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3 years ago

Explain the application of silver halides in darkening effect in industry

Chemistry

1 answer:

ioda3 years ago

4 0

Explanation:

Silver halides are ionic crystals consisting of a regular cubic lattice of Ag and halide ions together with a small proportion of defects, such as Ag ions that have been displaced from their regular lattice position to another “interstitial” position (the Ag ions are much smaller than the halide ions), and the corresponding vacancy in the lattice.

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Will a precipitate (ppt) form when 20.0 mL of 1.1 × 10 –3 M Ba(NO 3) 2 are added to 80.0 mL of 8.4 × 10 –4 M Na 2CO 3?

erastova [34]

Answer:

A precipitate will form, BaCO₃

Explanation:

When Ba²⁺ and CO₃²⁻ ions are in an aqueous media, BaCO₃(s), a precipitate, is produced following its Ksp expression:

Ksp = 5.1x10⁻⁹ = [Ba²⁺] [CO₃²⁻]

Where the concentrations of the ions are the concentrations in equilibrium

For actual concentrations of a solution, you can define Q, reaction quotient, as:

Q = [Ba²⁺] [CO₃²⁻]

If Q > Ksp, the ions will react producing BaCO₃, if not, no precipitate will form.

Actual concentrations of Ba²⁺ and CO₃²⁻ are:

[Ba²⁺] = [Ba(NO₃)₂] = 1.1x10⁻³ × (20.0mL / 100.0mL) = 2.2x10⁻⁴M

[CO₃²⁻] = [Na₂CO₃] = 8.4x10⁻⁴ × (80.0mL / 100.0mL) = 6.72x10⁻⁴M

100.0mL is the volume of the mixture of the solutions

Replacing in Q expression:

Q = [Ba²⁺] [CO₃²⁻]

Q = [2.2x10⁻⁴M] [6.72x10⁻⁴M]

Q = 1.5x10⁻⁷

As Q > Ksp

<h3>A precipitate will form, BaCO₃</h3>

8 0

3 years ago

Calculate the number of atoms contained in 5000cm^3 of carbon dioxide gas at room condition

noname [10]

Answer:

$\huge\boxed{\sf No.\ of\ atoms = 1.4 * 10^{20} \ atoms}$

Explanation:

Given Data:

Volume = v = 5000 cm³ = 0.005 m³

Density of CO₂ at RTP = 1.98 kg / m³

Molar Mass = M = 12 + 16 * 2 = 44 g / mol

Avogadro's No. = $\sf N_{A}$ = 6.023 * 10²³ mol⁻¹

Required:

Number of atoms = ?

Solution:

We know that:

No. of moles (n) = mass in grams / molar mass ∴ Mass = Density * Volume

n = D * v / M

n = 1.98*0.005 / 44

n = 0.000225

Now, Finding the number of atoms

No. of atoms = No. of moles * Avogadro's Number

No. of atoms = 0.000225 * 6.023 * 10²³

No. of atoms = 0.0014 * 10²³

No. of atoms = 1.4 * 10²⁰ atoms

$\rule[225]{225}{2}$

Hope this helped!

4 0

3 years ago