Answer:
We have to weigh 52.8 g of BaCl₂·2H₂O, add it to a 2.00 L flask and add water until reaching the final volume.
Explanation:
<em>Describe the preparation of 2.00 L of 0.108 M BaCl₂ from BaCl₂·2H₂O. (244.3 g/mol).</em>
Step 1: Calculate the moles of BaCl₂
We need to prepare 2.00 L of a solution that contains 0.108 moles of BaCl₂ per liter of solution.
2.00 L × 0.108 mol/L = 0.216 mol
Step 2: Calculate the moles of BaCl₂·2H₂O that contain 0.216 moles of BaCl₂
The molar ratio of BaCl₂·2H₂O to BaCl₂ is 1:1. The moles of BaCl₂·2H₂O required are 1/1 × 0.216 mol = 0.216 mol.
Step 3: Calculate the mass corresponding to 0.216 mol of BaCl₂·2H₂O
The molar mass of BaCl₂·2H₂O is 244.3 g/mol.
0.216 mol × 244.3 g/mol = 52.8 g
We have to weigh 52.8 g of BaCl₂·2H₂O, add it to a 2.00 L flask and add water until reaching the final volume.
. Consider a sample of oxygen gas at 27° C with a volume of 9.55L at a pressure
Nitrogen? calcium reacts with nitride which is water acids and metals burning in the air
<h3><u>Answer;</u></h3>
a. CH3CO2H
<h3><u>Explanation;</u></h3>
- An Arrhenius acid is a substance that dissociates in water to form hydrogen ions or protons. In other words an Arrhenius acid increases the concentration of H+ in aqueous solution.
- Acetic acid (CH3CO2) dissociates in aqueous solution to form hydrogen ions (H⁺) and acetic anion (CH₃COO⁻). Therefore, it is an Arrhenius acid.
- The equation of dissociation;
CH₃COOH(aq) ⇄ CH₃COO⁻(aq) + H⁺(aq).
