Answer:
24.9mL of the stock solution are required
Explanation:
To solve this question we have to find, as first, the moles of HCl that we need to prepare the desire solution. These moles are taken from the stock solution as follows:
<em>Moles diluted solution:</em>
500.0mL = 0.5000L * (0.613mol / L) = 0.3065 moles HCl
As these moles comes from the 12.3M HCl solution, the volume that we need of the stock solution is:
<em>Volume stock solution:</em>
0.3065 moles HCl * (1L / 12.3moles) = 0.0249L 12.3M HCl =
<h3>24.9mL of the stock solution are required</h3>
1L ------------ 1 kg
? ------------- 3.8 kg
3.8 x 1 / 1
= 3.8 L
Answer:
B. The student conducted the reaction in an open beaker, which allowed one of the products, a gas, to escape.
Explanation:
Based on the law of conservation of mass, matter is neither created nor destroyed during the course of a chemical reaction.
By this premise, the mass of reactants and products must remain the same during the course of a reaction.
- Here we find that this is not the case.
- The mass of the product reported is less than the mass of the reactants.
- The problem is that the mass of the gas bubbles produced during the course of this reaction was not accounted for.
- This leaves a mass deficit already
Answer:
It is considered an ionic compound since it is composed of the magnesium cation (Mg2+) and two hydroxide anions (OH-). There are no covalently shared electrons here. ... The reaction of the hydroxide anions with acid causes more of the magnesium hydroxide to dissolve until all of the acid has been neutralized.