You dissolve 15.71 g of NH₄NO₃ in 150.0 mL of solution (call this solution A). You take 20.0 mL of solution A and add water until the total volume is 75.0 mL (call this solution B). You take 15.0 mL of solution B and add 25.0 mL of water to it (call this solution C). You mix 10.0 mL of solution B and 10.0 mL of solution C (call this solution D). What is the concentration of ammonium nitrate in solution D? A) 0.240 M B) 0.190 M C) 0.131 M D) 0.279 M E) none of these

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The correct answer is A because the concentration of ammonium nitrate in solution D is 0.240 M. This can be calculated using the formula:M1V1 = M2V2where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration, and V2 is the final volume.In this case, the initial concentration is 0.1571 g / (80.04 g/mol * 0.150 L) = 0.131 M. The initial volume is 20.0 mL. The final volume is 75.0 mL. So, the final concentration is 0.131 M * (20.0 mL / 75.0 mL) = 0.035 M.The same formula can be used to calculate the concentration of ammonium nitrate in solution C. In this case, the initial concentration is 0.035 M, the initial volume is 15.0 mL, and the final volume is 40.0 mL. So, the final concentration is 0.035 M * (15.0 mL / 40.0 mL) = 0.013 M.Finally, the same formula can be used to calculate the concentration of ammonium nitrate in solution D. In this case, the initial concentration is 0.035 M, the initial volume is 10.0 mL, and the final volume is 20.0 mL. So, the final concentration is 0.035 M * (10.0 mL / 20.0 mL) = 0.0175 M.The concentration of ammonium nitrate in solution D is 0.0175 M.

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