Ask Question
8 June, 10:13

Calculate the concentration of buffer components present in 287.00 mL of a buffer solution that contains 0.310 M NH4Cl and 0.310 M NH3 immediately after the addition of 1.50 mL of 6.00 M HNO3.

+3
Answers (1)
  1. 8 June, 10:41
    0
    NH₄⁺: 0.340M

    NH₃: 0.277M

    Explanation:

    A buffer is the mixture of a strong acid with its conjugate base.

    For the buffer of NH₃ / NH₄⁺, moles of each one are:

    NH₄⁺: 0.287L * (0.310mol / L) = 0.0890 moles

    NH₃: 0.287L * (0.310mol / L) = 0.0890 moles

    The reaction of HNO₃ with NH₃ is:

    HNO₃ + NH₃ → NH₄⁺ + NO₃⁻

    Moles of 1.50mL of 6.00M HNO₃ are:

    1.50x10⁻³L * (6.00mol / L) = 9x10⁻³ moles of HNO₃. These moles are moles produced of NO₃⁻ and consumed of NH₃. Thus moles after reaction are:

    NH₄⁺: 0.0890 moles + 0.0090 moles = 0.0980moles

    NH₃: 0.0890 moles + 0.0090 moles = 0.0800moles

    As total volume is 287.00mL + 1.50mL = 288.50mL (0.28850L), concentrations are:

    NH₄⁺: 0.0980moles / 0.28850L = 0.340M

    NH₃: 0.0800moles / 0.28850L = 0.277M
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “Calculate the concentration of buffer components present in 287.00 mL of a buffer solution that contains 0.310 M NH4Cl and 0.310 M NH3 ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers