Colume of acid required to completely neutralize the base
Question: If 1.4 M H2SO4 is used to titrate a 300.0 mL solution of 1.76 M ammonia (NH3), what volume of acid is required to completely neutralize the base? Each mole of this strong diprotic acid produces two moles of hydronium ions in water.
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A compound having an approximate molar mass of 120-15 g has the following percent composition by mass: carbon, 38.44%; hydrogen, 4.839%; chlorine, 56.73%. Determine the empirical and molecular formulas of the compound.
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If 1.4 M H2SO4 is used to titrate a 300.0 mL solution of 1.76 M ammonia (NH3), what volume of acid is required to completely neutralize the base? Each mole of this strong diprotic acid produces two moles of hydronium ions in water.
Calculate the concentration of a solution prepared by adding enough water to 2.2 g of sucrose (C12H22O11) to make a total of 50 mL of solution.
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If Delta H = -80.0 kJ and Delta S = -0.300 kJ/K, the reaction is spontaneous below a certain temperature. Calculate that temperature.
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