(i)
Interpretation: The mathematical relation between solubility product,
Concept introduction: At equilibrium, the measure of maximum amount of solute that is to be dissolved in a solvent is known as solubility. Solubility product is defined as the product of concentration of ions in a saturated solution where each ion is raised to the power of their coefficients.
(ii)
Interpretation: The mathematical relation between solubility product,
Concept introduction: At equilibrium, the measure of maximum amount of solute that is to be dissolved in a solvent is known as solubility. Solubility product is defined as the product of concentration of ions in a saturated solution where each ion is raised to the power of their coefficients.
(iii)
Interpretation: The mathematical relation between solubility product,
Concept introduction: At equilibrium, the measure of maximum amount of solute that is to be dissolved in a solvent is known as solubility. Solubility product is defined as the product of concentration of ions in a saturated solution where each ion is raised to the power of their coefficients.
(iv)
Interpretation: The mathematical relation between solubility product,
Concept introduction: At equilibrium, the measure of maximum amount of solute that is to be dissolved in a solvent is known as solubility. Solubility product is defined as the product of concentration of ions in a saturated solution where each ion is raised to the power of their coefficients.
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Chapter 16 Solutions
Chemistry: Cengage Technology Edition
- 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,…arrow_forwardCalculate the molar solubility of BaCrO4. Ksp of BaCrO4 = 1.2 x 10-10arrow_forwardCalculate the Molar Solubility and Ksp of Borax. I have included the data and some calculation that can help with solving, but I am unsure if the calculation I have provided are accurate Data: 1. Concentration of standardized HCl Solution (mol/L) = 0.1563M 2. volume of saturated borax (mL) = 5 mL 3. Buret reading, initial (mL) = 24.60 mL 4. Buret reading, final (mL) = 29.53 mL 5. Volume of HCl added (mL) = 4.93mL Calculations: 6. Amount of HCl added (mol) = 0.00077mol 7. Amount of OH- in saturated solution (mol) = 8. [OH-] equillirium (mol/L) = Molar solubility of borax=? Ksp of borax=?arrow_forward
- Which of the following compounds will have the highest molar solubility in pure water? A) PbSO4, Ksp=1.82•10-8 B) MgCO3, Ksp=6.82•10-6 C) AgCl, Ksp=1.77•10-10 D) CdS, Ksp= 8.00•10-28 E) HgS, Ksp= 1.60•10-54 please show work if necessary or explain why.arrow_forwardCalculate the Molar Solubility of Calcium Hyroxide in the Presence of a Common Ion (CaCl2) I have included the data and some calculation that can help with solving, but I am unsure if the calculation I have provided are accurate Data: 1. Concentration of standardized HCl Solution (mol/L) = 0.0646 2. volume of saturated Ca(OH)2 with added CaCl2 solution (mL) = 25 mL 3. Buret reading, initial (mL) = 0.03 mL 4. Buret reading, final (mL) = 19.85 mL 5. Volume of HCl added (mL) = 19.82mL Calculations: 6. Amount of HCl added (mol) = 1.28x10^-3 7. Amount of OH- in saturated solution (mol) =1.28x10^-3 8. [OH-] equillirium (mol/L) =5.12x10^-2 Molar solubility of Ca(OH)2=?arrow_forwardHow would you use an experimentally determined Ksp value to calculate that Ag2CrO4 should precipitate when 5ml of 0.0040 M AgNO3 are added to 5ml of 0.0024 M K2CrO4. You can come up with your own experimentally Ksp value. I just want to see steps in solvingarrow_forward
- The molar solubility of Ca3(PO4)2 is 1.14×10-7 mol/L at 25°C. Calculate the solubility of Ca3(PO4)2 at 25°C in g/L and Calculate Ksp at 25°C.arrow_forwardConsider the dissolution of slightly soluble salt, PbCl2 (Ksp = 1.70 x 10-5): PbCl2(s) ⇌ Pb2+(aq) + 2Cl-(aq) Calculate the molar solubility of PbCl2 in:a. Pure Water b. 0.10 M Pb(NO3)2 Express the answer in four decimal placesarrow_forwardCalculate the molar solubility and solubility in g/L of lithium fluoride (LiF, 25.939 g/mol) in pure water. Ksp = 1.7 x 10-3 Calculate the molar solubility and solubility in g/L of gold(III) chloride (AuCl3, 303.33 g/mol) in pure water. Ksp = 3.2 x 10-25 Calculate the molar solubility and solubility in g/L of gold(III) chloride in a solution that is 0.010 M in MgCl2. Ksp = 3.2 x 10-25arrow_forward
- The Ksp for BaSO4 is (1.1 x 10-10) and that for BaSeO4 is (2.8 x 10-11), A 1 Molar solution of BaCl2 is added slowly to a solution that is 1.0 x 10¯4 Molar of sodium sulfate Na2SO4 and 1.0 x 10¯4 Molar of sodium selenate, Na2SeO4. What is the approximate percentage of one anion has precipitated at the point which the second anion just begins to precipitate? (Assume the addition of the BaCl2 solution does not change the overall solution volume to any significant degree.)arrow_forwardCalculate the molar solubility of Hg2C2O4(Ksp= 1.75 x 10-13) in 0.13 M Hg2(NO3)2.arrow_forward5, Calculate the molar solubility of Cobalt(II) hydroxide (blue) Co(OH)2 in pure water [ Select ] ["4.11x10-4", "1.14x10-5", "2.54x10-6", "5.24x10-3"] in 0.50M NaOH [ Select ] ["2.37x10-10", "7.32x10-13", "2.37x10-14", "3.27x10-7"] Ksp of Co(OH)2 = 5.92 ⋅ 10–15 6, In the supersaturated solution Group of answer choices Q = Ksp Q < Ksp Q > Ksp Ka = Ksp Calculate the pH of a buffer solution prepared by mixing 25 mL 0.400 M butyric acid, HC4H7O2 and 35 mL of 0.200 M potassium butyrate, KC4H7O2. Ka of butyric acid is 2.76 x 10-6. Group of answer choices 5.40 3.60 6.30 4.50arrow_forward
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