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3 November, 18:25

Calculate the concentration of buffer components present in 295.00 mL of a buffer solution that contains 0.390 M NH4Cl and 0.390 M NH3 immediately after the addition of 1.40 mL of 6.00 M HNO3.

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  1. 3 November, 22:00
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    The acid HNO₃ will react with the base NH₃ in the buffer to produce NH₄⁺, changing the concentrations of both NH₃ and NH₄⁺ in the buffer.

    Therefore, this question is solved by performing stoichiometric calculations based on those reactions:

    HNO₃ + NH₃ ⇒ NH₄⁺

    Vol HNO₃ = 1.40 mL x 1L / 1000 mL = 1.4 x 10⁻³ L

    # mol HNO₃ = 1.4 x 10⁻³ L x 6.00 mol/L = 8.4 x 10⁻³ mol HNO₃

    Since the reaction occurs in 1:1 ratio, 8.4 x 10⁻³ mol NH₃ will be consumed and 8.4 x 10⁻³ mol of NH₄⁺ will be produced.

    Initially we had

    # mol NH₄⁺ = 0.295 L x 0.390 mol/L = 0.115 mol

    # mol NH₃ = 0.115

    After reaction we will have

    # mol NH₄⁺ = 0.115 mol + 8.4 x 10⁻³ mol = 0.123 mol

    # mol NH₃ = 0.115 mol - 8.4 x 10⁻³ mol = 0.107 mol

    Therefore, their new concentrations will be

    Volume after reaction = 0.295 L + 0.0014 L = 0.296 L

    [NH₄⁺] = 0.123 mol / 0.296 L = 0.416 M

    [NH₃] = 0.107 mol / 0.296 L = 0.361 M
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