Does any solid PbCl2 form when 0.30 L of 0.86M NaCl is dissolved in 0.25 L of 0.12 M Pb(NO3)2? Ksp (PbCl2) = 1.6x10-5 [Select] Choose the reason to confirm your answer from the following. [Select] [Select] Q> Ksp Q< Ksp Q = Ksp PbCl2 (s) Pb2+(aq) + 2CI (aq)
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![Does any solid PbCl2 form when 0.30 L of 0.86M NaCl is dissolved in 0.25 L of 0.12 M Pb(NO3)2? Ksp (PbCl2) = 1.6x10-5
[Select]
Choose the reason to confirm your answer from the following.
[Select]
[Select]
Q> Ksp
Q< Ksp
Q = Ksp
PbCl2 (s) Pb2+(aq) + 2CI (aq)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf5692e5-2038-43a6-b294-65954a0835a6%2F03a8dfa5-0501-4726-80ef-87a2fcdd3c21%2Fujaj1c_processed.jpeg&w=3840&q=75)
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- A solution is prepared by mixing 20.0 mL of 0.100M Fe(NO3)3 with 20.0 mL of 0.00300M KSCN and 10.0 mL of DI water. Calculate the initial concentration of Fe^3+ in this solution? Give answer with correct amount of sig figs.Calculate the final [Ag1+] concentration in solution when 0.035 moles of AgNO3 are added to 500. mL of 0.21 M NaCN. Assume the volume remains constant. Ksp = 1.2 ✕ 10-16 for AgCN. (in M)a. Lead(II) chloride is a white pigment used in 15-century European sculptures. If 275 mL of a 0.134 M Pb(NO3)2 solution is added to 125 mL of a 0.0339 M NaCl solution and the Ksp of lead(II) chloride is 1.7x10-5, will a precipitate form? b. If your answer to part a was YES, calculate the grams of lead(II) chloride in solution. If your answer to part a was NO, calculate the minimum molarity of the 125 mL NaCl solution required to precipitate lead(II) chloride when added to 275 mL of 0.134 M Pb(NO3)2.
- If you had used 40mL of wash water to was .8555g of AgCl precipitate, and yhe wash water became 60% maximum saturation, how many grams of AgCl would you be washing away? Ksp for AgCl=1.8x10^-10 what % error too low would be in ur final answer, ie what % of the solid would be washed away96 mL of 0.080 M NaF is mixed with 32 mL of 0.20 M Sr(NO3)2. Calculate the concentration of Sr2+ in the final solution. Assume volumes can be added. (Ksp for SrF2 = 2.0 ×10-10)Use the Solver function in Excel to determine [Sr2+][Sr2+], [F−][F−], [HF][HF], [OH−][OH−], and [H+][H+] for a saturated solution of SrF2SrF2. The p?sppKsp for SrF2SrF2 is 8.588.58. The p?apKa for HFHF is 3.173.17. Ignore activity coefficients.
- A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in a volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M sodium hydroxide to reach the phenolphthalein endpoint From this experiment which is the standard solution used in titration? CH3COOH NaOH NaCH3COO C20H14O4100 ml 0.10M AgNo3 is added 100 ml of 0.12 M Nacl (ksp agcl = 1x10^-10) 1. CALCULATE THE NUMBER OF MILLIGRAMS of Ag+ not precipitate (m. W of ag = 107.8 g/mol) 2. If precipitate of agcl is washed with 200 ml of water at 25 c what is yhe maximum number of milligrams of agcl that could be lost by solubility in the wadh water? ( m. W agcl = 143,32 g /mol)The solubility of Fe(OH)3 is measured and found to be 2.30×10-8 g/L. Use this information to calculate a Ksp value for iron(III) hydroxide.
- Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3A solution of Na3AsO4 is added dropwise to a solution that is 0.0576 M in Cu2+ and 0.000398 M in Ag+.The Ksp of Cu3(AsO4)2 is 7.95e-36.The Ksp of Ag3AsO4 is 1.03e-22.(a) What concentration of AsO43- is necessary to begin precipitation? (Neglect volume changes.)[AsO43-] = ______M.(b) Which cation precipitates first? Cu2+Ag+ (c) What is the concentration of AsO43- when the second cation begins to precipitate?[AsO43-] = _____M.1 ) The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is 2) Calculate the pAg^ + at the equivalence point in the titration of 25.0ml of 0.0823 M Kl with 0.051M AgNO 3 . Ksp Agl=8.3*10^ -16 3) Commercial concentrated aqueous nitric acid is 70.4% HNO3(63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is 4) Consider the titration of 25ml of 0.0823M KI with 0.051M AGNO3, Kspagi =8.3x10-16 Calculate pAg* after adding 39.0 ml I03 Ag* + 103 ====AglO3 5) Commercial concentrated aqueous nitric acid is 70.4 1\%HNO 3 (63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is: 6) What mass in g of Na 2 CO 3 [106 g/mol] is required to prepare 250 ml of 0.3M aqueous solution in Na^ + [23.g/mol] ? 7) Calculate pAg^ + after adding 42.30ml AgNO 3 In the titration of of 0.0823M Kl with 0.051M AgNO 3 . KspAgl = 8.3 * 10 ^ - 16 8) The milliliters of concentrated HClO 4 (100.5 g/mol),6 60% by mass,…