Answer:
The effect is the increasing of the molar concentration.
Explanation:
When you standarize a solution of NaOH with KHP you are establish its molar concentration (That is the amount of moles of NaOH per liter of solution).
If you evaporated some water of the solution, you are increasing its concentration because volume is decreasing doing the amount of moles per liter increasing.
Description in biology, cell theory is the historic scientific theory, now universally accepted, that living organisms are made up of cells, that they are the basic structural/organizational unit of all organisms, and that all cells come from pre-existing cells.
Answer:
Xenon
Explanation:
The core electrons of an element are the electrons that do not take part in the chemical reactions of the element
The electronic configuration of barium Ba is presented as follows;
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s²
2+2+6+2+6+2+10+6+2+10+6
The valence electrons of boron are the 6s² electrons
The core electrons of boron are the; 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶
The electronic configuration of xenon, Xe, which is the previous noble element before barium, is presented as follows;
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ which is the same as the core electrons of barium
Therefore, the total number of electrons in xenon is equal to the number of core electrons in barium
Answer:C
Explanation: Because the hot air is less dense than the surrounding air
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Aluminium oxide is amphoteric. It is easy to see that it is a Bronsted-Lowry base through the following reaction:
Al2O3+6HCl →2AlCl3+3H2O
AlX2OX3+6HCl →2AlClX3+3HX2O
The Alumnium oxide splits and the oxygen accepts a proton, forming water.
But what about the reaction with a base? In my textbook, they say:
Al2O3+NaOH →2NaAlO2+H2O
AlX2OX3+NaOH →2NaAlOX2+HX2O
Now, the textbook claims that Aluminium oxide is an acid merely because it reacts with a base to form a salt and water, as is characteristic of a neutralization reaction.
But I'm not satisfied with this definition. I mean, acids aren't defined as 'things that neutralize bases', we have well-established definitions for them.
I tried to figure out for myself how this could be. Clearly, the Bronsted-Lowry theory cannot be applied here since the compound in question has no protons to donate. Therefore, the only alternative is the Lewis concept. I cannot see how that is applicable in this case.
The most basic definition of "acid" is that it is a proton donor (or one which accepts a lone pair)
All of this stuff is done in an aqueous medium, so we can assume that all aqueous ions and molecules are present. With this assumption (in this case, we are assuming that OH−OHX− is available to react), we get the following equation:
Al2O3+OH−⟶2AlO2−+H+
AlX2OX3+OHX−⟶2AlOX2X−+HX+
Similarly, we get:
Al2O3+6H+⟶2Al3++H2O
AlX2OX3+6HX+⟶2AlX3++HX2O
where it is acting like a proton acceptor (base).