Consider mixing 3.60L of A 0.345 K2SO4 solution with 2.40 L of A 0.721 M BaCl2...
Consider mixing 3.60L of A 0.345 K2SO4 solution with 2.40 L of A 0.721 M BaCl2 solution.
a) What compound precipitates from the solution?
b) What is the net ionic equation?
c) If 225.0 grams of the precipitate is recovered, what is the %
yield?
d) What is the concentration of each ion remaining in solution
after precipitation?
Please, please, please assist me with this question. I did all the work but I am not sure if I did it all right.
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Consider mixing 3.60L of A 0.345 K2SO4 solution with 2.40 L of A
0.721 M BaCl2...
3.) (Taken from General Chemistry: Principals and Modern Applications(8 Ed.) by Petrucci, Harwood L of 1.00 M NH,. How many of AgI(s) forming? and Herring) A 0.10 mol sample of AgNO,(s) is diss...
3.) (Taken from General Chemistry: Principals and Modern Applications(8 Ed.) by Petrucci, Harwood L of 1.00 M NH,. How many of AgI(s) forming? and Herring) A 0.10 mol sample of AgNO,(s) is dissolved in 1.00 grams of Nal can be dissolved in this solution without a precipitate 4.) (Modified from Chemistry: A Molecular Approach, 1" Ed. by Tro) Consider a solution that is 0.024 M in Cu and 0.017 M in Fe (a) If sodium hydroxide is used to selectively...
A solution is prepared by mixing 0.10 L of 0.12 M sodium chloride with 0.23 L...
A solution is prepared by mixing 0.10 L of 0.12 M sodium chloride with 0.23 L of a 0.19 M MgCl2 solution. What volume of a 0.20 M silver nitrate solution is required to precipitate all the Cl− ion in the solution as AgCl?
A solution is prepared by mixing 0.12 L of 0.13 M potassium chloride with 0.22 L...
A solution is prepared by mixing 0.12 L of 0.13 M potassium chloride with 0.22 L of a 0.19 M magnesium chloride. What volume of a 0.22 M silver nitrate solution is required to precipitate all of the chloride ion in the solution as silver chloride?
A solution is prepared by mixing 0.12L of 0.11 M sodium chloride with 0.26 L of...
A solution is prepared by mixing 0.12L of 0.11 M sodium chloride with 0.26 L of a 0.17 M MgCl2 soultion. what volume of a 0.20 M silver nitrate solution is required to precipitate all the Cl- ion in the solution as AgCl? express your answer using two significant figures.
please help i cant figure them out Consider the insoluble compound nickel(II) carbonate, NiCO3. The nickel...
please help i cant figure them out
Consider the insoluble compound nickel(II) carbonate, NiCO3. The nickel ion also forms a complex with cyanide ions. Write a net ionic equation to show why the solubility of NiCO3(s) increases in the presence of cyanide and calculate the equilibrium constant for this reaction. Solubility product constant data is found in the Chemistry References. For Ni(CN)4?: K = 2.0 1031. Use the pull-down boxes to specify states such as (aq) or (s). A solution...
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I need help please To a solution containing 0.15 M Ci- ion and 0.15 M Br- ion, you add some solid AgNO3. Ksp for AgCl is 1.6 * 10^-10 and for AgBr is 5.0*10^-13. the addition of solid doesn't change the total volume. a) which component AgCl or AgBr precipitates first? b) what is the concentration of the first anion to precipitate when the silver halide of the second anion starts to precipitate?
I mix the following things into a SINGLE 1 L beaker: 150 mL of 0.100 M Na2COs 50.0 mL of 0.050 M ...
I mix the following things into a SINGLE 1 L beaker: 150 mL of 0.100 M Na2COs 50.0 mL of 0.050 M BaCl2 100.0 mL of 0.025 M Cu(NO3)2 100.0 mL of 0.125 M Ca(NO3)2 50.0 mL of 0.100 M NaOH 50.0 mL of 1.00 M HCI After the "soup" is all done "cooking".. .er...after equilibrium has been established, tell me the following: 4. What (if any) are all of the precipitates? 5. What is the mass of each precipitate?...
QUESTION 3 A solution is prepared by mixing 30.0 mL of 0.60 M Ba(NO3)2 and 30.0...
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3.) (Taken from General Chemistry: Principals and Modern Applications(8 Ed.) by Petrucci, Harwood L of 1.00 M NH,. How many of AgI(s) forming? and Herring) A 0.10 mol sample of AgNO,(s) is dissolved in 1.00 grams of Nal can be dissolved in this solution without a precipitate 4.) (Modified from Chemistry: A Molecular Approach, 1" Ed. by Tro) Consider a solution that is 0.024 M in Cu and 0.017 M in Fe (a) If sodium hydroxide is used to selectively...
please help i cant figure them out
Consider the insoluble compound nickel(II) carbonate, NiCO3. The nickel ion also forms a complex with cyanide ions. Write a net ionic equation to show why the solubility of NiCO3(s) increases in the presence of cyanide and calculate the equilibrium constant for this reaction. Solubility product constant data is found in the Chemistry References. For Ni(CN)4?: K = 2.0 1031. Use the pull-down boxes to specify states such as (aq) or (s). A solution...
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I mix the following things into a SINGLE 1 L beaker: 150 mL of 0.100 M Na2COs 50.0 mL of 0.050 M BaCl2 100.0 mL of 0.025 M Cu(NO3)2 100.0 mL of 0.125 M Ca(NO3)2 50.0 mL of 0.100 M NaOH 50.0 mL of 1.00 M HCI After the "soup" is all done "cooking".. .er...after equilibrium has been established, tell me the following: 4. What (if any) are all of the precipitates? 5. What is the mass of each precipitate?...
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