Hydrogen ion, strictly, the nucleus of a hydrogen atom separated from its accompanying electron. The hydrogen nucleus is made up of a particle carrying a unit positive electric charge, called a proton. The isolated hydrogen ion, represented by the symbol H+, is therefore customarily used to represent a proton.
The molecular weight of LiOH would be 23.95 g/mol, so the amount of LiOH in mol would be: 1.64g/(<span>23.95 g/mol)= 0.069 mol
The reaction of LiOH with HCl would be:
</span><span>HCl + LiOH = H2O + LiCl
The coefficient of LiOH:HCL is 1:1 so you need the same amount of HCl to neutralize LiOH.
HCl= LiOH
volume* 0.15M= </span>0.069 mol
volume= 0.069 mol/ (0.15 mol/ 1000ml)
volume= 459.29 ml
Answer:
Chemistry is another word for science just higher level.the branch of science that deals with the identification of the substances of which matter is composed; the investigation of their properties and the ways in which they interact, combine, and change; and the use of these processes to form new substances.
Explanation:
<u>Answer:</u> The expression for equilibrium constant in terms of concentration is ![K_c=[CO_2]](https://tex.z-dn.net/?f=K_c%3D%5BCO_2%5D)
<u>Explanation:</u>
Equilibrium constant in terms of concentration is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric coefficients. It is represented by 
For a general chemical reaction:
The is written as:
![K_{c}=\frac{[C]^c[D]^d}{[A]^a[B]^b}](https://tex.z-dn.net/?f=K_%7Bc%7D%3D%5Cfrac%7B%5BC%5D%5Ec%5BD%5D%5Ed%7D%7B%5BA%5D%5Ea%5BB%5D%5Eb%7D)
The concentration of pure solids and pure liquids are taken as 1.
For the given chemical reaction:
The expression for is:
![K_{c}=\frac{[MgO][CO_2]}{[MgCO_3]}](https://tex.z-dn.net/?f=K_%7Bc%7D%3D%5Cfrac%7B%5BMgO%5D%5BCO_2%5D%7D%7B%5BMgCO_3%5D%7D)
In the above expression, magnesium oxide and magnesium carbonate will not appear because they are present in solid state.
So, the expression for 
becomes:
![K_{c}=[CO_2]](https://tex.z-dn.net/?f=K_%7Bc%7D%3D%5BCO_2%5D)
Hence, the equilibrium constant for the reaction is given above.
Answer:
3.0x10⁻²M
Explanation:
Silver sulfate, Ag₂SO₄, has a product constant solubility equilbrium of:
Ag₂SO₄(s) ⇄ 2Ag⁺ + SO₄²⁻
When an excess of silver sulfate is added, some Ag₂SO₄ will react producing Ag⁺ and SO₄²⁻ until reach the equilbrium determined for the formula:
ksp = 1.4x10⁻⁵ = [Ag⁺]² [SO₄²⁻]
Assuming the Ag₂SO₄ that react until reach equilibrium is X, we can replace in Ksp expression:
1.4x10⁻⁵ = [Ag⁺]² [SO₄²⁻]
1.4x10⁻⁵ = [2X]² [X]
1.4x10⁻⁵ = 4X³
3.5x10⁻⁶ = X³
0.015 = X
As [Ag⁺] is 2X:
[Ag⁺] = 0.030 = 3.0x10⁻²M
The answer is:
<h3>3.0x10⁻²M</h3>
