Chemsitry

The Ksp of PbBr2 is 6.60× 10^–6.

What is the molar solubility of PbBr2 in pure water?

What is the molar solubility of PbBr2 in 0.500 M KBr solution?

What is the molar solubility of PbBr2 in a 0.500 M Pb(NO3)2 solution?

  1. 👍 6
  2. 👎 2
  3. 👁 12,582
  1. PbBr2---> Pb + 2Br

    Ksp=[Pb][2Br]^2

    6.60× 10^–6=[x][2x]^2

    Solving for x

    6.60× 10^–6=4x^3

    6.60× 10^–6/4=x^3

    (6.60× 10^–6/4)^1/3=x

    B.)

    PbBr2---> Pb + 2Br

    Ksp=[Pb][2Br]^2

    6.60× 10^–6=[x][0.500M]^2

    Solve for x,

    6.60× 10^–6/[(0.500M)^2]=x

    C.)

    PbBr2---> Pb + 2Br

    Ksp=[Pb][2Br]^2

    6.60× 10^–6=[0.500M][2x]^2

    Solve for x,

    6.60× 10^–6/[(0.500M)^2]=x

    6.60× 10^–6/(0.500M)=4x^2

    sqrt*{[6.60× 10^–6/(0.500M)]/4}=x

    1. 👍 8
    2. 👎 4
  2. I don't disagree with any of the answers. Technically, and I realize this is nit-picking, I disagree with the set up. As an example,
    PbBr2 ==> Pb^2+ + 2Br^-
    But Ksp says "the product of the molar solubility of the ions, each raised to the power indicated in the balanced equation, is a constant". I would write that as Ksp = (Pb^2+)(Br^-)^2. It isn't twice the bromide ion x lead ion, it is THE bromide x lead ion. Yes, Pb ion is x and Br is 2x but 2x is THE bromide ion, not twice the bromide, but it is twice the PbBr2 that dissolves which is why it's 2x to begin with.

    1. 👍 2
    2. 👎 1
  3. I understand. That is why I worked on a problem and developed a headache when I couldn't figure out why the answer doubled compared to the answer that I calculated. If I set up the way that you mentioned then I would not have ran into that problem, and I can prevent others from performing the same mistake. Thank you for the advice. Also, I do not consider it nit-picking. I always thought it was nick-picking. We learn something new everyday.

    1. 👍 1
    2. 👎 0
  4. I lent my sleeping bag to a co-worker once, when I used it the next night I woke up suddenly, feeling something crawling in my crotch. I spent the next 2 hours picking the critters off. then I went cross eyed picking nits. I got them all. Unpicked nits can grow into a HUGE problem. Never think you are being to thorough, especially in chemistry!!

    1. 👍 3
    2. 👎 7
  5. t,mgbfjp[o;['

    1. 👍 0
    2. 👎 5

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Calculate the molar solubility of Cr(OH)3 in a solution with a PH of 11.6 knowing that the Ksp(Cr(OH)3)=6.7×10^-31.

  2. Chem 2

    what is the solubility of silver carbonate in water in 25 degrees celcius if Ksp=8.4X10-12? i don't know what to do Write the equation. Ag2CO3(s) ==> 2Ag^+ + CO3^= Ksp = (Ag^+2)(CO3^=) Let x = solubility of Ag2CO3. At

  3. Chemistry

    (Ksp= 5.0*10^-13) 1) Calculate the molar solubility of AgBr in 3.0×10^−2 M AgNO3 solution. 2) calculate the molar solubility of AgBr in 0.10 M NaBr solution. I tried solving using this the quadratic formula, but it didn't work.

  4. chemistry

    what is the solubility of barium sulfate in a solution containing 0.050 M sodium selfate? The Ksp value for barium sulfate is 1.1E-10. An insoluble salt with formula MX3 has a solubility product constant written in terms of

  1. chemistry

    Determine the molar solubility (S) of Zn(CN)2 in a solution with a pH = 4.91. Ksp (Zn(CN)2) = 3.0 × 10-16; Ka (HCN) = 6.2 × 10-10.

  2. Chemistry

    Which of the following substances has the greatest solubility in water? A. Ca(OH)2, Ksp = 6.5 × 10-6 B. Ag2SO4, Ksp = 1.5 × 10-5 C. PbI2, Ksp = 7.9 × 10-9 D. Zn(IO3)2, Ksp = 3.9 × 10-6 E. BaF2, Ksp = 1.5 × 10-6

  3. Chem 2

    4) Calculate the solubility of calcium hydroxide, Ca(OH)2 (Ksp = 5.5 x 10-5) in grams per liter in: a. Pure water b. 0.10 M CaCl2

  4. Chemistry

    #25 The Ksp of nickel(II) hydroxide, Ni(OH)2, is 5.84 × 10-16. Calculate the molar solubility of this compound.

  1. chemistry

    The Ksp of Ag2CrO4(s) is 1.12 x 10^-12. Calculate the molar solubility of AgCrO4(s) a)in pure water b) in a solution of 0.10 mol/L sodium chromate, Na2CrO4(s)

  2. Chemistry

    Copper (I) chloride, CuCL, has Ksp = 1.9 x 10^ -7.calculate the molar solubility of CuCL in A)pure water, B)0.0200M HCl solution C) 0.200M HCl solution, and d) 0.150M CaCl2 solution. I used the ice table and for a) i got 0.000435

  3. Chemistry

    Calculate the molar solubility of Ag2SO4 when dissolved in water (Ksp = 1.8 x 10-5)

  4. chemistry

    Calculate the molar solubility of MX2, if the Ksp=3.3x10^-8 how can i solve this problem?

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