You mix 25 mL of 1.45 × 10^–4 M silver nitrate with 55 mL of 6.11 × 10–4 M sodium bromide. No precipitation occurs. The Ksp of AgBr is 7.9 × 10^–15. Is the solution unsaturated, saturated, or super saturated
The solution is :
You mix 25 mL of 1.45 × 10^–4 M silver nitrate with 55 mL of 6.11...
How many moles of moles of silver nitrate can be added to 100 mL of a 0.1 M aqueous sodium chloride solution before precipitation of a solid silver chloride occurs? (AgCl Ksp = 1.8x 10^-10 at 25 degrees Celsius)
Solid silver nitrate is added slowly to a solution that is 0.0010 M in sodium chloride and 0.0010 M in sodium bromide. What % of the bromide ions remain in solution, ie , unprecipitated, Just before silver chloride begins to precipitate? Kap for AgCI-1.8 x 10-10, Kp for AgBr- 3.3 x 10-13 10. 0.18% 0.018% 0.0010% 0.00010% 0.0018% a. b. c. d. e. 11. Calculate the concentration of F ions in saturated CaF2 solution at 25°C. Kap- 3.9x 10-" a....
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Given that 50.0 mL of 0.100 M magnesium bromide reacts with 13.9 mL of silver nitrate solution according to the unbalanced equation MgBr2 + AgNO3 = AgBr + Mg(NO3)2 (a) What is the molarity of the AgNO3 solution? (b) What is the mass of AgBr precipitate?
When 25.0 mL of a 2.7010-4 M silver nitrate solution is combined with 18.0 mL of a 7.80x10-5 M sodium bromide solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to
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1.Solid sodium sulfide is slowly added to 125 mL of a 0.0450 M silver nitrate solution. The concentration of sulfide ion required to just initiate precipitation is M. 2.Solid barium acetate is slowly added to 50.0 mL of a 0.0522 M ammonium sulfite solution. The concentration of barium ion required to just initiate precipitation is M. 3.Solid potassium hydroxide is slowly added to 150 mL of a 0.0329 M iron(III) nitrate solution. The concentration of hydroxide ion required to just initiate precipitation...
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
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