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Aqueous solutions of the following reactants are mixed. Calculate the concentration in mol/L) of calcium ions in solution after the reaction has gone to completion. 75.0 mL of 1.50 M AgNO, are mixed with 75.0 mL of 2.1 M Cacly DO NOT include units in your answer. If you round during your calculation, be sure to keep at least four (4) decimal places. Report your answer to two (2) decimal places. Answer: Calculate the mass of precipitate formed (in grams) when aqueous solutions of the following reactants are mixed. Assume that the reaction goes to completion. 79 mL of 1.50 M AgNO3 are mixed with 75.0 mL of 1.00 M CaCl, Do NOT include units in your answer. If you round during your calculation, be sure to keep at least four (4) decimal places. Report your answer to two (2) decimal places. Answer:

Respuesta :

The concentration (in mol/L) of calcium ions in solution after the reaction has gone to completion. 75.0 mL of 1.50 M AgNO, are mixed with 75.0 mL of 2.1 M is 0.75 mol / L.

The reaction is given as :

2AgNO₃(aq)    +   CaCl₂(aq)   ----->   Ca(NO₃)₂(aq)    +   2AgCl(s)

moles of AgNO₃ = molarity × volume

                            = 1.50 × 0.075

                            = 0.1125 mol

moles of  CaCl₂ = 2.1  × 0.075

                           = 0.1575 mol

AgNO₃ is a limiting reactant ,2mole of AgNO₃ produces 1 mole of Ca(NO₃)₂

moles of Ca(NO₃)₂ = 0.1125 / 2 = 0.05625 mol

concentration of Calcium ion is = 0.05625  / 0.075

                                                    = 0.75 mol/ L

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