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.
Answers: 3
Chemistry, 22.06.2019 02:50, Jerrikasmith28
The conventional equilibrium constant expression (kc) for the system below is: 2icl(s) ⇄ i2(s) + cl2(g) [cl2] ([i2] + [cl2])/2[icl] [i2][cl2]/[icl]2 none of the listed answers are correct [i2][cl2]/2[icl]
Answers: 2
Chemistry, 22.06.2019 12:00, daytonalive83481
Ican determine the molar mass of an element by looking on the under the atomic mass for the element. for example the molar mass of phosphorus is 30.974 grams/mole. avogadro’s number tells me the amount of representative particles in 1 mole of any substance. this means 12.011 gram sample of carbon and a 32.0 gram sample of sulfur have the same number of atoms.
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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