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A common experiment to determine the relative reactivity of metallic elements is to place a pure sample of one metal into an aqueous solution of a compound of another metallic element. If the pure metal you are adding is more reactive than the metallic element in the compound, then the pure metal will replace the metallic element in the compound. For example, if you place a piece of pure zinc metal into a solution of copper(II) nitrate, the zinc will slowly dissolve to produce zinc nitrate solution, and the copper(II) ion of the copper(II) nitrate will be converted to metallic copper. Write the unbalanced equation for this process. (Include states-of-matter under the given conditions in the answer)
Calculate the number of grams of HC2H3O2 needed to make 450 mL of 0.322 M solution.
The solubility of nitrogen in water exposed to the atmosphere, where the partial pressure of nitrogen is 593 mm, is 5.3 × 10-4 M. At the same temperature, what would be the solubility of pure nitrogen, at a pressure of 760 mm
What volume will the second student calculate for this bottle. Will this bottle hold the 75 cm^3 of water. However, the second student reports that the same bottle is 3.2 cm in diameter and 10.5 cm tall. To calculate the volume of the bottle, use t..
How does the entropy of the system PbI2(s) + H2O(l) change as PbI2(s) dissolves in water at 25°C?
A sample of gas is stored in 716 mL tank at 205 kPa and 300 K. The gas is transferred to a different tank with a volume of 925 mL and 325 K. What is the pressure of the gas in the second tank?
Carbon dioxide is dissolved in blood to form a mixture of carbonic acid and bicarbonate. Neglecting free CO2 what fraction will be present as carbonic acid?
An industrial vat contains 2,500 liters of an acidic aqueous solution with a pH of 3.5. How many grams of NaOH need to be added to raise the pH to 4.3?
The light sources were controls. How would the experiment be different if you used different light sources? Explain why it was not important to know the exact intensity of either light source.
6.48 g of NaH2PO4 and 21.96 gm of K2HPO4 are dissolved in sufficient water to make a liter of solution. Calculate the pH of the resulting solution.
Calculate the systematic treatment of equilibrium. Remember C2O4^2- is a weak base so you must consider other equilibria. (Ksp(ZnC2O4)=7.5X10^-9, Kb1=1.8X10^-10, Kb2=1.8X10^-13). Solve using systematic treatment of equilibrium.
Will solutions of the following salts be acidic, basic, or neutral? a)K2SO4 b)KNO2 c)CaF2 d)NH4Cl
We titrated a 0.1033 M NaOH solution into an unknown concentration of a weak acid (25.00 mL). It also says the unknown acid will have a concentration of about 0.1 M.
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