Calculate the pH after 0.010 mol gaseous HCl is added to 250.0 mL of each of the following buffered solutions:
a. .050 M NH3/.15 M NH4Cl
b. .5 M NH3/ 1.5 M NH4Cl

  1. 👍 0
  2. 👎 0
  3. 👁 1,028
  1. millimols NH3 initial = 250 x 0.05 = 12.5
    mm NH4Cl initial = 250 x 0.15 = 37.5
    add 0.01 mol = 10 mmols HCl.

    .......NH3 + HCl ==> NH4Cl

    Substitute the E line into Henderson-Hasselbalch equation and solve for pH.
    b is done the same way.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    A 0.450-gram sample of impure CaCO3(s) is dissolved in 50.0 mL of 0.150 M HCl(aq). The equation for the reaction is: CaCO3(s)+2HCl(aq) -> CaCl2(aq) + H2O(l) + CO2(g) The excess HCl(aq) is titrated by 9.75 mL of 0.125 M NaOH(aq).

  2. chemistry

    Changing 1 mol of Mg(s) and 1/2 mol of O2 (g) to gaseous atoms requires a total of approximately 150kJ of energy. The first and second ionization energies of Mg are 737kJ/mol and 1450kJ/mol respectively. The first and second

  3. chemistry

    The pH of a solution prepared by mixing 45 mL of 0.183 M KOH and 65 mL of 0.145 M HCl is i solved it but my answer is wrong. the right one is 1.97. am i missing a step? moles of HCl left over = (moles of HCl) – ( moles of KOH)

  4. Chemistry- college

    The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to H ions;that is, delta H(f) [H+(aq)]=0 A.for this reaction: calculate delta H(f) for the Cl- ions. HCl(g)

  1. chemistry

    How many moles of magnesium chloride are formed when 55 mL of 0.70 M HCl is added to 42 mL of 1.204 g Mg(OH)2? Mg(OH)2(s) + 2HCl(aq) MgCl2(aq) + 2H2O(l) A. 0.019 mol B. 0.012 mol C. 0.021 mol D. 0.039 mol

  2. Grade 12 chemistry

    This is the second reaction: HCl(aq)+NaOH(aq)-->NaCl(aq)+H2O(l) (Heat of neutralization) This reaction involves mixing two solutions: 1.00 mol/L NaOH and 1.00 mol/L HCl. Trial 1: 48.0 mL of the NaOH solution is mixed with 47.5 mL

  3. Chemistry

    Suppose a 250. mL flask is filled with 1.1 mol of Cl2 and 0.60 mol of HCl. The following reaction becomes possible: H2(g)+Cl2(g) 2HCl (g) The equilibrium constant K for this reaction is 0.931 at the temperature of the flask.

  4. chemistry

    Given a 1.00 L solution that is 0.60 M HF and 1.00 M KF, calculate the pH after 0.080 mol NaOH is added, and calculate the pH after 0.24 mol HCl is added to the original solution.

  1. Chemistry

    Can you check my calculations, please? It's for a lab we did in order to find the the enthalpy of formation of NH4Cl(s). My final answer was -299.4 kJ, while the theoretical, or actual, value is -314.4 kJ. It was the closest value

  2. Chemistry

    The reaction of gaseous H2 and liquid Br2 to give gaseous HBr has ΔH = -17.4 kcal/mol (-72.8 kJ/mol) and ΔS = 27.2 (cal/mol⋅K) (114 J/(mol⋅K)). What is the value of ΔG (in kcal and kJ) for the reaction at 297 K ?

  3. CHEM

    Can you please check my work? I got -4.3KJ/mol If this is not right can you tell me what I am doing wrong? Thank you! Questions. 1.a. Use Hess's Law and the measured mean enthalpy changes for the NaOH-HCl and NH3-HCl reactions to

  4. Chemistry

    Calculate the pH of the resulting solution if 25.0 mL of 0.250 M HCl(aq) is added to (a) 35.0 mL of 0.250 M NaOH(aq). (b) 15.0 mL of 0.350 M NaOH(aq).

You can view more similar questions or ask a new question.