Answer:Therefore, HCl is 2.765 % Hydrogen and 97.235 % Chlorine by mass.
Answer:
The answer is
<h2>1.74 g/mL</h2>
Explanation:
The density of a substance can be found by using the formula
From the question
mass of magnesium = 11.81 g
volume = 6.80 mL
The density of the metal is
We have the final answer as
<h3>1.74 g/mL</h3>
Hope this helps you
Answer:
Ok; first of all, you must correct the Molecular Formula; FeSO4•7H20
So, work out the Molar Mass;,
(4x18)O+ 55.? Iron + 32 Sulphur, PLUS
(7x 18) H2O = 1 molar mass.
Now, take that times 5.24, show your work & check the Mol. Weights, I am going by memory.
Oxygen
Explanation:
Answer:
The order of solubility is AgBr < Ag₂CO₃ < AgCl
Explanation:
The solubility constant give us the molar solubilty of ionic compounds. In general for a compound AB the ksp will be given by:
Ksp = (A) (B) where A and B are the molar solubilities = s² (for compounds with 1:1 ratio).
It follows then that the higher the value of Ksp the greater solubilty of the compound if we are comparing compounds with the same ionic ratios:
Comparing AgBr: Ksp = 5.4 x 10⁻¹³ with AgCl: Ksp = 1.8 x 10⁻¹⁰, AgCl will be more soluble.
Comparing Ag2CO3: Ksp = 8.0 x 10⁻¹² with AgCl Ksp = AgCl: Ksp = 1.8 x 10⁻¹⁰ we have the complication of the ratio of ions 2:1 in Ag2CO3, so the answer is not obvious. But since we know that
Ag2CO3 ⇄ 2 Ag⁺ + CO₃²₋
Ksp Ag2CO3 = 2s x s = 2 s² = 8.0 x 10-12
s = 4 x 10⁻12 ∴ s= 2 x 10⁻⁶
And for AgCl
AgCl ⇄ Ag⁺ + Cl⁻
Ksp = s² = 1.8 x 10⁻¹⁰ ∴ s = √ 1.8 x 10⁻¹⁰ = 1.3 x 10⁻⁵
Therefore, AgCl is more soluble than Ag₂CO₃
The order of solubility is AgBr < Ag₂CO₃ < AgCl