60.0 mL of a silver chlorate solution with a concentration of 0.654 M is mixed with 59.2 mL of a potassium sulphate solution with a concentration of 0.475 M. The concentration of the sulphate ions in the final mixture after the precipitation reaction is complete is __________ M. Assume 100% conversion. (Write the value only not the unit and round your answer to FOUR decimal places, e.g. 2.6921 or 0.0124)
60.0 mL of a silver chlorate solution with a concentration of 0.654 M is mixed with...
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
A 829.0-mL aliquot of 0.880 M aqueous potassium hydroxide is mixed with 829.0 mL of 0.880 M aqueous magnesium nitrate. ( just need d.) a.)Write a balanced chemical equation for any reaction that occurs. b.) The precipitate is magnesium hydroxide Mg(OH)2 c.) What mass of precipitate is produced? d.)Calculate the concentration of each ion remaining in solution after precipitation is complete. Assume that the precipitate is completely insoluble The concentration of K+ = ____ M The concentration of OH- =...
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 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−]=
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?
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
Solid silver acetate is slowly added to 50.0 mL of a 0.0570 M potassium sulfide solution. The concentration of silver ion required to just initiate precipitation is
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...
A 55.0 mL sample of a 0.102 M potassium sulfate solution is mixed with 35.0 mL of a 0.114 M lead (II) acetate solution. The solid lead (II) sulfate is collected, dried, and found to have a mass of 1.01 g. The Balanced Reaction is: Pb(CH3COO2)(aq) + K2SO4 --> PbSO4(S) + 2K (aq) + 2CH3COO- (aq) b.Write the net ionic reaction. c.Which ions are spectators? d.Determine the limiting reagent. e. Determine the theoretical yield. f.Determine the percent yield. g. Determine...
Please help!!!!! A 80.0 mL aliquot of a 0.250 M Ca(NO_3)_2 solution was mixed with 60.0 mL of a 0.500 M NaF solution. K_sp(CaF_2) = 3.90 times 10^-11. Calculate the mass of CaF_2 that was formed. Determine the equilibrium concentrations of Ca^2+ and F^- ions remaining in the resultant solution.