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krok68 [10]
3 years ago
7

Can someone please help me

Chemistry
1 answer:
Lilit [14]3 years ago
3 0
It is A. Barium

Explanation: I did that already
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Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid. The acid dissociation constant o
sattari [20]

Answer:

4.26 %

Explanation:

There is some info missing. I think this is the original question.

<em>Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid. The acid dissociation constant of nitrous acid is  4.50  ×  10 ⁻⁴.</em>

<em />

Step 1: Given data

Initial concentration of the acid (Ca): 0.249 M

Acid dissociation constant (Ka): 4.50  ×  10 ⁻⁴

Step 2: Write the ionization reaction for nitrous acid

HNO₂(aq) ⇒ H⁺(aq) + NO₂⁻(aq)

Step 3: Calculate the concentration of nitrite in the equilibrium ([A⁻])

We will use the following expression.

[A^{-} ] = \sqrt{Ca \times Ka } = \sqrt{0.249 \times 4.50 \times 10^{-4}  } = 0.0106 M

Step 4: Calculate the percent ionization of nitrous acid

We will use the following expression.

\alpha = \frac{[A^{-} ]}{[HA]} \times 100\% = \frac{0.0106M}{0.249} \times 100\% = 4.26\%

4 0
3 years ago
You wish to prepare a buffer consisting of acetic acid and sodium acetate with a total acetic acetate plus acetate concentration
vovangra [49]

<u>Ans: Acetic acid = 90.3 mM and Sodium acetate = 160 mM</u>

Given:

Acetic Acid/Sodium Acetate buffer of pH = 5.0

Let HA = acetic acid

A- = sodium acetate

Total concentration [HA] + [A-] = 250 mM ------(1)

pKa(acetic acid) = 4.75

Based on Henderson-Hasselbalch equation

pH = pKa + log[A-]/[HA]

[A-]/[HA] = 10^(pH-pKa) = 10^(5-4.75) = 10^0.25 = 1.77

[A-] = 1.77[HA] -----(2)

From (1) and (2)

[HA] + 1.77[HA] = 250 mM

[HA] = 250/2.77 = 90.25 mM

[A-] = 1.77(90.25) = 159.74 mM



7 0
3 years ago
When precipitation falls in summer, sometimes wind pushes it back up into freezing temperatures before falling again. What will
SVETLANKA909090 [29]

Answer:

A

Explanation:

hail will fall push it back up making it bigger comes back down

3 0
3 years ago
Which of the following will have the slowest rate of diffusion at a given temperature?
marysya [2.9K]
<h3>Answer:</h3>

Chlorine gas (Cl₂)

<h3>Explanation:</h3>
  • According to the Graham's law of diffusion, the diffusion rate of a gas is inversely proportional to the square root of its density or molar mass.
  • Therefore, a lighter gas will diffuse faster at a given temperature compared to a heavy gas.
  • Consequently, the heavier a gas is then the denser it is and the slower it diffuses at a given temperature and vice versa.

In this case we are given gases, CI₂

, H₂,He and Ne.

  • We are required to identify the gas that will diffuse at the slowest rate.
  • In other words we are required to determine the heaviest gas.

Looking at the molar mass of the gases given;

Cl₂- 70.91 g/mol

H₂- 2.02 g/mol

He - 4.00 g/mol

Ne- 20.18 g/mol

Therefore, chlorine gas is the heaviest and thus will diffuse at the slowest rate among the choices given.

8 0
3 years ago
Consider the unbalanced chemical equation HBr + B = BBr3 + H2. When
Vitek1552 [10]

Answer:

B and BBr3

Explanation:

1) 3HBr + B = BBr3 + H2 (double all equation because H2)

2) 6HBr + <em>2B </em>= <em>2BBr3</em> + 3H2

4 0
3 years ago
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