3) Fluoridated teeth, CaF2 has a Ks.p. = 6.5 x 10-11. How many grams of Calcium would dissolve per 100 ml : (a) in pure water, (b) in a 0.75M AIF3 solution
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is a sparingly soluble salt and can be partially dissociated as:
If the concentration of calcium fluoride is M, then we can have the following relation:
According to the definition of solubility product, we have
Again, we can write
This will be the final expression of solubility product for
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- How many grams of CaF2 (molar mass 78.077) will dissolve in 250 mL of 0.20 M NaF solution? The Ksp for CaF2 is 3.8904e-11.Calculate the solubility at 25°C of CaF2 in pure water and in a 0.0060M NaF solution. You'll find Ksp data in the ALEKS Data tab. (CaF2 Ksp is 3.45×10−11 Round both of your answers to 2 significant digits. solubility in pure water: ? gL? solubility in 0.0060 M NaF solution:? gL?One gram of sodium hydroxide (NaOH) is used to adjust the pH of an aqueous solution (200 gallons) thatcontains 10 lbs of finely ground rhodochrosite (MnCO3) ore. Does the NaOH raise or lower the solutionpH? What is the amount of NaOH added in lbs/ton? What is the molarity (mol/l) of the system? Assumingthe NaOH is completely soluble and the system is at room temperature, what is the solid-to-liquid ratio(wt%) of the system?
- KNO3 (aq) added to CaC2O4 (Ksp = 1.3 x 10-8) in solution will lead to __________ in solubility of the solid no effect then decrease increase no effect3. To 20,00 ml of 0,1250 mol/l solution of silver nitrate – 25,00 ml of 0,1000 mol/l solution of potassium thiocyanate were added. Calculate pAg of this mixture. pKs(AgSCN) = 11,97 Express numerical result with an accuracy of: Х,ХXPS. Further values required for the solvings are give in the various situations below. (ANSWER) Situation: A community in a mountainous area of Bohol uses water collected from a nearby natural spring. A sample was submitted to a laboratory for the analysis of its total hardness. Required: SHOW YOUR COMPLETE CALCULATIONS. BASED ON THE IMAGE PROVIDED BELOW FOR THIS QUESTION: Calculate the amount of titrant used in each trial to reach endpoint. Report total hardness of the sample as mean ±sd. a. 250.0 mL of 500.0 ppm of CaCO3 solution from a primary standard (assume solvent is distilled water only). Answer : Mass of CaCO3 = 0.125 g b, The EDTA solution was standardized by titrating it with a 25.0 mL aliquot of the CaCO3 solution. How much of the titrant was consumed. Answer: Volume of EDTA consumed = 12.405 g c. Calculate the average titer (mg CaCO3/mL EDTA). Mass of CaCO3 in 25 mL CaCO3 solution: 0.0125 g Answer: 1.008 mg CaCO3/ mL EDTA
- Calculate the solubility at 25° of CaF2 in pure water and in a 0.0010M NaF solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits.In gravimetric analysis, volatile electrolyte is used in peptization step a. to form small nucleib. to easily dry precipitatec. to reprecipitate the analyteexplain please6. A 100mLSolution containing 0.145g of NiCl2 was supplied in the lab. Students were advised to use 5mL of this solution for gravimetric determination of Ni. The density of solution = 1g/mL Mass of precipitate was calculated to be .0291g and .0353g for two trials of the experiment. Calculate the average amount of Ni in unit ppm (parts per million). Gf = .2031
- . 100 ml boiled cooled and filtered water sample takes 9.6 ml of M/50 EDTA in titration. The Permanent hardness of the water sample in terms of ppm of CaCO3 equivalent isA 0.098 M K2Cr2O7 titrant was used for titration of 30 mL of aqueous Ethanol (C2H6O) solution and consumed 41.40 mL. (a) Calculate the mass of Ethanol and (b) determine degree proof of ethanol (density of pure ethanol= 0.789 g/mL).3. On a separate sheet show calculations for: 5.0 mL of water Solubility (g/L) of NiCl₂ = 0.67 Molar solubility of NiCl2 [Ni²+] = [CI] =_ - Ksp for NiCl2 = - g/L 3.35g of Nicla, net 3.359 Nicl₂ /0.0 NICI M M M