1. Questions

Chemistry

When 5 mL of 0.10 M HCl are added to 10 mL of 0.10 M NH3, what is the approximate pOH?
Kb for NH3 is 1.8 x 10^-5.

I get pOH between 4 and 5. Is that right?

  1. 👍
  2. 👎
  3. 👁
Mary

  1. I don't think so.
    NH3 + NaOH ==> NH4Cl

    Initial:
    NH3 = 10 mL x 0.1M = 1 mmol
    HCl = 5 mL x 0.1 M = 0.5 mmol

    This will form 0.5 mmole NH4Cl, all of the HCl will be used up and it will leave 0.5 mmole NH3 unreacted. What do we have? We have weak base (NH3) and its salt (NH4Cl) which is a buffer.
    pH = pKa + log p(base)/(acid)] =
    pH = 9.255 + ....... you can finish.

    1. 👍
    2. 👎
    DrBob222

Respond to this Question

First Name

Your Response

Similar Questions

  1. Honors Chemistry

    "How many grams of NH3 can be produced from the reaction of 28 g of N2 and 25 g of H2? N2 + 3H2 ---> 2NH3 ==> 28 g N2 x (1 mol N2/14.0 g N2) x (2 mol NH3/1 mol N2) x ( 17.0 g NH3/ 1 mol NH3) = 68 g NH3 25 g H2 x ( 1mol H2/2.0 g

  2. Chemistry

    Calculate the change in PH when 6 ml of 0.1 M HCl is added to 100 ml of a buffer solution that is 0.1 M in NH3 and 0.1 M in NH4Cl. And calculate the change in PH when 6 ml of 0.1 M NaOH is added to the original buffer solution.

  3. chem

    Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCl. Calculate the pH after the following volumes of titrant have been added. (The Kb for NH3 is 1.8e-05.) (a) 0 mL . (b) 25.0 mL . (c) 59.0 mL . (d) 60.0 mL (e) 63.0

  4. Chemistry

    The reaction of hydrochloric acid (HCl) with ammonia (NH3) is described by the equation: HCl + NH3 → NH4Cl A student is titrating 50 mL of 0.32 M NH3 with 0.5 M HCl. How much hydrochloric acid must be added to react completely

  1. Chemistry

    The conjugate acid in the reaction described in HCl(g) + NH3(aq) → NH4 +(aq) + Cl- (aq) is A. HCl(g). B. NH3(aq). C. NH4+ (aq). D. Cl-(aq). I think its B or C?

  2. Chemistry

    What mass of NH4Cl must be added to 0.750 L of a 0.100 M solution of NH3 to give a buffer solution with a pH of 9.26? Kb(NH3) = 1.8 x 10^-5. (Hint: Assume a negligible change in volume as the solid is added.)

  3. 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

  4. Chemistry

    100 mL of each of the following solutions is mixed; which one of the mixed solutions is a buffer? A) 1.0 M NH3(aq) + 0.6 M KOH(aq) B) 1.0 M NH4Cl(aq) + 1.0 M KOH(aq) C) 1.0 M NH3(aq) + 0.4 M HCl(aq) D) 1.0 M NH4Cl(aq) + 0.4 M

  1. Chemistry

    Calculate the enthalpy change (ΔH) for: HCl(aq) + NH3(aq) → NH4Cl(aq) The reaction of 50.0 mL of 1.00 M HCl with 50.0 mL of 1.00 M NH3 causes a temperature rise of 6.4 ˚C in the resulting 100.0 mL of solution. The NH4Cl

  2. Chemistry

    Combine and rearrange the neutralization of HCl by NH3 and the dissolution of NH4Cl in water to arrive at the decomposition of NH4Cl? I know the eq. is NH4Cl -> NH3(g)+HCl(g) But I am confused how this works with the decomposition

  3. Chemistry

    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

  4. chem

    A sample of 7.80L of NH3 (ammonia) gas at 22 degrees and 735mmHg is bubbled into a 0.350L solution of 0.400M HCL(hydrochloric acid). The Kb value for NH3 is 1.8x10-5 Assuming all the NH3 dissolves and that the volume of the

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