Answer:
See Explanation
Explanation:
Resonance is a valence bond terminology which is used to describe a situation in which a single structure is not able to fully describe the nature of bonding in a molecule.
In such cases, we invoke more than one structure. Each structure contributes significantly to our understanding of the nature of bonding in the molecule under consideration and these structures are called canonical or resonance structures.
The real structure of the molecule is somewhere in between these structures - a resonance hybrid.
For ozone, two equivalent structures can be used to describe the bonding in the molecule. These structures are equivalent as shown in the mage attached. We can see from these structures that the bond order in ozone is 1.5(one and half bonds)
1) Molarity
M = n / V
n: number of moles of solute
V: volume of the solution in liters
n = mass / molar mass = 0.000333 g / 332.32 g / mol = 1*10 ^ - 6 moles
V = 225 ml * 1 liter / 1000 ml = 0.225 liter
M = 10^-6 mol / 0.225 liter = 0.00000444 M
2) ppm
ppm = parts per million
grams of solute: 0.000333 g
grams of solution = volume * density = 225 ml * 0.785 g / ml = 176.625 g
ppm = [0.00033 g / 176.625 g] * 1,000,000 = 1.868 ppm
For the first one, compound might mean more than one thing or i team. But mixture is a very specific definition for chemistry. And for the second one, it would be wrong because “pure” means only that substance, where as it would only be “orange juice”, or something else. But pure refers to only a clean not contaminated substance.
Answer:
The steps are explained below, the essential step is to find mass here, 120 g of NaOH.
Explanation:
In order to answer this question, we need to define molarity conceptually firstly to see what variables we need. According to the formula, molarity is equal to the ratio between moles and volume, while moles itself is a ratio between mass and molar mass. This means we have a formula for molarity involving mass, molar mass and volume:
In order to prepare a 500.0 mL of stock solution of 6.0 M of NaOH, we then need to find the mass of NaOH dissolved in this solution using the equation above:
Now, since we have the mass of NaOH, we can describe the steps needed to prepare this solution:
- measure 120 grams of solid NaOH;
- add this mass of NaOH into a 500.0-mL Erlenmeyer flask;
- fill approximately half of the flask with distilled water and stir gently to make sure that NaOH dissolves, if it doesn't, add more water and repeat the process;
- when NaOH fully dissolves, fill the flask to the mark.
Our solution is prepared.
