Answer : The given statement is, false.
Explanation :
Ionic product of water : It is defined as the product of the concentration of hydrogen ion and the concentration of hydroxide ion.
The mathematical expression will be,
![[H^+][OH^-]=10^{-14}](https://tex.z-dn.net/?f=%5BH%5E%2B%5D%5BOH%5E-%5D%3D10%5E%7B-14%7D)
When the concentration of hydrogen ion and hydroxide ion are equal then the solution is neutral and the value will be, 
. And the pH of the solution is, 7.
When the concentration of hydrogen ion is greater than then the solution is acidic in nature. And the pH of the solution is, less than 7.
When the concentration of hydrogen ion is less than then the solution is basic in nature. And the pH of the solution is, greater than 7.
Hence, the given statement is false.
Answer: Near the Protons. The electron structure of bromine is illustrated above. In chemical reactions, how does the valence configuration of Bromine tend to change? ... It loses one electron.
Explanation:
btw i found that on google lol
Concentration of the solution (% mass) = 4%
<h3>Further explanation</h3>
<em>Rosa prepared a salt water solution by mixing 120 mg of water with 5 mg of common salt, what concentration is the solution she prepare?</em>
<em />
<em />
<em />
mass solute=mass of salt=5 mg
mass solution :
mass solute(salt)+mass solvent(water) :
Answer: 160 g Fe2O3
Explanation: solution attached.
First convert molecules to moles using Avogadro's number then convert to mass using the relationship between moles and molar mass of Fe2O3
The answer is <span>the
reaction will shift to the left (toward the reactants).
Reaction is at equilibrium can be expressed as,
Reactants </span>⇄ products<span>
<span>After coming to the equilibrium, if one condition
is changed, then according to the </span>Le chatelier's Principal,<span> the system
will act to maintain the equilibrium by reducing the effect. As an example, if
we reduce the pressure, then system acts to increase the pressure to maintain
the equilibrium.</span>
<span>Likewise, if we add products into the reaction
which is in equilibrium, the system acts to reduce the effect by promoting the backward
reaction to produce reactants.</span></span>
