Calculate the solubility at 25 °C of CaF, in pure water and in a 0.0110M NaF solution. You'll find K, data in the ALEKS Data tab. sp Round both of your answers to 2 significant digits. solubility in pure water: solubility in 0.0110 M NaF solution: Dlo
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- Calculate the solubility at 25°C of Zn(OH)2 in pure water and in a 0.0080M ZnSO4 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. ksp of zn(OH)2 =3.0×10−17 solubility in pure water: gL solubility in 0.0080 M ZnSO4 solution: gLIn lecture I mentioned that standard state is usually at 25oC; however, it can be at any specified temperature. In problems 9 and 10 you will calculate ΔGo from Ksp data. The Ksp range over the temperature range in these two problems is consistent with some actual solubility data; however, in order to allow each student to do their own calculation I have made this data for an "unknown" ionic solid. Calculate the value of ΔGo (kJ/mol) at 3.3oC for the dissolution of an ionic solid with a Ksp of 2.5 x 10-11 at 3.3oC. Your answer should have 2 sig figs.Calculate the solubility of lead(II) sulfate (Ksp = 2.53x10-8) in a 0.0034 M solution of sodium sulfate. Give your answer to three sig. figs. and in exponential form (e. g. 1.23E-3).
- By the use of Henderson Hasselbalch equation; pH = pKa + log{[acetate ion]/[acetic acid]} 4.5 = 4.75 + log{[0.10 M]/[acetic acid]} -0.25 = log{[0.10 M]/[acetic acid]} [Acetic acid] = 0.10 M/ 10-0.25 [Acetic acid] = 0.10 M/0.56 [Acetic acid] = 0.1786 M Moles of sodium acetate dissolved in 250 mL buffer solution = 0.10 M× (250mL/1000mL) × 1L = 0.025 mol Weight (w) of sodium acetate (purity 100%) dissolved to prepare 250 mL of solution with buffer concentration of 0.10 M is calculate as follow; w100% = 0.025 mol × 82.0343 g/mol = 2.051 g Weight (w) of sodium acetate (purity 99%) is calculate as follow; w99% = 2.051 g× (100/99) = 2.072 g What was the volume of 6.12 M acetic acid HC2H3O2 needed to prepare the 250 mL acetic acid/acetate ion buffer solution required in this part? Show your calculations.The following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mL. A solution was prepared by mixing 4.00mL of 2.00 x 10-3 M Fe(NO3)3 and 3.00mL of 5.00 x 10-3 M NaSCN and diluting the mixture with water to a total of 10.00mL. Use your average value of Kc to calculate the equilibrium concentration of FeSCN2+ in the mixture. [Hint: Use as many significant figures as you legitimately can in your calculations] my average you can find on the picture below PLS HELP ASAP!!
- The student then determined ΔH neutralization for the reaction of sodium hydroxide and acetic acid, using the procedure described in this module. The student added 100.0 mL of 0.8500M NaOH to 100.0 mL of 0.8404M acetic acid. Prior to and following the mixing of the acid and base solutions, the following temperature-time data were collected. g) Identify the limiting reagent and briefly explain why it is limiting. h) Find ΔH neutralization for the reaction.1. The Ksp of Ca3(PO4)2 is 1.3 × 10−26. Estimate the solubility of this salt in units of g. L−12. If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence. Please only answer 2nd QuestionA chemist mixes 10.0 mg of Ca(NO3)2 to a 100.0 mL sample of 0.010 M Na2C2O4 at 25 oC. Assume the volume of solution does not change. Given that for CaC2O4, Ksp = 2.7 x 10-9 at 25 oC, determine a) the value of Qsp (number and magnitude) of CaC2O4 dissolution and b) whether a precipitate should form.
- Note: Express % strength with 4 decimal places. For ratio strength, state the volume only% Astelin nasal spray contains 0.1% azelastine hydrochloride and 125 mcg/mL of benzalkonium chloride as a preservative. A container is capable of delivering 200 metered sprays of 0.137 mL each. The percent concentration of benzalkonium chloride in the preparation is _______%, which is equivalent to a ratio strength of 1 in _____ w/v.In an experiment to calculate the solubility product (Ksp) of barium nitrate (Ba(NO3)2), an excess amount of Ba(NO3)2 was added to 2 liters of water at 25oC until the solution is saturated. Because Ba(NO3)2 is only slightly soluble in water, the excess Ba(NO3)2 was filtered out to get a solid-free mixture. The proponents of the experiment thought about using the concept of colligative properties, specifically boiling point elevation, to determine Ksp. It was observed in their experiments that the solution boils at 100.15 K. Barium nitrate dissociates via the process: Ba(NO3)2(s) ⇄ Ba2+(aq) + 2NO?-3(?q) Ksp = [Ba2+][NO3−]2 Calculate the following if Kb,water = 0.51 K-kg/mol: a) Amount of Ba(NO3)2 dissolved in grams. Molar mass of Ba(NO3)2 = 261.3 g/mol b) Solubility product, Ksp c) Vapor pressure of the solution in kPaIn an experiment to calculate the solubility product (Ksp) of barium nitrate (Ba(NO3)2), an excess amount of Ba(NO3)2 was added to 2 liters of water at 25oC until the solution is saturated. Because Ba(NO3)2 is only slightly soluble in water, the excess Ba(NO3)2 was filtered out to get a solid-free mixture. The proponents of the experiment thought about using the concept of colligative properties, specifically boiling point elevation, to determine Ksp. It was observed in their experiments that the solution boils at 100.15 K. Barium nitrate dissociates via the process: ?a(??3)2(?) ⇄ ??2+(?q) + 2??-3(?q) ??p = [??2+][??3−]2 Calculate the following if Kb,water = 0.51 K-kg/mol: a) Amount of Ba(NO3)2 dissolved in grams. Molar mass of Ba(NO3)2 = 261.3 g/mol b) Solubility product, Ksp c) Vapor pressure of the solution in kPa