A 14.2 ml solution of 0.036 M CaCl2 is mixed with10.1 ml of 0.04 M...
A 14.2 ml solution of 0.036 M CaCl2 is mixed with 10.1 ml of 0.04 M BaCl2. Aqueous KF is added. Calculate the fluoride ion concentration (in M) that will separate the metal ions. Enter a number to 4 decimal places.
Ksp for CaF2 = 3.2x10−11 Ksp for BaF2 = 1.5x10−6
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A 14.2 ml solution of 0.036 M CaCl2 is mixed with10.1 ml of 0.04 M...
QUESTION 3 A solution is prepared by mixing 30.0 mL of 0.60 M Ba(NO3)2 and 30.0...
QUESTION 3 A solution is prepared by mixing 30.0 mL of 0.60 M Ba(NO3)2 and 30.0 mL of 0.60 M Ca(NO3)2. Sodium fluoride is added to the mixture. Assume there is no volume change from the addition of sodium fluoride. Which compound precipitates first and at what concentration of F will we first see the precipitate form? Ksp BaF2 = 1.8 x 107 and Ksp CaF2 = 1.5 x 10-10 1. BaF2; 3.6 × 10-3M 2. CaF2; 7.2 10-4 M...
A 185.0 mL solution of 2.714 M strontium nitrate is mixed with 215.0 mL of a...
A 185.0 mL solution of 2.714 M strontium nitrate is mixed with 215.0 mL of a 3.460 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. mass: g Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a 0 for the concentration. [Na+]= M [NO−3]= M [Sr2+]= M [F−]= M
A 150.0 mL solution of 3.241 M strontium nitrate is mixed with 205.0 mL of a...
A 150.0 mL solution of 3.241 M strontium nitrate is mixed with 205.0 mL of a 3.569 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. mass: g Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a 0 for the concentration. [Na+]= M [NO−3]= M [Sr2+]= M [F−]=
A 165.0 mL solution of 2.777 M strontium nitrate is mixed with 210.0 mL of a...
A 165.0 mL solution of 2.777 M strontium nitrate is mixed with 210.0 mL of a 3.278 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate Number Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a zero for the concentration. Number Number 2+ Na Number Number
if 25.00 ml of 0.275 M solution of AgNO3(aq) is mixed with 25.00 ml of 0.300...
if 25.00 ml of 0.275 M solution of AgNO3(aq) is mixed with 25.00 ml of 0.300 M CaCl2(aq), what will be the reaction? What is the final concentration of all of the ions after the two solutions are mixed?
10) 2.00 mL ofa 0.0500 M CusO, solution is mixed with 2.00 mL of a 0.0100...
10) 2.00 mL ofa 0.0500 M CusO, solution is mixed with 2.00 mL of a 0.0100 M solution of K. Ksp (CuF2) 1.61 x 109 a) (7 pts) What is the concentration of Cu (aq) ion in the solution after equilibrium is established? b) (6 pts) Water is added to bring the volume of the solution to 1.00 L, and the mixture is stirred until equilibrium is reestablished. Calculate Q for this mixture. Is all of the CuF2 dissolved?
7. Will calcium fluoride (Ksp 5.3 x 10") precipitate when 200 mL of a 4.50 x...
7. Will calcium fluoride (Ksp 5.3 x 10") precipitate when 200 mL of a 4.50 x 10' M solution of Ca(NO,), is added to a 0.170 L solution of 2.5 x 10 M solution of KF? Ca(NO), + 2KF → 2KNO, + CaF2
375 mL of a 0.150 M aqueous solution of silver (I) nitrate is mixed with 125...
375 mL of a 0.150 M aqueous solution of silver (I) nitrate is mixed with 125 mL of a 0.125 M aqueous solution of sodium phosphate. Calculate the mass of precipitate that forms and the final concentration of each ion in the mixed solution. Volumes are additive and the precipitation reaction goes to completion. Can you show all work for calculating the final concentration of each ion in the reaction including Ag, NO3^-1, Na and PO4^-3
Using the appropriate Ksp values, find the concentration of NO3− ions in the solution at equilibrium...
Using the appropriate Ksp values, find the concentration of NO3− ions in the solution at equilibrium after 650 mL of 0.45 M aqueous Cu(NO3)2 solution has been mixed with 350 mL of 0.40 M aqueous KOH solution. (Enter in M.) (Ksp for Cu(OH)2 is 2.6x10-19). Now find the concentration of OH− ions in this solution at equilibrium. (Enter in M.)
A 1.00 mL solution containing 0.400g BaCl2-2H20 is mixed with 50.00 mL of a solution containing...
A 1.00 mL solution containing 0.400g BaCl2-2H20 is mixed with 50.00 mL of a solution containing 0.300 g NalO3. Determine the mass of Ba(IO3)2 formed. Ksp(Ba(IO3)2) = 1.6x10-9 Determine the saturation state of seawater (n) for calcite at pH 8.10 (current) and pH 7.80 (year 2100). The concentration of calcium is constant at 0.0103 M. The concentration of carbonate is 2.40x10- M (pH 8.10) and 1.48*10M (pH 7.8) Ksp (calcite) 4.272x10-7
QUESTION 3 A solution is prepared by mixing 30.0 mL of 0.60 M Ba(NO3)2 and 30.0 mL of 0.60 M Ca(NO3)2. Sodium fluoride is added to the mixture. Assume there is no volume change from the addition of sodium fluoride. Which compound precipitates first and at what concentration of F will we first see the precipitate form? Ksp BaF2 = 1.8 x 107 and Ksp CaF2 = 1.5 x 10-10 1. BaF2; 3.6 × 10-3M 2. CaF2; 7.2 10-4 M...
A 165.0 mL solution of 2.777 M strontium nitrate is mixed with 210.0 mL of a 3.278 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate Number Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a zero for the concentration. Number Number 2+ Na Number Number
10) 2.00 mL ofa 0.0500 M CusO, solution is mixed with 2.00 mL of a 0.0100 M solution of K. Ksp (CuF2) 1.61 x 109 a) (7 pts) What is the concentration of Cu (aq) ion in the solution after equilibrium is established? b) (6 pts) Water is added to bring the volume of the solution to 1.00 L, and the mixture is stirred until equilibrium is reestablished. Calculate Q for this mixture. Is all of the CuF2 dissolved?
7. Will calcium fluoride (Ksp 5.3 x 10") precipitate when 200 mL of a 4.50 x 10' M solution of Ca(NO,), is added to a 0.170 L solution of 2.5 x 10 M solution of KF? Ca(NO), + 2KF → 2KNO, + CaF2
A 1.00 mL solution containing 0.400g BaCl2-2H20 is mixed with 50.00 mL of a solution containing 0.300 g NalO3. Determine the mass of Ba(IO3)2 formed. Ksp(Ba(IO3)2) = 1.6x10-9 Determine the saturation state of seawater (n) for calcite at pH 8.10 (current) and pH 7.80 (year 2100). The concentration of calcium is constant at 0.0103 M. The concentration of carbonate is 2.40x10- M (pH 8.10) and 1.48*10M (pH 7.8) Ksp (calcite) 4.272x10-7
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