1. chemistry

    how do I set up a problem for the solubility product(Ksp) of a salt given the osmotic pressure at 781atm?
  2. 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 solubility,s, in the form a)
  3. chemistry ksp

    i feel like none of these answers are right. if the solubility of the solid is 'S' mol/ L, what is the Ksp of the product of the salt? Ca3PO42-(s) --> 3Ca2+(aq) + 2PO42- (aq) A)ksp=S^2 B)ksp=4S^3 C)ksp=27S^4 D)ksp=108S^5 Only leaning towards D because
  4. chem

    i feel like none of these answers are right. if the solubility of the solid is 'S' mol/ L, what is the Ksp of the product of the salt? Ca3PO42-(s) --> 3Ca2+(aq) + 2PO42- (aq) A)ksp=S^2 B)ksp=4S^3 C)ksp=27S^4 D)ksp=108S^5 Only leaning towards D because
  5. chemistry

    this is my work, would you please check my work, thank you! part A a liter of a solution saturated at 225 degree C with calcium oxalate, CaC2O4, is evaporated to dryness, giving a 0.0061 gm residue of CaC2O4. calculate the concentrations of the ions, and
  6. Chemistry(Please check)

    What is molar solubility of Al(OH)3 at 25 degrees C given the solubility product Ksp = 5.0e-33? I set this up as Al^3+ + 3OH^- Ksp=[Al^3+][OH^-]^3 5.0e-33 = (x)(3x)^3 Before I go any further did I do this correctly?
  7. Chem

    if salt has the solubility product expression Ksp={Br3+}2{S2-}3 what is the equilibrium equation for the solubility?
  8. Chemistry

    Which of the following compounds has the greatest molar solubility? A) AgBr, Ksp= 5.4 x 10^13 B) Ba3(PO4)2, Ksp = 3.0 x 10^-23 C) Al(OH)3, Ksp = 1.9 x 10^-33 D) MgF2, Ksp = 7.4 x 10^-11 E) Pb(OH)2, Ksp = 1.2 x 10^-15 I know the answer for this problem is
  9. chemistry

    determine the solubility product of the slightly soluble salt calcium oxalate,cac2o4 by titrating 200cm^3 sample of a suturated solution of this salt with 0.00135mol dm^3 HCl solution.calculate Ksp?
  10. chemistry

    I have no idea how to solve this problem, please help me out.... thanks a) A liter of a solution saturated at 25degree with calcium oxalate, CaC2O4, is evaporated to dryness, giving a 0.0061gm residue of CaC2O4. calculate the concentrations of the ions,
  11. Chemistry

    The solubility of Chromium (II) Hydroxide is .0035g/100mL - Calculate the solubility product of Chromium (II) Hydroxide. I know that we have to find Ksp. but i do not understand how to make the Ksp equation to calculate the solubility product, if it is
  12. Chemistry

    what is the molar solubility of lead sulfate in 1.0 X 10^-3 M Na2SO4? The Solubility Product Constant PbSO4 Ksp= 1.8 x 10^-8 The Ksp expression is: Na2SO4 = [2Na][SO4^-2] [2Na]=2x [SO4^-2]=x Ksp= 1.8 x 10^-8 = (x)(2x) Ksp= 1.8 x 10^-8 /4x^3 1.8 x 10^-8/4 =
  13. chemistry

    what is the most soluble salt of the following set? a) AgCN with Ksp=6.0 x 10^-17 b) Al(OH)3 with Ksp = 1.9x10^-33 c) Fe(OH)3 with Ksp = 2.6 x 10^-39 d) Sn(OH)2 with Ksp = 1.6 x 10^-19
  14. chemistry

    In quality control of raw materials for pharmaceutical production often used foul reactions to prove that raw materials in salt form containing the appropriate salt. Hydrochloride (eg. Amitriptyline hydrochloride) can be detected for example by
  15. chem

    The molar solubility of MgF2 at 25°C is 1.2 10-3 mol/L. Calculate Ksp. i got the euqation ksp= [F-]^2[Mg]2+ and plugged in 1.2e-3 and got 1.7e-9 but it is wrong. also this question If 0.0968 g of CaF2 dissolves per liter of solution, calculate the
  16. chemistry

    You are doing an experiment to determine the Ksp of a salt. If, while filtering, some of the solid passed through the filter and was not taken out before titrating, how would the calculated Ksp and solubility be affected? Thanks.
  17. Chem

    (a) The molar solubility of Ag2CrO4(s) at 35°C is 1.3 10-4 mol/L. Calculate Ksp. (b) If 0.0490 g of AgIO3 dissolves per liter of solution, calculate the solubility-product constant. (c) Using the appropriate Ksp value from Appendix D, calculate the
  18. Chemistry

    A generic salt, AB, has a molar mass of 159 g/mol and a solubility of 3.20 g/L at 25 °C. What is the Ksp of this salt at 25 °C?
  19. chemistry

    A generic salt, AB, has a molar mass of 313 g/mol and a solubility of 4.30 g/L at 25 °C. What is the Ksp of this salt at 25 °C?
  20. chemistry

    A generic salt, AB, has a molar mass of 293 g/mol and a solubility of 2.20 g/L at 25 °C. What is the Ksp of this salt at 25 °C?
  21. chemistry

    A generic salt, AB, has a molar mass of 293 g/mol and a solubility of 2.20 g/L at 25 °C. What is the Ksp of this salt at 25 °C?
  22. chemistry

    A generic salt, AB2, has a molar mass of 159 g/mol and a solubility of 3.30 g/L at 25 °C. What is the Ksp of this salt at 25 °C?
  23. Chemistry

    generic salt, AB3, has a molar mass of 333 g/mol and a solubility of 2.30 g/L at 25 °C. What is the Ksp of this salt at 25 °C?
  24. 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
  25. chemistry

    the solubility of the fictitious compound administratium fluoride in water is 3.091e-4.calculate the value of solubility product ksp
  26. Chemistry

    The solubility of the fictitious compound, administratium fluoride ( AdF3 ) in water is 3.091x10^-4M . Calculate the value of the solubility product Ksp .
  27. Chemistry - Solubility Equilibria

    If the solubility of CaCO_3 in water at 25°C is 5.84 ✕ 10^−3 g/L, calculate the solubility-product constant (Ksp) of CaCO_3, assuming complete dissociation of the CaCO_3 that has dissolved.
  28. Chemistry

    When excess NaOH is added to Zn(OH)2, the complex ion Zn(OH)4 2- is formed. Determine the molar solubility of Zn(OH)2 in .10 M NaOH. Compare with the molar solubility of Zn(OH)2 in pure water. I thought I knew how to do this problem, but I'm not getting
  29. chemistry

    The solubility of the fictitious compound, administratium fluoride (AdF3) in water is 3.091×10−4 M. Calculate the value of the solubility product Ksp.
  30. Chemistry

    The solubility of the fictitious compound, administratium fluoride (AdF3) in water is 3.091×10−4 M. Calculate the value of the solubility product Ksp.
  31. science..chemistry

    given the solubility product;Ksp,of calcium hydroxide is 0.0000064M,caculate its solubility at this temperature in i.water ii.0.1M calciumchloride solution
  32. Chemistry

    The solubility of the fictitious compound, administratium fluoride (AdF3) in water is 3.091×10−4 M. Calculate the value of the solubility product Ksp.
  33. chemistry check

    Dr.Bob you had told me to ignore 2x so I wondering if I wrote my did these steps correctly. Calculate the molar solubility of nickel (II) hydroxide in 0.100 M sodium hydroxide The solubility product of nickel (II) hydroxide at 25°C is 1.6 x 10-16. Ni(OH)2
  34. Chemistry

    Estimate the solubility of TISCN in a solution of which ionic strength is 1.265e-2M at 25 degree and Ksp=1.6e-4. I do not know why Prof. gives me ionic strength? In the next question, Prof. said " For a sparingly soluble ionic compound of type AB the
  35. Chemistry

    Question: The solubility of a salt in water increases if either ion of the salt undergoes hydrolysis. Comput the molar solubility of AgCN in water assuming no hydrolysis. B) compute the molar solubility of AnCN in water assuming hydrolysis occurs. The
  36. chemistry

    he solubility of the fictitious compound, administratium fluoride (AdF3) in water is 3.091×10−4 M. Calculate the value of the solubility product Ksp.
  37. chemistry

    The solubility of the fictitious compound, administratium fluoride (AdF3) in water is 3.091×10−4 M. Calculate the value of the solubility product Ksp.
  38. chem

    The solubility product of silver sulfate is 1.6* 10^-5. What is the molar solubility of this compound? Ksp= [Ag]^2[So4^2-] 1.6*10^-5 = x^3 x= .0252 but the answer in my book is (16/4)^1/3 *10^-2 which equals to 0.158
  39. chemistry

    A pan full of hot salt water, NaCl(aq), is cooled and NaCl(s) precipitates. Explain why this happens. Chloride ions are more strongly attracted to the metal in the pan than the sodium ions at low temperatures. As the vapor pressure of the solution
  40. Chemistry

    Consider a saturated solution of calcium fluoride in 0.086 M potassium nitrate. Complete the following tasks, and then answer the question. a) Write the chemical equation corresponding to Ksp. b) Write the defining expression for the thermodynamic
  41. Chemistry

    Tooth enamel is made up of hydroxyapatite, Ca_10(PO_4)_6(OH)_2 or the empirical formula, Ca_5(PO_4)_3(OH). Use the empirical formula for all calculations because stoichiometry plays two significant roles. A. Print the balanced chemical equation for the
  42. Chemistry

    We are given that the solubility product of platinum (II) sulfide is 9.9x10^-74 We are told to write a balanced equation for dissolving platinum (II) sulfide. I put : PtS(S) <> Pt^2+(aq) + S^2-(aq) and then we had to write the Ksp expression:
  43. Chemistry

    Given a saturated solution of CaF2, write the ionic equilibrium and use it to calculate the solubility of CaF2. My answer for the ionic equation is CaF2(s)<->Ca2+(aq)+ 2F-(aq) Ksp= [Ca2+][F-]2 the given ksp is 3.32*10-4 how do i figure out the
  44. chemistry

    Write the balanced equation and solubility product expression for the solubility equillibrium of Mn3(PO4)2: Ksp expression?
  45. Chemistry

    What mass of silver chromate can be dissolved in 125 mL of water? How do I find this out? Ag2CrO4 is not very soluble. Look up the solubility product and calculate the solubility from Ksp. Wow, thank you so much. I realised that I wrote my chemical formula
  46. chemistry

    Calulate the molar solubility of Al(OH)3 in water. (Ksp = 3 x 10^-34) Al(OH)3(s) ==>Al^+3 + 3OH^- Ksp = (Al^+3)(OH^-)^3 = 3E-34 Let x = molar solubility of Al(OH)3 then x molar = (Al^+3) and 3x molar = (OH^-) Plug in to Ksp and solve for x. Don't forget
  47. chem can u check answer please

    the solubility of silver sulfate in water is 0.223%(w/v) at 35 degrees celsius.calculate the solubility product of this salt at this temp. I got 1.46 X 10^-6 M is this right please thanks Andy
  48. Chemistry

    Determine the molar solubility of Y for XY2 if Ksp is 2.2x10^-4. The 2 in Xy2 is a subscript. I found the Ksp equation which is ksp=[x^2+][Y^-]^2 Then I did the ICE table and got x and 2x for the equilibrium concentrations. Then I did: 2.2x10^-4=(x)(2x)^2
  49. chemistry

    The solubility of MnS was found to be 0.000963 g per 700 mL of water. Calculate the solubility product constant (Ksp) for MnS. MnS (s)=Mn2+ (aq) + S2- (aq)
  50. Chem

    HCl is slowly added to a solution that is .250 M in Pb^2+ and .00150 M in Ag+. Which precipitate forms first, PbCl2 or AGCl? At what Cl- ion concentration will the precipitate first appear? Ksp for PbCl2= 1.6*10^-5, Ksp for AgCl= 1.7*10^-10 Seriously don't
  51. Chemistry !

    The solubility of Mn(OH)2 is 3.04 x 10^-4 gram per 100 ml of solution . A) write the balanced chem equation for Mn(OH)2 in aqueous solution B) calculate the molar solubility of Mn(OH)2 at 25 degrees celcius C) calculate the value of the solubility product
  52. chemistry

    Given a saturated solution of CaF2, write the ionic equilibrium and use it to calculate the solubility of CaF2. My answers for the ionic equation and ksp values are CaF2(s)<->Ca2+(aq)+ 2F-(aq) Ksp= [Ca2+][F-]2 ksp=2.02*10^-4 it asks what will happen
  53. chem/solubility

    the Ksp of CaF2 = 1.46*10^-10 and Ka of HF = 3.5*10^-4 Calculate the pH of a solution in which the solubility of CaF2 = .0100 moles/liter. so Ksp =[Ca2+][F-]^2 and Ka =[H3O+][F-]/[HF] I'm not sure how to continue...
  54. chemistry

    Will a fluoride concentration of 1.0 mg/L be soluble in a water containing 200 mg/L of calcium? This is what i found for ksp CaF2<--> Ca(2+) +2F(-) Ksp=(x)(4x^2) where x=solubility Therefore, Ksp=3.7 x 10^-11 and for Qsp I am not sure how to go on
  55. Chemistry Explanation??

    So what would the explanation for this be? Its really confusing me. The Ksp is independent of [NaOH] while the solubility of Ca(OH)2 decreases as the [NaOH] increases. Explain why this is the case. ( in the data table, the naoh concentration is 0 M, and
  56. chemistry

    the solubility product expression for BiS3 is Ksp= a.[Bi2^3][S3^2-]. b. [Bi^3+][S^2-]. c. [Bi^3+]^2 [S^2-]^3 d. none of these
  57. High school AP chem

    The solubility of Mn(OH)2 is 3.04 x 10^-4 gram per 100 ml of solution . A) write the balanced chem equation for Mn(OH)2 in aqueous solution B) calculate the molar solubility of Mn(OH)2 at 25 degrees celcius C) calculate the value of the solubility product
  58. Chem

    The solubility of Mn(OH)2 is 3.04 x 10^-4 gram per 100 ml of solution . A) write the balanced chem equation for Mn(OH)2 in aqueous solution B) calculate the molar solubility of Mn(OH)2 at 25 degrees celcius C) calculate the value of the solubility product
  59. To Dr.Bob

    The problem you helped me with: A liter of a solution saturated at 25 deg C with calcium oxalate, CaC2O4 is evaporated to dryness, giving a .0061 gm residue of CaC2)4. Calculate the concentrations of the inons, and the molar solubility and the solubility
  60. Chemistry

    What is the solubility of PbI2 in 0.4 M KI given the solubility constant of PbI2 is 7.1 x 10-9 a. 3.5 x 10-3 M b. 1.2 x 10-3 M c. 4.4 x 10-8 M Ksp = 7.1 x 10-9 Ksp = x * (2 * 0.4) (7.1 * 10-9)/.8 = x 8.8 x 10-9 = x ------ But this is not one of the
  61. Chemistry

    The molarity of Sr2+ in a saturated solution of SrSO4 was determined to be 0.000500 M. Calculate the solubility product constant (Ksp) for SrSO4. SrSO4(s) = Sr^2+(aq) + SO4^2- (aq) Molar Mass (g/mol) SrSO4 183.68 This is what I know: Ksp = [Sr][SO4]
  62. 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 equilibrium,(Ag^+) = 2x; (CO3^=) =
  63. chemistry

    What pb2+ concentration should be maintained in PbNO3 to produce a solubility of 1.7×10−4 PbI2/L when PbI2 is added? I found the ksp of PbI2 to be 7.1*10(-9), divided the ksp by the solubility, and took the square root, resulting in 6.5*10(-3). my
  64. Chemistry

    At 25 °C only 0.0610 mol of the generic salt AB2 is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C? AB2(s) <- -> A^2+(aq)+2B^-(aq) Is the answer ksp=9.08*10^-4?
  65. chemistry

    Calculate the molar solubility of MX2, if the Ksp=3.3x10^-8 i already asked this but im confused about one of the steps. Ksp = (x)(2x)^2 = 4x^3 = 3.3X10^-8 x = solubility = 0.00202M. but i don't understand do i substitute the x in 4x^3 3.3X10^-8 and then
  66. chemistry

    At a certain temperature, the solubility of strontium arsenate, Sr3(AsO4)2, is 0.0510 g/L. What is the Ksp of this salt at this temperature?
  67. Chemistry

    #24 At a certain temperature, the solubility of strontium arsenate, Sr3(AsO4)2, is 0.0660 g/L. What is the Ksp of this salt at this temperature?
  68. Chemistry

    Hi, I have a few chemistry problems that I'm having trouble solving. I put my attempted solutions after the problems in *'s. There was one problem I had no idea how to solve. What concentration of silver chromate (Ksp = 9.0 x 10-12) will dissolve to make a
  69. chemistry

    Calculate the solubility of silver chloride in a 0.1 mol/L solution of sodium chloride at 25°C.? At SATP, Ksp AgCl(s) = 1.8 x 10^-10 What did I do wrong? AgCl <----> Ag+ + Cl- [Ag+] = x [Cl-] = x + 0.1 Ksp = [Ag+] [Cl-] 1.8 x 10^-10 = (x) ( x + 0.1)
  70. chemistry

    It is possible to manipulate the solubility of some compounds through pH adjustments. What is the appropriate pH that will yield a Molar solubility for Mg(OH)2 of 2.51 x 10-8? The Ksp for Mg(OH)2 is 1.2 x 10-11. (Hint: you may assume the concentration of
  71. Chemistry

    Calculate the value of the solubility product (Ksp) for CdS given the following standard reduction potentials: CdS + 2e- --> Cd + S-2 E° = -1.21V Cd+2 + 2e- --> Cd E° = -0.402V --------------------------------------- CdS + Cd --> Cd + Cd+2 + S-2
  72. Solubility

    What is the solubility product of CaF2 if 0.1 M Ca2+ and 0.02 M F- are in solution just before precipitation occurs? 4.0 × 10^-5 The solubility product cannot be determined. 1.6 × 10^-4 2.0 × 10^-3
  73. Chemistry(Please help)

    The solubility product expression for mercury(I) iodide, Hg2I2 is Ksp = ? My answer is [Hg2^2+^][2I^-^]^2^ Would you agree?
  74. Chemistry -- to Dr.Bob I need your help!!!

    The solubility of product constant (ksp) for the dissolution of Pb3(Aso4)2 as represented by the chemical equation is 4.0 x 10^-36 Pb3(AsO4)2 (s)--->3Pb 2+ (aq) + 2 AsO4^3 (aq) Calculate the molar solubility (mol/L) of Pb3(AsO4)2 in water
  75. Chem

    Aqueous solutions of Zn+2 and Pb+2 both .0010M. Both form insoluble sulfides. Appx. what pH will allow maximum precipitation of one ion and leave the other in solution? Do I just use Ksp and the equations? If so what do I do next? See the selective
  76. chemistry

    a liter of a solution saturated at 25C with CaC2O4 is evaporated to dryness giving a 0.0061 gm residue of CaC2O4. Calculate the concentrations of the ions, and the molar solubility and the solubility product constant for this salt at 25C. Show the balanced
  77. -Chemistry-

    I have asked this question before but I was wondering if I solved this question correctly. A solution of barium chromate is prepared by dissolving 6.3 x 10-3 g of this yellow solid in 1.00 L of hot water. Will solid barium chromate precipitate upon cooling
  78. Chemistry-Repost for DrBob222

    My question was: A saturated solution of MgF2 at 23 degrees C was prepared by dissolving solid MgF2 in 1 L water. The Ksp of MgF2 is 1.5e-5. a.)Calculate the mass of MgF2 dissolved. b.) When .1 mols of solid KF was dissolved in the MgF2 solution,
  79. Chemistry

    Thallium (I) iodate is only slightly soluble in water. Its Ksp at 25°C is 3.07 x 10-6. Estimate the solubility of thallium iodate in units of grams per 100.0 ml of water. TlIO3(s) <==> Tl^+ + IO3^- Let x = molar solubility of TlIO3. The x is molar
  80. science( chem)

    Calculate the molar solubility of Mg(OH)2 in water I know Mg(OH)2=> Mg2+ + 2OH- 2H2O=> H3O+ + OH- Ksp= [Mg2+][OH]2 Kw= [H30+][OH-] Mass balance [Mg2+]=2[OH] So.. [OH-]=2[Mg2+]+ [H3O+] Charge balance is where I get kind of confused I know that the
  81. Chemistry

    A 1.00-L solution saturated at 25°C with calcium oxalate (CaC2O4) contains 0.0061 g of CaC2O4. The solubility constant (Ksp) for this salt is [CaC2O4=128.09 g/mol]
  82. chemisty

    the solubility product constant (Ksp) of ca(oh)2 at 25 C is 4.42*10^-5. a 500 ml of saturated solution of ca(oh)2 is mixed with equal volume of .4M naoh. what mass of ca(oh)2 is precipitated?
  83. chemistry

    When I have the table filled out, what would I need to do in order to calculate the solubility product for calcium hydroxide? The following is what I have in mind, please tell if I am incorrect or correct. Ksp = [Ca+2][OH-1]2 You should have an average
  84. College Chemistry

    A 1.00-L solution saturated at 25°C with calcium oxalate (CaC2O4) contains 0.0061 g of CaC2O4. The solubility constant (Ksp) for this salt is [CaC2O4=128.09 g/mol]
  85. Chemistry

    The solubility of sodium chloride is 35.9/100 ml in STP, try dissolving 1 kg of salt in 1 l of water what happens? how much salt will be dissolved and how much salt will be insoluble?
  86. chemistry

    Given the following solubility constants, which list arranges the solutes in order of increasing solubility? CaCO3: Ksp = 2.8 × 10-9 Ca(OH)2: Ksp = 5.5 × 10-6 CaSO4: Ksp = 9.1 × 10-6 CaF2: Ksp = 5.3 × 10-9 A. CaSO4 < Ca(OH)2 < CaCO3 < CaF2 B.
  87. chemistry

    What is the solubility of AgCl when it is in a solution of 0.15 M NaCl? (AgCl has Ksp = 1.8 x 10-10.) Make a reaction table. Include rows for initial concentration, change in concentration, and equilibrium concentration. Write down the equation for the Ksp
  88. chemistry

    What is the solubility of AgCl when it is in a solution of 0.15 M NaCl? (AgCl has Ksp = 1.8 x 10-10.) Make a reaction table. Include rows for initial concentration, change in concentration, and equilibrium concentration. Write down the equation for the Ksp
  89. Chemistry

    Consider the reaction Zn(OH)2(s) + 2CN-(aq) <--> Zn(CN)2(s) + 2OH-(aq) a) Calculate K for the reaction. (Ksp Zn(CN)2= 8.0 x 10^-12) b) Will Zn(CN)2 precipitate if NaCN is added to a saturated Zn(OH)2 solution? I tried splitting this into two
  90. chemistry

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

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

    A 1.00-L solution saturated at 25°C with lead(II) iodide contains 0.54 g of PbI2. Calculate the solubility-product constant for this salt at 25°C.
  93. Chemistry

    A 1.00 L solution saturated at 25°C with lead(II) iodide contains 0.54 g of PbI2. Calculate the solubility-product constant for this salt at 25°C. thanks
  94. chemistry

    The solubility product constant (Ksp) for the dissolution of Cu(OH)2 as represented by the chemical equation is 2.6 x 10-19. Cu(OH)2 (s) Cu2+ (aq) + 2 OH- (aq) Calculate the moles of Cu(OH)2 that dissolves in 1900 mL of water. i know how to do it when its
  95. AP Chem (Thanks!)

    Hey guys! Stuck on some! My maybe answers are written next to the problem (1 problem-5 parts). Thanks for any help: 1. Lead (II) chromate, PbCrO4, is a slightly soluble salt. Write a net ionic equation for the dissolution of solid PbCrO4 in water. My
  96. Chemistry(Please help)

    What is the molar solubility of barium phosphate in a 0.282M barium acetate solution? If I set up and ice table I would have 0.282M - X = ? Would I use the molar mass of barium acetate to complete the equation to find X? Ba3(PO4)2 ==> 3Ba^2+ + 2PO4^3-
  97. Chemistry

    The osmotic pressure (T=25°C) of a saturated solution of CaC03 is 0.0179 atm. Determine the solubility product of the salt
  98. Chemistry

    If the concentration of a saturated solution of SrCO3 is 0.000040 mol*L^-1, what is the value for the solubility product constant of this salt. How do I start this please
  99. science

    In an experiment to determine the solubility of lead chloride (PbCl2), 5.6g of (NH4)2SO4 was added to a 250ml solution containing an unknown amount of dissolved lead chloride (PbCl2) resulting in the formation of Lead sulfate precipitate. The mass of the
  100. Solubility of a Salt - Chemistry

    a) How many grams of potassium nitrate (KNO_3) can be dissolved in 100 mL of water at 30°C, 60°C, and 70°C? b) How many grams of potassium nitrate should be added to 100 mL of water at 25°C to make a saturated solution? c) The solubility of potassium