Answer: 1. The solvent in a mixture of gases is generally considered to be the substance in greater amount. 2. The solid dissolved in a solution is known as the solute. 3. Solid solutions are called alloys.
Explanation:
A binary solution is made up of two components ,called as solute and another as solvent.
A solute is defined as the component which is present in smaller proportion. It can be in solid, liquid or gaseous phase. A solvent is defined as the component which is present in larger proportion in a solution. It can be in solid, liquid or gaseous phase.
Usually in liquid solutions , solid acts as solute and liquid acts as solvent. For example: In salt solution, salt is the solute and water is the solvent.
Solid solutions contains solid as solute and solid as solvent. These are called as alloys. For example : In brass, zinc is the solute and copper is the solvent.
Let's use Boyle's Law here. P1*V1 = P2*V2
Given: (assuming that there are decimals at the end for Sig Figs)
P1 = 900.mmHg
P2 = 1140.mmHg
V1 = ???
V2 = 250.mL
900.mmHg* ??? = 1140.mmHg * 250.mL
??? = 1.27*250.mL
??? = 318.mL
Therefore, the original volume is 318mL.
Balanced chemical reaction (dissociation) : CaCl₂(aq) → Ca²⁺(aq) + 2Cl⁻(aq).
n(CaCl₂) = 3,5 mol.
From chemical reaction: n(CaCl₂) : n(Ca²⁺) = 1 : 1.
n(Ca²⁺) = 3,5 mol.
From chemical reaction: n(CaCl₂) : n(Cl⁻) = 1 : 2.
n(Cl⁻) = 2 · 3,5 mol.
n(Cl⁻) = 7 mol.
Calcium chloride is salt that completely dissociate in water on calcium cations and chlorine anions.
Answer: Homogeneous mixture
Explanation:
Homogeneous mixtures are those mixtures in which the dispersed phase is uniformly distributed throughout the dispersion medium. The dispersed phase has uniform composition throughout the dispersion medium and thus there is no physical boundary between the dispersed phase and the dispersion medium. Example: salt in water
Heterogeneous mixtures are those mixtures in which the dispersed phase is not uniformly distributed throughout the dispersion medium. The dispersed phase does not has uniform composition throughout the dispersion medium and thus there is a distinct physical boundary between the dispersed phase and the dispersion medium. Example: Sand in water
