How many moles of CaF2 will dissolve in 3.0 liters of 0.061 M NaF solution? (Ksp for CaF2-4.0 x 10-11) 1.1x 10-8 22x 10-10 3.2x 10-8 3.6 x 10-9 none of these
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- Was wondering how to solve this hw problem? Calcium Flouride (dissociation) K@25 C = 3.94 *10^-11 Calcium fluoride is not very soluble in water. ** Its dissociation is: CaF2 (s) Ca²+ (aq) + 2 F¯ (aq) a. At 25°C, how many milligrams of CaF2 would dissolve in 2.0 L of water? b. What were your initial and final values of Q?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.How many grams of Ag2CO3 will be soluble in 250 ml of 0.180 M AgNO3? (Ksp of Ag2CO3 = 5.95 x 10-10) Cr2O72- + 14 H+ + 6 e ----- 2 Cr3+ + 7H2O Eo = - 1.25 VMnO4- + 8 H+ + 5 e ---- Mn2+ + 4 H2O Eo = - 1.27 VFe3+ + e ------ Fe2+ Eo = - 1.20 VZn2+ + 2e --------- Zn Eo = - 0.76 V ( R = 0.08205 L.atm/mol.K; R = 8.314 J/mol.K; F = 96481 C/mol electron) ΔG = ΔH – TΔS ; E = Eo - 0.0257 ln Q ; ΔG = ΔGo + RT ln Q
- Question 1Consider the sparingly soluble salt silver oxalate, Ag2C2O4. Assume a solution temperature of 25°C in all cases unless otherwise indicated. (a) Calculate the solubility, in mol*L–1 of silver oxalate in distilled water at 25°C. You will need to look up the value of Ksp for silver oxalate in your textbook, the reference sheet from the previous solubility worksheet, or online. (b) Is the solubility of Ag2C2O4 at pH 3 expected to be greater than, less than, or equal to its solubility in distilled water at pH 7? Justify your answer using at least one chemical equation as part of your explanation. Answer for part 'a' already found, so just need answer and explanation for part 'b'. Ksp for silver oxalate provided. Please include a chemical equation(s) for part b.Question 1Consider the sparingly soluble salt silver oxalate, Ag2C2O4. Assume a solution temperature of 25°C in all cases unless otherwise indicated. (a) Calculate the solubility, in mol*L–1 of silver oxalate in distilled water at 25°C. You will need to look up the value of Ksp for silver oxalate in your textbook, the reference sheet from the previous solubility worksheet, or online. (b) Is the solubility of Ag2C2O4 at pH 3 expected to be greater than, less than, or equal to its solubility in distilled water at pH 7? Justify your answer using at least one chemical equation as part of your explanation. (c) Calculate the solubility, in mol*L–1 of silver oxalate in the following solutions: (i) 0.200 M AgNO3(ii) 0.150 M K2C2O4 Question 2Calculate the concentrations of all ions at equilibrium when 120.0 mL of 0.336 M Fe2(SO4)3 is mixed with 160.0 mL of 0.560 M KOH. You will need to identify the precipitate and look up the value of Ksp for that precipitate. Assume a temperature of at 25°C…Ksp of Cd(IO₃)₂ (462.22 g/mol) is 2.3 × 10⁻⁸. How much dissolved Cd(IO₃)₂ is in a 750.0 mL Cd(IO₃)₂ clear solution? Choices: 621.1 mg 52.57 mg 985.9 mg None of these
- Ksp for MgF2=5.2 x 10-11 Calculate the solubility in 1) Moles/L (Molarity) and 2) g/LWhat mass of NicO3, will dissolve in 1.2 L of 0.435 M Na2CO3 solution? Ksp of NICO3, is 6.6x10^-9What is the cobalt(II) ion concentration in a solution prepared by mixing 357 mL357 mL of 0.396 M0.396 M cobalt(II) nitrate with 475 mL475 mL of 0.399 M0.399 M sodium hydroxide? The ?spKsp of cobalt(II) hydroxide is 5.92×10−155.92×10−15 .
- Chemistry written by hand. Calculate the concentration of F- using M1V1=M2V2 if 0.027g of NaF was used to make 250.00 ml of 50 ppm F- stock solution. Thank you. Details and clear steps please and thank you.What hydrogen I on concentration should be required to dissolve 0.10 M MgF2 if the Ksp for magnesium fluoride is 6.8*10^-9 and Ka for HF is 6.5*10^-4?Knowing that Ksp of PbI2 = 10-⁷ find out if precipitate will form when mixing 100ml of 0.01 N Pb solution (NO3) 2 and 200ml of 0.01 M NaI solution