50.0 mL of saturated 0.020 M Ca(OH)2 is titrated with 20. mL of 0.10 M HF to reach the equivalence point. What is the concentration of the CaF2 at the equivalence point? Ca(OH)2 + 2HF → CaF₂ + 2H₂O Coefficient ?] x 10²] M [CaF₂] = [?] x Exponent Enter
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- 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,…A reprecipitation was employed to remove occluded nitrate from BaSO4 precipitate prior to isotopic analysis of oxygen for geologic studies.9 Approximately 30 mg of BaSO4 crystals were mixed with 15 mL of 0.05 M DTPA in 1 M NaOH. After dissolving the solid with vigorous shaking at 708C, it was reprecipitated by adding 10 M HCl dropwise to obtain pH 3–4 and allowing the mixture to stand for 1 h. The solid was isolated by centrifugation, removal of the mother liquor, and resuspension in deionized water. Centrifugation and washing was repeated a secondtime to reduce the molar ratio NO-3 /SO-4 2 from 0.25 in the original precipitate to 0.001 in the purified material. What will be the predominant species of sulfate and DTPA at pH 14 and pH 3? Explain why BaSO4 dissolves in DTPA in 1 M NaOH and then reprecipitates when the pH is lowered to 3–4.Will a B(OH)2 precipitate form if 50.0 mL of 0.03 M B3X2 is mixed with 350.0 mL of pH 11.5Mg(OH)2 solution at 250C? Ksp of B(OH)2 is 2.1 x 10−13.
- Consider the titrimetric determination of acetic acid (60.05 g/mol) in vinegar. Titration of a 5.00 mL vinegar sample requires 12.15 mL of 0.250 M NaOH to reach the phenolphthalein endpoint. How many grams of acetic acid are present in the sample?100 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)A 20.0-mL sample of a 0.125 M diprotic acid (H2A) solution is titrated with 0.1019 M KOH. The acid ionization constants for the acid are Ka1 = 5.2 * 10 - 5 and Ka2 = 3.4 * 10 - 10. At what added volume of base does each equivalence point occur?
- The experimental Ksp of calcium hydroxide is _________ x 10-6 if 23.09mL of the sat. calcium hydroxide solution was titrated with 12.53mL of 0.049M HCl(aq), considering 4 as an exact value for the calculation?The Ksp of a salt is given to be 3.5 x10-7. The salt contains a cation with a +2 charge and an anion with a -3 charge. What is the molar solubility of the salt in mol/L. What is the molar solubility of MgO in a solution that is .0061 M in MgCl2? The Ksp for MgO is 7.77 x 10-10The Ksp of Ag2CO3 (MM = 275.81 g/mol) at 25°C is 8.1 x 10-12a. Calculate the molar solubility of Ag2CO3 at 25°C.b. What is the solubility of Ag2CO3 in mg/L?
- Mix 4 liters of 0.02 N K2SO4 solution with 6 liters of solution containing 6.62 grams of lead nitrate Pb (NO3) 2. Does precipitate form in this case, given that Ksp of PbSO4 = 10-⁸?The concentration of K+ and Cl- in a saturated solution of KCl is 3.7 M(9a): What is the Ksp of KCl?(9b): Two test tubes each contain 100 mL of saturated KCl and no solid KCl is present in either test tube.100 mL of 6.0 M HCl is added to test tube A and 100 mL of 12 M HCl is added to test tube B. Calculate theconcentrations of K+ and Cl- in both test tubes after mixing but before any reactions happen.(9c): Calculate the reaction quotient, Q, in each test tube.(9d): Predict what you would observe in both test tubes and explain your prediction.A saturated solution of magenusium hydroxide is prepared and the excess solid magneusium hydroxide is settled. A 25.0 mL aliquot of the saturated solution is withdrawn and transfered to a flask, 2 dropfs of indicator are added. A 0.00053 M HCL solution is dispensed from a buret into the solution. The soution changes color after the addition of 13.2 mL. How many moles of hydroxide ion are neutralized in the analysis?