A 10.14 g 10.14 g sample of a weak acid (HA) is dissolved in 511.0 g 511.0 g of water. The freezing point of the solution is − 0.368 °C −0.368 °C . The molar mass of the weak acid is 93.0 g/mol. 93.0 g/mol. Calculate the acid dissociation constant, K a Ka , of the weak acid.
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Chemistry, 21.06.2019 16:30
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Chemistry, 22.06.2019 00:50
If a reactant was removed, did the new equilibrium system shift to make more reactants or more products?
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Chemistry, 22.06.2019 07:20
Describing intermolecular forces use the drop down menus to match the type of intermolecular force to its name dipole dipole interactions dipole induced dipole interactions london dispersion forces hydrogen bond van der waals forces done
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Chemistry, 22.06.2019 11:40
Modern pennies are composed of zinc coated with copper. a student determines the mass of a penny to be 2.482 g and then makes several scratches in the copper coaling (to expose the underlying zinc). the student puts the scratched penny in hydrochloric acid, where the following reaction occurs between the zinc and the hcl (the copper remains undissolved): zn(s) + 2 hcl(aq) → h2(g) + zncl(aq)the student collects the hydrogen produced over water at 25 °c. the collected gas occupies a volume of 0.899 l at a total pressure of 79 j mmhg. calculate the percent zinc (by mass) in the penny. (assume that all the zn in the penny dissolves.)
Answers: 1
A 10.14 g 10.14 g sample of a weak acid (HA) is dissolved in 511.0 g 511.0 g of water. The freezing...
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