Answer:
Empirical formula for the oxide is P₂O₃
Explanation:
Oxides from P, are:
P₂O; P₂O₃; P₂O₅; P₂O₇; P₄O₆; P₄O₁₀
The reaction is:
P₄ + 3O₂ → P₄O₆
Ratio between the white phosphorus and the oxide is 1:1
Molar mass P₄ = 123.89 g/m
Mass / Molar mass = mole
6.5 g/ 123.89 g/m = 0.0524 mole P₄
0.0524 mole of P₄O₆ have been formed.
Molar mass P₄O₆ = 219.89 g/m
Mol . molar mass = mass
0.0524 mole . 219.89 g/m = 11.52 g
I think it might be Core Electrons and Valence Electrons respectively. As core electrons are the name of the electrons for the inner levels. While valence is the outer shell electrons.
<span>the ionization constant, Ka, for and indicator, HIn, is 1.0x10^-8. The color of the unionized form is red and the color of the ionized form is yellow. What is the color of the indicator in a solution whose pH is 4.6? (Hint: the color of an indicator can be estimated by considering the ratio of [HIn]/[In]. If the ratio is equal to or greater than 10, the color will bet hat of the unionized form. If the ratio is equal to or smaller than 0.1, the color will be that of the ionized form.
</span><span>Ka=[H+][A-]/[HA]
substitute for pH and find the value of A-/HA.
</span><span>
</span><span>so it'd just be 1x10^-8 divided by 4.6</span>