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3 years ago

Given the following equation: Na2O + H2O ---> 2 NaOH

Chemistry

1 answer:

andreyandreev [35.5K]3 years ago

7 0

Answer:

2.04 moles

Explanation:

Since the ratio of Na2O to NaOH is 1:2, you multiply the number of moles by 2, equaling 2.04 moles.

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From the Henderson-Hasselbalch equation, explain how the ratio [Al/[HA] changes with changing pH

Kryger [21]

Answer:

The ratio [A-]/[HA] increase when the pH increase and the ratio decrease when the pH decrease.

Explanation:

Every weak acid or base is at equilibrium with its conjugate base or acid respectively when it is dissolved in water.

$HA + H_{2}O$ ⇄ $A^{-} + H_{3}O^{+}$

This equilibrium depends on the molecule and it acidic constant (Ka). The Henderson-Hasselbalch equation,

$pH = pKa + Log \frac{[A^{-}]}{[HA]}$

shows the dependency between the pH of the solution, the pKa and the concentration of the species. If the pH decreases the concentration of protons will increase and the ratio between A- and AH will decrease. Instead, if the pH increases the concentration of protons will decreases and the ratio between A- and AH will increase.

5 0

3 years ago

What is electroluminescence? Give one example.

vredina [299]

Answer:

electroluminescence is a production of light by the flow of electrons, as within certain crystals. An example is at most resataurants with a bright sign that either says open or closed.

Explanation:

5 0

3 years ago

2. (2 pts) How would you prepare 1.5 liters of 2 M KCI (MW=74.55 g/mol)

ra1l [238]

Answer:

Dissolve 226 g of KCl in enough water to make 1.5 L of solution

Explanation:

1. Calculate the moles of KCl needed

$n = \text{1.5 L} \times \dfrac{\text{2 mol}}{\text{1 L}}= \text{3.0 mol}$

2. Calculate the mass of KCl

$m = \text{3.0 mol} \times \dfrac{\text{74.55 g}}{\text{1 mol}}= \text{224 g}$

3. Prepare the solution

Measure out 224 g of KCl.
Dissolve the KCl in a few hundred millilitres of distilled water.
Add enough water to make 1.5 L of solution. Mix thoroughly to get a uniform solution.

8 0

3 years ago

How might the yield of 1-bromobutane be affected if water was not added, and what product(s) would be favored?

jek_recluse [69]

Due to the inability of the reaction to take place, the yield of 1-Bromobutane would drop.

Since 1-Butanol won't react with the additional sodium bromide, bromination won't happen.

If water had been supplied, the equilibrium would have shifted extremely far to the left, preventing the reactants from interacting with the acid and favoring the yield of 1-bromobutane instead.

<h3>What is Bromination?</h3>

When a substance undergoes bromination, bromine is added to the compound as a result of the chemical reaction.

After bromination, the result will have different properties from the initial reactant.
For example, an alkene is brominated by electrophilic addition of $Br_{2}$ .
Benzene ring bromination by electrophilic aromatic substitution.