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- Give the formula of a compound which will give a precipitate with KI and K3PO4? SOLUBILITY RULES Solubilities of ionic substances in water: 1) All salts of Na+, K+, NH4+ are soluble in water. 2) All salts of NO3-, CH3COO- (C2H3O2-) are soluble in water. 3) All salts of Cl-, Br-, I- are soluble in water (except Ag+, Pb2+, Hg22+ ) 4) All salts of SO42- are soluble in water ( except Ba2+, Pb2+, Sr2+) SO42- of Ca2+, Ag+, Hg22+ are slightly soluble in water. 5) All salts of CO32-, PO43- are insoluble in water (except Na+, K+, NH4+) 6) All salts of S2- are insoluble in water ( except Na+, K+, NH4+, Ba2+,Ca2+, Mg2+, Sr2+) 7) All salts of O2-, OH- are insoluble in water ( except Na+, K+, NH4+, (Ba2+)) OH- of Ca2+, Sr2+, (Ba2+) are slightly soluble in water OH- of Mg2+ is very very slightly soluble in water STRONG ACIDS STRONG BASES HCl LiOH HBr…A 0.7802-g sample is dissolved in cyanide solution to convert its sulfur (32.066 g/mol) to thiocyanate. 43.51 mL of 0.2352 M potassium iodate solution in strong hydrochloric acid. What is the % w/w S of the sample? CHOICES: 14.02% 28.04% 42.06% None of theseThe digestion of a 0.1159 gram sample of a phosphorous-containing compound in a mixture of HNO3 and H2SO4 resulted in the formation of CO2, H2O, and H3PO4. Addition of ammonium molybdate yielded a solid having the composition (NH4)3PO4·12MoO3 (FW = 1876.3). This precipitate was filtered, washed, and dissolved in 50.00 mL of 0.2000 M NaOH: (NH4)3PO4•12MoO3(s)+26OH-(aq)->HPO42-(aq)+12MoO42-(aq)+14H2O(l)+3NH3(g) After the solution was boiled to remove the NH3, the excess NaOH was back-titrated with 14.84 mL of 0.1626 M HCl to a phenolphthalein end point. Calculate the percent phosphorous (FW = 30.9737) in the sample.
- Why is Mg2+ Most likely to give a precipitate with PO43- explain the answer4.87 Determine the mass of product that will precipitatewhen 50.0 mL 0.135 M Pb(NO3)2 and 50.0 mL of0.250 M KCl are combined.A sample of 0.0500 M barium nitrate solution and 0.0500 M sodium sulfate solution was labeled with radioactive . The radioactivity of the initial sodium sulfate solution was 1.22 x106 counts per second. After the formation of the precipitate and purification by filtration the remaining radioactivity in solution was 250 counts per second. Calculate the Ksp for the following dissociation: BaSO4(s) ↔Ba+2(aq) + SO4-2(aq) Group of answer choices 5.96x104 1.02x10-5 1.05x10-10 5.12x10-7
- How many grams of PbF2 (molar mass = 245.2) will dissolve in 700 mL of 0.60 M NaF solution? The Ksp for PbF2 is 2.69e-08.84 mL of 0.060 M NaF is mixed with 28 mL of 0.15 M Sr(NO3)2. Calculate the concentration of Sr2+ in the final solution. Assume volumes can be added. (Ksp for SrF2 = 2.0 × 10-10) A. 0.038 M B. 0.00012 M C. 0.015 M D. 0.045 M E. 0.075 MMixing 20.0 mL of 5.00 M magnesium chloride solution with 40.0 mL of 2.00 M silver (I) nitrate solution results in a precipitate. The resulting mixture contains a total free chloride ion concentration of: a) 2.86M Cl- b) 2.00M Cl- c)0.120M Cl- d) 0.500M Cl- e) not enough information is provided
- Which ion below is most likely to give a precipitate with PO4 3- ? And explain why NH 4+ H+ Cs+ Mg 2+ NO -3 F- C2H3O2 - SO4 2-A sample of freshly precipitated and filtered silver chloride weighs 459.0 mg. If 1.00 % of the silver chloride becomes photo decomposed, what is the precipitate’s weigh?A solution was made by dissolving 9.0g of hydrated aluminium sulphate Al2(SO)3 in 250cm3 of solution. (R.A.M: Al = 27, O = 16, S = 32, H = 1) Calculate the number of moles of hydrated aluminium sulphate solution the number of moles of sulphate ions in this solution the concentration (moldm-3) of the hydrated aluminium sulphate