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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...
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...
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 9.59x102 M in Mn2+ and 0.106 M in Ca24 СаСОз Ksp 3.80x10-9 MnCO3 = 1.80x10-11 Kşp 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 precipitated,...
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 ftrom a solution that is 0.102 M im Cu? and 0.110 M in NP Kp-2.50 10-10 NiCOs Kup-6.60 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? When 990% of the least sol ble cat nate has precipt ated,...
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...
help! [Review Topica] [References) Use the References to access important values if needed for this question....
help!
[Review Topica] [References) Use the References to access important values if needed for this question. The maximum amount of iron(II) carbonate that will dissolve in a 0.293 M sodium carbonate solution is M. Submit Answer Retry Entire Group 9 more group attempts remaining Ote- e * @NN Solubility Product Constants (Ksp at 25 °C) Ksp Type Bromides Formula PbBr2 6.3 x 10-6 AgBr 3.3 * 10-13 Carbonates BaCO3 8.1 * 109 CaCO3 3.8 x 10 COCO3 8.0 * 10-13...
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...
At a certain temperature* (probably not 25 °C), the solubility of silver sulfate, Ag2SO4, is 0.012...
At a certain temperature* (probably not 25 °C), the solubility of silver sulfate, Ag2SO4, is 0.012 mol/L. Calculate its solubility product constant for this temperature. SIG. FIG. (required because number is small) Solubility product constants are very temperature sensitive. They are generally reported at 25°C. Not necessarily using this temperature allows me some flexibility. Answer: At a certain temperature, the solubility of potassium iodate, KIO3, is 36.1 g/L. Calculate its solubility product constant for this temperature. Answer: At a certain...
Ksp = [Ba²+][10,1 2. 10. mL of 0.10 M Ba(NO), is mixed with 10. mL of...
Ksp = [Ba²+][10,1 2. 10. mL of 0.10 M Ba(NO), is mixed with 10. mL of 0.10 M KIO,, a precipitate forms. for barium a. Which ion will still be present at appreciable concentration in the equilibrium mixture if K iodate is very small? b. What would that concentration be? 3. Lead chloride, PbCly, is slightly soluble with K equal to 1.7 x 10. a. What is the solubility of lead chloride in pure water? b. What would the solubility...
can yall help me with all four questions please? Consider these compounds A. MgCO3 B. AgzCO3...
can yall help me with all four questions please?
Consider these compounds A. MgCO3 B. AgzCO3 C. MnS D. MgF2 Complete the following statements by entering the letter(s) corresponding to the correct compound(s). (If more than one compound fits the description, include all the relevant compounds by writing your answer as a string of characters without punctuation, e.g, ABC.) Without doing any calculations it is possible to determine that manganese(Il) carbonate is more soluble than , and manganese(I) carbonate is...
1. In which solution will aluminum hydroxide, Al(OH)3, be least soluble? The solutions are similar except...
1. In which solution will aluminum hydroxide, Al(OH)3, be least soluble? The solutions are similar except that they have the following pH values: Hint: Common ion effect. Which two ions dictate acidity and basicity? a. 3 b. 7 c. 9 d. 11 2. Potassium perchlorate has a solubility product constant of 10-2. Which is true about the following solution of KClO4: [K+] = 0.01 M, [ClO4 −] = 0.01 M a. Ksp < Q and no precipitation occurs b....
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 9.59x102 M in Mn2+ and 0.106 M in Ca24 СаСОз Ksp 3.80x10-9 MnCO3 = 1.80x10-11 Kşp 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 precipitated,...
It is of interest to decide if an analytical separation of the metal ions can be effected by selective precipitation of carbonates ftrom a solution that is 0.102 M im Cu? and 0.110 M in NP Kp-2.50 10-10 NiCOs Kup-6.60 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? When 990% of the least sol ble cat nate has precipt ated,...
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...
help!
[Review Topica] [References) Use the References to access important values if needed for this question. The maximum amount of iron(II) carbonate that will dissolve in a 0.293 M sodium carbonate solution is M. Submit Answer Retry Entire Group 9 more group attempts remaining Ote- e * @NN Solubility Product Constants (Ksp at 25 °C) Ksp Type Bromides Formula PbBr2 6.3 x 10-6 AgBr 3.3 * 10-13 Carbonates BaCO3 8.1 * 109 CaCO3 3.8 x 10 COCO3 8.0 * 10-13...
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...
At a certain temperature* (probably not 25 °C), the solubility of silver sulfate, Ag2SO4, is 0.012 mol/L. Calculate its solubility product constant for this temperature. SIG. FIG. (required because number is small) Solubility product constants are very temperature sensitive. They are generally reported at 25°C. Not necessarily using this temperature allows me some flexibility. Answer: At a certain temperature, the solubility of potassium iodate, KIO3, is 36.1 g/L. Calculate its solubility product constant for this temperature. Answer: At a certain...
Ksp = [Ba²+][10,1 2. 10. mL of 0.10 M Ba(NO), is mixed with 10. mL of 0.10 M KIO,, a precipitate forms. for barium a. Which ion will still be present at appreciable concentration in the equilibrium mixture if K iodate is very small? b. What would that concentration be? 3. Lead chloride, PbCly, is slightly soluble with K equal to 1.7 x 10. a. What is the solubility of lead chloride in pure water? b. What would the solubility...
can yall help me with all four questions please?
Consider these compounds A. MgCO3 B. AgzCO3 C. MnS D. MgF2 Complete the following statements by entering the letter(s) corresponding to the correct compound(s). (If more than one compound fits the description, include all the relevant compounds by writing your answer as a string of characters without punctuation, e.g, ABC.) Without doing any calculations it is possible to determine that manganese(Il) carbonate is more soluble than , and manganese(I) carbonate is...
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