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- Flammability is a measure of how easily a substance bursts into flame, through fire. It is is a chemical reaction that occurs between a fuel and an oxidizing agent that produces energy, usually in the form of heat and light. O True O FalseExpress the quantity 33.2×10−4m33.2×10−4m in mmmm.when an acid is added to sodium bicarbonate gas is formed. when dry ice sublimes, gas is formed. one process is chemical and the other is physicsl. Explain.
- You need to prepare a solution of 0.123M CuSO4 by starting with solid CuSO4·5H2O. You would be able to use a lab scale that measures to the thousandths and any size volumetric flasks, and pipets that you would need.1 Hydrogen peroxide solutions can easily be decomposed by dust, trace amounts of metals or light. It is therefore necessary to periodically determine the purity of the peroxide solutions. This can be done via a redox titration as follows: • The density of a particular surgical grade hydrogen peroxide solution is 1.11g.cm³. • Exactly 10 mL of this solution was pipetted and quantitatively transferred, along with a sufficient amount of a dilute sulphuric acid solution, into a 250.00 mL volumetric flask and made up to the mark. • A 25.00 mL portion of this diluted solution is pipetted into a conical flask, and titrated with a 0.372 M KMNO4 solution. • The endpoint of the titration is determined when the colourless solution in the conical flask turns a persistent bright pink due to the presence of excess permanganate ions. • The average titration value is 26.20 mL of the KMNO4 solution. The reaction stoichiometry is as follows: 2KMN0,(aq) + 3H280,(aq) + 5H20, (aq) → 2MNS0,(aq) + K2s0,(aq) +…A student weighs out 0.213 g MgCl2·H2O (Mw = 131.235 g mol-1) of and 0.167 g of NaOH (Mw = 39.997 g mol-1 ) and dissolves both these in DI water to make up two separate solution. What are the mole amounts of both these reagents and which is the limiting reagent?
- A 0.200 M K2SO3 solution is produced by A) diluting 250.0 mL of a 1.00M K2SO3 solution to 1.00 L B) diluting 100.0 mL of a 2.50 M K2SO3 solution to 250.0 mL C) diluting 20.0 mL of a 5.00 M K2SO3 solution to 500.0 mL D) diluting 1.00 mL of a 250M K2SO3 solution to 1.00 L O B C OD O Alook at the dissolution of solid sodium chloride in water. In answering the following questions, you may draw, but not replace, your explanation with the drawing a) Describe the structural features and type of chemical bonding that exists in solid sodium chloride. b) Describe the structural features and the type of chemical bonding that exist in water molecules. c) Explain how water molecules dissolve salts like sodium chloride.What happens if a solute is added to a saturated solution? A) Nothing will happen, solute will not mix with a saturated solution. B) The added solute provides a template for the solid to begin to crystallize from solution, and a precipitate will form. C) The added solute makes the solution less saturated. D) The added solute provides a template for the gas to begin to boil from solution, and a gas will form. Why is A false?
- The following evidence was obtained from an experiment to determine the molar concentration of a sodium nitrate solution. A sample of sodium nitrate solution was evaporated to dryness and the mass of solid residue was measured.Evidence:Volume of solution = 10.00 mLMass of beaker = 79.54 gMass of beaker and residue = 82.96 gFrom this data, calculate the molar concentration of the original sodium nitrate solution. Record only your numerical answer with the correct number of significant digits. You do not need to include units as the units appear for you beside the answer box already.For the reaction that occurs when aqueous solutions of Sr(C104)2 and Ag2SO4 are mixed; which of the following is correct? I. SRSO4 precipitates II. AgC104 precipitates III. Ci04 is a spectator ion IV. SO42 is a spectator ion (Solubility Rules are given as below) • All salts of ammonium (NH4) and Group I metals (Li, Na, K, Rb, Cs) are soluble in water. • All Chlorides (CI), Bromides (Br") and Iodides (I) are soluble in water; except those of silver (Ag), mercury(I) (Hg"), and lead(II) (Pb2+). • All Nitrates (NO3), Chlorates (C103), Perchlorates (C104) and Acetates (C2H302) are soluble in water. • All Sulfates (SO42-) are soluble in water; except those of mercury(I) (Hg*), lead(II) (Pb2+) strontium (Sr2*) and barium (Ba2+). • All Oxides (O2), Carbonates (CO32-), Phosphates (PO43) and Oxalates (C2042-) are insoluble in water; except those of Group I and NH,* are soluble. • All Hydroxides (OH) and Sulfides (S2-) are insoluble; except those of Group I and NH4* are soluble, calcium (Ca2") &…Drainage from agriculture contains phosphate ions from fertilizers and pesticides, thus, contributes to environmental pollution. true false
