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Damm [24]
3 years ago
9

What is the total concentration of ions in a 0.10 M solution of barium chloride?

Chemistry
2 answers:
Murljashka [212]3 years ago
4 0
It is 0.30 because BaCl2 breaks into Ba+2 + 2Cl-... each on has 0.10 M so (0.10) + 2(0.10)= 0.30M
alexgriva [62]3 years ago
4 0

Answer:

0.30 M is the total concentration of ions in a 0.10 M solution of barium chloride.

Explanation:

Concentration of  solution of barium chloride = 0.10 M = 0.10 mol/L

BaCl_2(aq)\rightarrow Ba^{2+}(aq)+2Cl^-(aq)

1 Mole of barium chloride gives 1 mole of barium ions and 2 moles of chloride ions.

Concentration of barium ions in solution = [x]

[x]=1\times 0.10 mol/L=0.10 mol/L

Concentration of chloride ions in solution = [y]

[y]=2\times 0.10 mol/L=0.20 mol/L

Total concentration of ions in the solution : [x]+[y]

0.10 mol/L + 0.20 mol/L = 0.30 mol/L

0.30 M is the total concentration of ions in a 0.10 M solution of barium chloride.

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Problem PageQuestion The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of sodium
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Answer:

1. 2NaN₃(s) → 2Na(s) + 3N₂(g)

2. 14.5 g NaN₃

Explanation:

The answer is incomplete, as it is missing the required values to solve the problem. An internet search shows me these values for this question. Keep in mind that if your values are different your result will be different as well, but the solving methodology won't change.

" The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of sodium azide, which produces large volumes of nitrogen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid sodium azide (NaN₃) into solid sodium and gaseous dinitrogen. 2. Suppose 71.0 L of dinitrogen gas are produced by this reaction, at a temperature of 16.0 °C and pressure of exactly 1 atm. Calculate the mass of sodium azide that must have reacted. Round your answer to 3 significant digits. "

1. The <u>reaction that takes place is</u>:

  • 2NaN₃(s) → 2Na(s) + 3N₂(g)

2. We use PV=nRT to <u>calculate the moles of N₂ that were produced</u>.

P = 1 atm

V = 71.0 L

n = ?

T = 16.0 °C ⇒ 16.0 + 273.16 = 289.16 K

  • 1 atm * 71.0 L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 289.16 K
  • n = 0.334 mol

Now we <u>convert N₂ moles to NaN₃ moles</u>:

  • 0.334 mol N₂ * \frac{2molNaN_{3}}{3molN_2} = 0.223 mol NaN₃

Finally we <u>convert NaN₃ moles to grams</u>, using its molar mass:

  • 0.223 mol NaN₃ * 65 g/mol = 14.5 g NaN₃

6 0
3 years ago
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