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What is the pH at the equivalence point when 40.00 mL 0.100 propionic acid, CH3CH2COOH, Ka = 1.3 x 10-5, is titrated with 0.1000 M NaOH?
One beaker contains 10.0 mL of acetic acid/sodium acetate buffer at maximum buffer capacity (equal concentrations of acetic acid and sodium acetate), and another contains 10.0 mL of pure water.
A particular first-order reaction has a rate constant of 1.35 × 102 s-1 at 25°C. What is the magnitude of k at 75°C if Ea=85.6 kJ/mol
that the reaction was endothermic. If the enthalpy of reaction is negative, then we say that energy was released or that the reaction was exothermic. Most chemical reactions are exothermic.
Consider the mechanism of reduction of WO3. At least two mechamisms are possible to the formation of HxWO3 during intercalation of WO3
how much energy is released when 89 grams of water vapor (steam) is cooled from 503 K to 354 K?
What is the final temperature of the sand A 1.00 kg gold bar at 1010 K is dropped into 0.750 kg of sand at twenty five degree Celsius?
CaCN2 + 3 H2O → CaCO3 + 2 NH3 . How much CaCO3 is produced if 47.5 moles NH3 are produced?
Determine What is the final concentration and calculate what is the Ksp of this salt at temperature of 25 degrees Celsius?
Calculate the mass of ice at -15°C that must be added to cool the water to 10°C after thermal equilibrium is achieved. To find the mass of water use the density of water = 1.0 g/mL.
Calculate the molality, molarity and mol fraction of a 25.4% (by mass) aqueous solution of phosphoric acid (H3PO4). in one litre of solution.
If iron is oxidized to Fe2+ by a copper(II) sulfate solution, and 0.704 grams of iron and 12.6 mL of 0.581M copper(II) sulfate react to form as much product as possible,
a typical aspirin tablet contains 324 mg of aspirin (acetylsalicylic acid, C9H8O4, Ka = 3.0×10-4). Imagine you dissolve two aspirin tablets in a 275 mL glass of water. Calculate the solution's pH.
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