Ksp for Ag2CO3 (molar mass = 276 g/mol) is 3.50x10-6. Into a 100.00 mL saturated Ag2CO3...
Ksp for Ag2CO3 (molar mass = 276 g/mol) is 3.50x10-6.
Into a 100.00 mL saturated Ag2CO3 solution, 0.0200 mol of Na2CO3 solid is added. How many grams (3 sig fig) of solid will precipitate?
(hint: find how many moles of Ag2CO3 is dissolved in pure water, and how many moles is dissolved in Na2CO3 solution. The difference is how many moles will precipitate out from solution.)
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Ksp for Ag2CO3 (molar mass =
276 g/mol) is 3.50x10-6.
Into a 100.00 mL saturated Ag2CO3...
A solution of 1.0 L saturated with Ag2CO3 at 5.0 ⁰C is filtered to remove the...
A solution of 1.0 L saturated with Ag2CO3 at 5.0 ⁰C is filtered
to remove the solid. Enough HCl (aq) is added to completely
decompose the dissolved compound. The CO2 (g) that is generated is
collected in a 19.0 mL vial and exerts a pressure of 114 mmHg at
25.0 ⁰C. a. Write the reaction for decomposing the silver carbonate
with the acid. b. Determine the number of moles of CO2 that are
produced. c. Determine the Ksp for silver...
A saturated solution of Co(OH)2 was found to contain 3.7 ✕ 10−6 mol OH − in 100.0 mL. Calculate the Ksp of Co(OH)2. 4 si...
A saturated solution of Co(OH)2 was found to contain 3.7 ✕ 10−6 mol OH − in 100.0 mL. Calculate the Ksp of Co(OH)2. 4 sig figs
Consider zinc hydroxide. It can be formed when solutions of zinc nitrate and sodium hydroxide are...
Consider zinc hydroxide. It can be formed when solutions of zinc nitrate and sodium hydroxide are mixed. Its Ksp is 4.0x10-17. a) Write the equilibrium balanced equation and the Ksp equilibrium expression equation for zinc hydroxide. b) How many moles of sodium hydroxide must be added to 575 mL of 0.0300 M zinc nitrate to just start the precipitation of zinc hydroxide? c) Will a precipitate form if 10.00 mL of 0.0200 M NaOH is added to 250 mL of...
The solubility product constant for Ba(IO3)2 is 1.57×10-9 at 25 oC. What is the molar concentration...
The solubility product constant for Ba(IO3)2 is 1.57×10-9 at 25 oC. What is the molar concentration of IO3- ions in a saturated solution of Ba(IO3)2? Assume an ideal solution at 25 oC. How many grams of Ba(IO3)2 (487.1 g/mol) can be dissolved in 1000 mL of pure water at 25 oC? How many grams of Ba(IO3)2 can be dissolved in 1000 mL of a 0.100 M KIO3 solution at 25 oC? Use activities for this calculation.
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...
(a) Based on the measured [HC4H4O6−] and the molar mass of KHC4H4O6 (188.18 g/mol), what is...
(a) Based on the measured
[HC4H4O6−] and the molar mass of KHC4H4O6 (188.18 g/mol), what is
the gram solubility (g/L)of KHC4H4O6 in solution #2 trial 1? Answer
to 2 decimal places.
(b) TRUE/ FALSE: The Ksp of solution #1 and solution #2 should
be the same even with the add KCl.
(c) TRUE/ FALSE: Using LeChatlier’s Principle, the molar
solubility of KHC4H4O6 should be
the same for solution #1 and #2.
Assigned saturated solution (circle) Solution Concentration of NaOH solution:...
The solubility product constant for La(IO3)3 is 1.00×10-11 at 25 oC. What is the molar concentration...
The solubility product constant for La(IO3)3 is 1.00×10-11 at 25 oC. What is the molar concentration of IO3- ions in a saturated solution of La(IO3)3? Assume an ideal solution at 25 oC. How many grams of La(IO3)3 (663.6 g/mol) can be dissolved in 900 mL of pure water at 25 oC? How many grams of La(IO3)3 can be dissolved in 900 mL of a 0.100 M KIO3 solution at 25 oC? Use activities for this calculation. Activity coefficients can be found...
41 A solution is made 0.10 molar in Mo2+, 0.10 molar in NH3, and 1.0 molar...
41 A solution is made 0.10 molar in Mo2+, 0.10 molar in NH3, and 1.0 molar in NH,CI. ill Mg(OH)2 precipitate? 42 How many grams of ammonium chloride must be added to 100 ml of 0.050-molar ammonium hydroxide to revent the precipitation of ferrous hydroxide, Fe(OH)2, when the NH4CI- NH4OH mixture is added to 100 ml of 0.020-molar FeCl2? Assume that the addition of solid NH4Cl produces no volume change 43 The Ksp of calcium phosphate, Ca3(PO4)2, is 1.3 X...
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...
A 49.5 ml solution containing 3.03 g of Na2CO3 (molar mass = 106 g/mol) and 50.5...
A 49.5 ml solution containing 3.03 g of Na2CO3 (molar mass = 106 g/mol) and 50.5 ml solution containing excess Al(NO3)3 (molar mass = 213 g/mol) are mixed. What is the molecular formula of the insoluble product and how much of that product is formed? Al2(CO3)3; 2.23 g formed AICO; 1133 g formed Al2(CO3)3: 6.38 g formed Nag(NO3)63.03 g formed NaNO3;2.23 g formed NaNO3: 6.38 g formed
A solution of 1.0 L saturated with Ag2CO3 at 5.0 ⁰C is filtered
to remove the solid. Enough HCl (aq) is added to completely
decompose the dissolved compound. The CO2 (g) that is generated is
collected in a 19.0 mL vial and exerts a pressure of 114 mmHg at
25.0 ⁰C. a. Write the reaction for decomposing the silver carbonate
with the acid. b. Determine the number of moles of CO2 that are
produced. c. Determine the Ksp for silver...
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...
(a) Based on the measured
[HC4H4O6−] and the molar mass of KHC4H4O6 (188.18 g/mol), what is
the gram solubility (g/L)of KHC4H4O6 in solution #2 trial 1? Answer
to 2 decimal places.
(b) TRUE/ FALSE: The Ksp of solution #1 and solution #2 should
be the same even with the add KCl.
(c) TRUE/ FALSE: Using LeChatlier’s Principle, the molar
solubility of KHC4H4O6 should be
the same for solution #1 and #2.
Assigned saturated solution (circle) Solution Concentration of NaOH solution:...
41 A solution is made 0.10 molar in Mo2+, 0.10 molar in NH3, and 1.0 molar in NH,CI. ill Mg(OH)2 precipitate? 42 How many grams of ammonium chloride must be added to 100 ml of 0.050-molar ammonium hydroxide to revent the precipitation of ferrous hydroxide, Fe(OH)2, when the NH4CI- NH4OH mixture is added to 100 ml of 0.020-molar FeCl2? Assume that the addition of solid NH4Cl produces no volume change 43 The Ksp of calcium phosphate, Ca3(PO4)2, is 1.3 X...
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...
A 49.5 ml solution containing 3.03 g of Na2CO3 (molar mass = 106 g/mol) and 50.5 ml solution containing excess Al(NO3)3 (molar mass = 213 g/mol) are mixed. What is the molecular formula of the insoluble product and how much of that product is formed? Al2(CO3)3; 2.23 g formed AICO; 1133 g formed Al2(CO3)3: 6.38 g formed Nag(NO3)63.03 g formed NaNO3;2.23 g formed NaNO3: 6.38 g formed
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