aq). 2. Using stoichiometry, calculate the limiting reactant and the theoretical yield (the mass of Caco, product) for the reaction. 3. What is the actual yield of Cacox(s) formed from your experiment? Show your work. 4. Determine the percent yield of the...
I need help figuring out the flowchart and if I have the right answers for the...
I need help figuring out the flowchart and if I have the right
answers for the prelab please and thank you!
Group I, the Chloride Group BACKGROUND The precipitating reagent for the chloride group is chloride ion in an acidic solution. Only three of the 18 metal ions form a precipitate with this reagent: silver ion (Ag'), mercury(I)ion (Hg). and lead ion (Pb). Since lead chloride is somewhat soluble, it is not completely precipitated here, and a low concentration of...
I need help with the prelab and the flowchart. I’m totally clueless on the flowchart. For...
I need help with the prelab and the flowchart. I’m totally
clueless on the flowchart.
For the prelab questions I have some answers but I don’t know
if they’re right. If they’re wrong, I would greatly appreciate an
explanation for the correct answer. I’m really trying to learn the
material but it’s hard now that classes are cancelled so I’m sorry
if these are dumb
1. PbCl ?
2. Ag+
3. ?
4. S1
Group 1, the Chloride Group BACKGROUND...
Group I Cations A INTRODUCTION Most metal halides are soluble in water and dilute hydrochloric acid....
Group I Cations A INTRODUCTION Most metal halides are soluble in water and dilute hydrochloric acid. The exceptions are silver ion, Ag mercurous ion, Hg,: and lead(II) ion, Pb. Consequently, the addition of HCI to a solution of metal cations leads to the selective precipitation of these three ions. While the theory behind the separation and identification of these ions has been outlined in the general discus- sion of the qualitative analysis scheme, some aspects of this chemistry need to...
Many metal ions are precipitated from a solution by the sulfide ion. As an example, consider treating a solution of copper(II) sulfate with sodium sulfide solution: CuSO4(aq) + Na2S(aq) → CuS(s) + Na2SO4(aq) What volume of 0.104 M Na2S solution would be required to precipitate all of the copper(II) ion from 13.4 mL of 0.120 M CuSO4 solution? Volume = mL Submit Answer Try Another Version 7 item attempts remaining Generally, only the carbonates of the Group 1 elements and...
Calcium carbonate (CaCO3) reacts with stomach acid (HCl, hydrochloric acid) according to the following equation: CaCO3(s) + 2HCl(aq) + CO2(g) + H2O(l) + CaCl2(aq) A typical antacid contains CaCO3. If such an antacid is added to 25.0 mL of a solution that is 0.300 M in HCl, how many grams of CO2 gas are produced? Express the mass to three significant figures and include the appropriate units. TI MÃ + + + a ? Value Units MCO: = Submit Previous...
How could you use a precipitation reaction to separate the two metal ions? We could add HF (aq) to obtain a precipitate of AgF (s). We could add more H2O to obtain a precipitate of AgOH(s). We could add HCl (aq) to obtain a precipitate of AgCl (s). o We could add HCl (aq) to obtain a precipitate of NaCl(s).
04 (a) Calcium ions can be determined by precipitation of the oxalate according to the equation: Ca2+ (aq) + C2O42- (aq) = CaC204 (s) The solid may then be filtered off, washed and oxalic acid is regenerated by the addition of excess sulfuric acid. The amount of oxalic acid is then quantified by titration using potassium permanganate according to the equation: H2C204 + MnO4 + H+ = CO2 + Mn2+ + H20 (unbalanced) In an experiment to find the concentration...
All multiple parts to the same problem, thank you! :)
Solution Stoichiometry: We need to make a 0.250 M sodium carbonate solution. We will use a 100.00 mL volumetric flask. How many grams of solid sodium carbonate should we add to the flask to make the solution? Use 105.99 as the molar mass, report correct sig figs, and use g as the unit. Solution Stoichiometry: We need to make a 0.200 M calcium chloride solution. We will use a 100.00...
DATA ANALYSIS Part 1 - Precipitation, Filtration, and Drying of Calcium Carbonate 1. Write a balanced chemical equation for the reaction between calcium chloride and potassium carbonate. K2CO3 (aq) + CaCl2 (aq) > CaCO3 (s) + 2 KCl (aq). 2. Using stoichiometry, calculate the limiting reactant and the theoretical yield (the mass of Caco, product) for the reaction. 3. What is the actual yield of Cacox(s) formed from your experiment? Show your work. 4. Determine the percent yield of the...
I need help figuring out the flowchart and if I have the right
answers for the prelab please and thank you!
Group I, the Chloride Group BACKGROUND The precipitating reagent for the chloride group is chloride ion in an acidic solution. Only three of the 18 metal ions form a precipitate with this reagent: silver ion (Ag'), mercury(I)ion (Hg). and lead ion (Pb). Since lead chloride is somewhat soluble, it is not completely precipitated here, and a low concentration of...
I need help with the prelab and the flowchart. I’m totally
clueless on the flowchart.
For the prelab questions I have some answers but I don’t know
if they’re right. If they’re wrong, I would greatly appreciate an
explanation for the correct answer. I’m really trying to learn the
material but it’s hard now that classes are cancelled so I’m sorry
if these are dumb
1. PbCl ?
2. Ag+
3. ?
4. S1
Group 1, the Chloride Group BACKGROUND...
Group I Cations A INTRODUCTION Most metal halides are soluble in water and dilute hydrochloric acid. The exceptions are silver ion, Ag mercurous ion, Hg,: and lead(II) ion, Pb. Consequently, the addition of HCI to a solution of metal cations leads to the selective precipitation of these three ions. While the theory behind the separation and identification of these ions has been outlined in the general discus- sion of the qualitative analysis scheme, some aspects of this chemistry need to...
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