Ask Question
21 April, 05:28

Calculate the ph of a solution formed by mixing 250.0 ml of 0.15 m nh4cl with 100.0 ml of 0.20 m nh3. the kb for nh3 is 1.8 x 10-5.

+3
Answers (1)
  1. 21 April, 05:33
    0
    Equation is as under:

    pOH = pKb + log ([salt]/[base])

    Now:

    We have to find pKb for NH3:

    As,

    pKb = - log [Kb]

    pKb of NH3 = - log Kb = - log (1.8*10^-5) = 4.74

    Volume of final solution = 200+250 = 450mL

    As the equation of molarity is M1V1 = M2V2

    So,

    M1V1 = M2V2

    V1 = 450mL

    V2 = 250mL

    M2 = 0.15 M

    Putting all values into equation:

    M1*450 = 0.15*250

    M1 = 0.15*250/450

    M1 = 0.0833M

    Now we have to find molarity of [NH3]:

    [NH3]

    M1V1 = M2V2

    V1 = 50 mL

    V2 = 200mL

    M2 = 0.12M

    Putting all the values again in equation:

    M1*50 = 0.12*200

    M1 = 0.12*200/450

    M1 = 0.05333

    Using the equation pOH = pKb + log ([salt]/[base])

    pkb = 4.74

    salt = 0.0833 M

    base = 0.0533M

    Substitute:

    pOH = 4.74 + log (0.0833/0.0533)

    pOH = 4.74 + log 1.563

    pOH = 4.74 + 0.19

    pOH = 4.93

    pH = 14.00-pOH

    pH = 14.00-4.93

    pH = 9.07
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “Calculate the ph of a solution formed by mixing 250.0 ml of 0.15 m nh4cl with 100.0 ml of 0.20 m nh3. the kb for nh3 is 1.8 x 10-5. ...” 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