19. What is the experimental K of CACO, if the residue after evaporation of a - 1.00 L saturated solution is found to have a mass of 0.006 90 g? CaCOg(8) Ca*(aq) + CO3 (ag) 20. For a saturated silver chromate solution, the molar concentration of CrO is - 6.54'X 10- M, and the K of Ag2CrO4 is 1.12 x 10- at equilibrium. Calculate the concentration of Ag* in the solution. sp Ag2CrO4(s) 2Ag*(aq) + CrO (ag)
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- In an experiment to determine the concentration of H2SO4 in a brand of toilet cleanser, 10.0 cm3 of the cleanser was first diluted to 250.0 cm3 with distilled water. 25.0 cm3 of the diluted cleanser were titrated with 0.320 mol dm–3 NaOH solution, using methyl orange as indicator.If 29.2 cm3 of NaOH solution is used, what is the concentration of H2SO4 in the undiluted toilet cleanser?a. 2.30 mol dm–3b. 4.60 mol dm–3 c. 9.20 mol dm–3 d. 11.50 mol dm–3If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility = mol/LIn the determination of chloride by the Mob method, what will be the equiliblium concentration of silver ions in mgil, on the basis of the solubility product principle, when the chloride concentation has been reduced to 0.2 ma? (b) If the concentration of chromate indicator used is 5X M, how much excess silver ion in mgil must be present before the formation of a red precipitate will begi(a) In the defermination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in meL., an the basis of the solubility. pcoduct principle, when the chloride concencration has beea reduced to 0.2m 1.2m? (b) If -3 the concentration of chromate indicator ased is 5 x 10M, bow much excess silver ion in mel, must be present before the formatice of a red precipitate will begin?
- For µ=0.1, the activity coefficient (gamma) of M2+ is 0.41 while gamma of X- is 0.75. Calculate how many micrograms of MX2 dissolve in 324 mL of 0.10 M NaX solution. The molar mass of MX2 is 201 g/mol, and its Ksp is 3.8 x 10-9. Note that NaX is a salt of X-, an ion that participates in the equilibrium that applies to the solubility of MX2. a. 110 µg b. 27 µg c. 9.7 µg d. 44 µg e. 1000 µgWill Mn(OH)2 precipitate from a 0.01 M solution of MnCl2 at pH = 9? Ksp(Mn(OH)2) = 1,0 x 10-13. Discuss from solubility diagrams and prove by calculation.calculation. Co is a metal that is present in every lithium battery to stabilize its charge and toincrease stability. Every cell phone, tablet and electric car relies on the availability ofcobalt, 97% of which is extracted from mines in places like the Congo, where essentially slave labor is used.Cobalt ions form complexes with e.g. CN- . You see solubility diagrams and fraction diagrams for CoCO3 with and without the addition of 10 mM CN- .. Explain whythe solubility of cobalt carbonate increases at high pH when cyanide ions are present.Write reaction formulas for the formation of the dominant cobalt cyanide complexes.Calculate the solubility (in g/L) of silver chromate in water at 25°C if the Ksp for Ag3PO4 is 1.75 × 10-18. Ag3PO4(s) <==> 3Ag+ (aq) + PO43- (aq); Ksp = 27s4, s = _________ mol/L x MM of Ag3PO4 = _________ g/L.
- The cations in an aqueous solution that contains 0.150 M Ba(NO3)2 and 0.0800 M Ca(NO3)2 are to be separated by taking advantage of the difference in the solubilities of their sulfates. Ksp(BaSO4) = 1.1 × 10-10 and Ksp(CaSO4) = 2.4 × 10-5 . What should be the concentration of sulfate ion for the best separation?The solubility of Ag2CrO4 (Ksp = 1.2 x 10-12) is several times greater than that of AgCl (Ksp = 1.82 x 10-10), so the red precipitate cannot form until all the chloride ions have effectively been removed from the solution. If a student uses 1 mg of K2CrO4 Aas an indicator for 100 mL of sample solution, what is the concnetrion of chloride ion in the solution when the red precipitate (Ag2CrO4) starts to form?A 1 L solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. A. Can the metal ions be separated by slowly adding Na2CO3? Assume that for successful separation 99% of the metal ion must be precipitated before the other metal ion begins to precipitate, and assume no volume change on addition of Na2CO3. Ksp of CuCO3 = 1.4 x10-10Ksp of NiCO3 = 1.42X 10-7B. What would be the Molarity of Na2CO3 you will use in A , so that assumption of no volume change on addition of Na2CO3 will be valid ? please answer only B.
- Enough silver sulfite (Ag2SO3 , Ksp = 1.5 × 10-14 ) is dissolved in 2.00 L to produce a saturated solution. Calculate the mass of silver sulfite that dissolved in 2.00 L in a neutral solution and in a pH = 2.00 solution.The solubility of Ag2CrO4 (Ksp = 1.2 x 10^-12) is several times greater than that of AgCl (Ksp = 1.82 x 10^-10), so the red precipitate cannot form until all the chloride ions have effectively been removed from the solution. If a student uses 1 mg of K2CrO4 as an indicator for 100 mL of sample solution, what is the concentration (M) of chloride ion in the solution when the red precipitate (Ag2CrO4) starts to form?What is the maximum solid solubility of Mg in Al? At what temperature does it occur? e. An Al-Mg alloy (10 wt% Mg, 90 wt% Al) is heated slowly (to insure equilibrium) from a temperature of 200 C: i. At what temperature does the first liquid phase form? ii. What is the composition of the liquid phase at the temperature in part i.? iii. At what temperature does complete melting (no solid phase remaining) occur? iv. What is the composition of the last solid remaining prior to complete melting? f. Using the equilibrium phase diagram of Figure 1, identify the phases present, their compositions, and their relative mass fractions at equilibrium for a 70 wt% Mg – 30 wt% Al alloy held at 300 C.