chemistry

Calculate the ionic strength of the solution.
a) 100 mL of 0.8M magnesium perchlorate, Mg(ClO4)2, is added to 900 mL of 0.30M perchloric acid, HClO4. No reaction.

B)25 mL of 0.200M potassium iodide, KI, are mixed with 75 mL of 0.0300 M silver nitrate, AgNO3. Silver iodide precipitates.


For (a) you first need to determine the molarity of the resulting Mg(ClO4)2 and HClO4. Then use the ionic strength formula to determine the ionic strength. That is mu = AZ1^2 + BZ2^2 + CZ3^2where A is the Mg^+2 ion molarity and Z1^2 is the charge on the Mg^+2; B is the total molarity of the ClO4^- and Z2^2 is the charge on the ClO4^- ion; C is the molarity of the H^+ and Z3^2 is the charge on the H^+. For (b), you must first determine the reaction (a ppt of AgI will take place) and use the rxn to determine the final molarities of K^+, I^-, NO3^- and Ag^+. Then plug into the mu forumla to determine ionic strength. Please post your work if you need further assistance or if you would like us to check your answer. We need your work in order to determine the nature of your problem (but you probably won't have any trouble.) I hope this helps you get started.


I just noticed that I omitted the 1/2 on mu. It should read
nu = 1/2(AZ1^2 + BZ2^2 + CZ3^2) etc. Sorry about that.


That's mu and not nu. =)


define Physical science


Andrew:
You did the correct thing by posting a SEPARATE posting for this question. I saw this posting just by chance. I answered the later posting above. However, for definitions you can go to www.dictionary.com and look them up much faster than typing them here and waiting for a reply.

  1. 👍 0
  2. 👎 0
  3. 👁 165
asked by bria

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Calculate the number of moles of magnesium, chlorine, and oxygen atoms in 6.10 moles of magnesium perchlorate, Mg(ClO4)2.

    asked by Landis on March 24, 2019
  2. Chemistry

    What is the activity coefficient of H^+ in a solution containing 0.073 M HCl and 0.0090 M Ca(ClO4)2? What is the pH of the solution? I believe I have to find the ionic strength of the solution first, but I don't know how to find

    asked by Sam on February 4, 2013
  3. chem

    The mole fraction of an aqueous solution of potassium perchlorate is 0.125. Assuming that the density of this solution is 1.20g mL-1, calculate the following: (A) the mass percent of potassium perchlorate in the solution. (B) the

    asked by Lori on December 14, 2010
  4. Chemistry

    Write equations for the dissociation of the following in water. Do not include states in your answer. 1) sodium acetate (NaC2H3O2) NaC2H3O2 ---> Na+ + (C2H3O2)- 2) copper(II) perchlorate Cu(ClO4)2 ---> Cu2+ + 2(ClO4)- Enter

    asked by T on October 9, 2016
  5. Chemistry

    A solution contains 0.010 M BaCl2. Calculate the molarity of the ions in solution, the ionic strength of the solution, the activity coefficient of the barium ion and its activity. Repeat for the chloride ion. So I know the

    asked by sea lively on August 5, 2018
  6. gravimetric prob

    A pure organic compound weighing 947.4mg was heated in a stream of oxygen. The effluent gas was swept successively through a tube of magnesium perchlorate dessicant weighing 18.6137g and a tube of Ascarite weighing 16.8425g. After

    asked by vivian on April 20, 2015
  7. Chemistry

    Calculate [H3O ], [ClO4–], and [OH–] in an aqueous solution that is 0.130 M in HClO4(aq) at 25 °C. [H+]= [ClO4-]= [OH-]=

    asked by Sevy on October 20, 2011
  8. Chemistry

    Calculate [H3O ], [ClO4–], and [OH–] in an aqueous solution that is 0.130 M in HClO4(aq) at 25 °C. [H+]= [ClO4-]= [OH-]=

    asked by Sevy on October 20, 2011
  9. Chemistry

    Considering the effect of ionic strength, calculate the solubility of BaSO4 in 0.100 mol/L NaCl solution Ksp of BaSO4 = 1.1 X 10^-10

    asked by Patel on October 20, 2008
  10. Chemistry 111

    calculate the number of moles of magnesium, chlorine, and oxygen atoms in 8.80 moles of magnesium perchlorate?

    asked by kee on July 14, 2011

More Similar Questions