Formula AIPO4 Cd3(PO4)2 Ca3(PO4)2 Li3PO4 With which of the following solutions would a 3.5 x 10€ M solution of PO ³+ ions FORM a precipitate? (Assume the concentrations given are after mixing the solutions.) Ksp 9.84 x 10-21 2.53 x 10-33 2.07 x 10-33 2.37 x 10-4 A) 5.0 x 10-15 M A1³+ B) 5.0 x 10-15 M Cd²+ C) 5.0 x 10-15 M Ca²+ D) 5.0 x 10-15 M Li*

Formula AIPO4 Cd3(PO4)2 Ca3(PO4)2 Li3PO4 With which of the following solutions would a 3.5 x 10€ M solution of PO ³+ ions FORM a precipitate? (Assume the concentrations given are after mixing the solutions.) Ksp 9.84 x 10-21 2.53 x 10-33 2.07 x 10-33 2.37 x 10-4 A) 5.0 x 10-15 M A1³+ B) 5.0 x 10-15 M Cd²+ C) 5.0 x 10-15 M Ca²+ D) 5.0 x 10-15 M Li*

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Magnesium sulfate, MgS04, is added to 72.0 mL of 9.50 x 102 M sodium hydroxide, NaOH, until precipitate just forms. How many grams of magnesium sulfate were added? Assume that the volume of the solution is not changed significantly by the addition of magnesium sulfate. Ksp (Mg(OH)2) = 1.8 x 10-11
Calculate the maximum solubility of calcium fluoride, CaF2 in g/L when in the presence of 0.077 M Ca(NO3)2. The solubility product of CaF2 is 4.2x1011 and CaF2 has a molar mass of 78.08 g/mol. Express your answer to the correct number of significant figures, in scientific notation and include the unit with your answer.
If the concentration of Mg2+ ion in seawater is 1.35 x 10³ mg/L, what OH concentration is required to precipitate Mg(OH)2? Ksp (Mg(OH)2) = 5.6 × 10-¹² OH concentration must be greater than M.
A lab scientist mixes 20.0 mL of a 0.670 M solution of CaCl2 with 10.0 mL of a 0.856 M solution of Li3PO4. How many grams of precipitate did he create and what is the identity of that precipitate (be careful with the balancing of this equation)?
suppose you wanted to remove the lead ions Pb2+ from drinking water without removing the calcium ions (Ca2+) which provided drinking water its distinctive taste. What is the maximuin amount of hydroxide you would add to precipitate out Pb2+ without removing Ca+2. The Ksp for Ca(OH)2 and Pb(OH)2 are 5.5x10^-6 and 2x10^-15, respectively.
A solution contains 1.45x10-2 M sodium carbonate and 9.94x10-3 M ammonium sulfide. Solid copper(II) nitrate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of copper(II) ion when this precipitation first begins? [Cu²+] = M
Determine the mass, in grams, of precipitate that forms when 608, ml. of 0.499 M Na₂CO, reacts with 882. ml. of 0.455 M Ca(OH)₂. Round your answer to 3 significant figures. Ca(OH)₂ (aq) + Na₂CO, (aq) Caco, O.P - 2NaOH(aq) + CaCO, (s)
11c.
A solution contains 7.27x103 M lead nitrate and 1.16x102 M calcium acetate. Solid ammonium sulfate is added slowly to this mixture. What is the concentration of lead ion when calcium ion begins to precipitate? [Pb2*] =| M
If a student uses 1 mg K2CrO4 as indicator for 100 mL of NaCl sample solution, what is the concentration (M) of chloride ion in the solution when red precipitate (Ag2CrO4) starts to form?
+2 When excess Na,So, solution was added to 20.0 mL of an unknown solution containing Ca 0.0472 g of Caso, precipitated. What is the molar concentration (molarity) of Ca ion, in the unknown solution? (molar mass of CaSo, - 136.14 g/mol A) 1.36 x 10 B) 2.47 x 10 C) 2.10 x 10 D) 1.73 x 10 E) 3.83 x 10 Select one: a. 2.10 x 10 2. b. 1.73 x 10 c. 1.36 x 10 -2 d. 3.83 x 10 e. 2.47 x 10 1- Which of the following pairs of aqueous solutions would not produce a reaction when mixed? Select one: a. Cacl, and Na PO, b. AGNO, and HCI c. NaNO, and CuCl, d. Ba(OH), and HNO, e. Which of the following groups of elements is arranged correctly in order of increasing first ionization energy? Select one: a. Al < B< O
Step 1 Lead(II) ions of Lead(II) nitrate reacts with chloride ion of NaCl to form a PbCl2 precipitate. Pb2+(aq) + 2Cl-(aq) →PbCl2(s) arrow_forward Step 2 The precipitate of PbCl2 starts forming when the reaction quotient (Q=[Pb2+][Cl-]2) is greater than the solubility product of PbCl2. The solubility product of PbCl2 is Ksp=1.17×10-5 To find the concentration of chloride ion that starts the precipitation of PbCl2, equate Q to solubility product and solve for the concentration of Chloride ion. [Pb2+][Cl-]2 =1.17×10-5 [Cl-]2 =1.17×10-5[Pb2+] [Cl-] =1.17×10-5[Pb2+] [Pb2+] = concentration of lead(II) nitrate solution [Cl-] =1.17×10-51.0×10-2=3.4205×10-2 M arrow_forward Step 3 The mass of NaCl needed to start the precipitation of PbCl2 is calculated below. mass of NaCl =[Cl-]×Volume of solution ×Molar mass of NaCl mass of NaCl =3.4205×10-2 M×800 mL ×58.44 gmol mass of NaCl =3.4205×10-2 molL×800 ×10-3 L ×58.44 gmol mass of NaCl =159915.216×10-5 g =1.599 g =1.6