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3 years ago

_____ occurs when the product of the ion concentrations exceeds the Ksp.

Chemistry

2 answers:

arlik [135]3 years ago

4 0

Precipitation occurs when the product of the ion concentration exceeds the Ksp.

serious [3.7K]3 years ago

4 0

Answer : Precipitation occurs when the product of the ion concentrations exceeds the $K__{sp}$ .

Explanation :

Ionic product : It is the product of the concentrations of the ions in solution raised to the same power by its stoichiometric coefficient in a solution of a salt. This takes place at any concentration. The ionic product is represented as, Q.

Solubility product constant : It is defined as the product of the concentration of the ions present in a solution raised to the power by its stoichiometric coefficient in a solution of a salt. This takes place at equilibrium only. The solubility product constant is represented as, $K__{sp}$ .

There are three cases for the solubility :

When $Q$ this means that the solution is unsaturated solution and more solid will be dissolve.
When $Q=k_{sp}$ this means that the solution is saturated solution.
When $Q>k_{sp}$ this means that the solution is supersaturated solution and solid will be precipitate.

Hence, the precipitation occurs when the product of the ion concentrations exceeds the $K__{sp}$ .

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Strontium (Sr) has the FCC crystal structure, an atomic radius of 0.215 nm, and an atomic weight of 87.62 g/mol. What is its the

Valentin [98]

Answer:Theoretical density =2.576g/cm³

Explanation:

Theoretical density p= (A×n)/Vc ×Av

A= molecular weight

n= effective number of atoms per unit cell

Vc=Volume of unit cell = a³

Av = Avogadro's constant = 6.02×10²³

Given that A= 87.2g/mol

n= 4 (For FCC crystal structure)

Vc= a³

Where a = 2R√2 and R is the atomic radius

R=0.215

a= 2 × 0.215×√2

a= 0.608nm = 0.608×10^-7 cm

Vc= (0.608×10^-7 cm)³

Vc=2.25×10^-22 cm³

P= (87.2 × 4)/

(2.25×10^-22) × (6.02×10²³)

P= 2.576g/cm³

Therefore the theoretical density of strontium is 2.576g/cm³

3 0

3 years ago

Aqueous solutions of silver nitrate (agno3) and iron(iii) chloride (fecl3) are mixed together. which ion combines with the chlor

Anna [14]

The answer is that "Ag+ ion combines with the chloride ion to form a precipitate".

Silver chloride is formed in the form of precipitates, Ag⁺ is a cation and Cl⁻ is an anion so both ions attract each other and combines to form AgCl.

The equation for the ionic reaction that occurs is;

Ag⁺(aq)+Cl⁻(aq)→AgCl(s)

7 0

3 years ago

9. Calculate the approximate number of atoms in a bacterium. Assume the average mass of an atom in the bacterium is 10 times the

Natali5045456 [20]

The question is incomplete, the complete question is :

Calculate the approximate number of atoms in a bacterium. Assume the average mass of an atom in the bacterium is 10 times the mass of a hydrogen atom.(Hint the mass of hydrogen atom is on order of $10^{-27}$ kg and the mass of bacterium is on order of $10^{-15}$ kg

Answer:

The total numbers of atom in bacterium are $10^{12}$ .

Explanation:

Mass of hydrogen atom, m= $10^{-27}$ kg

Mass of bacterium , M= $10^{-15}$ kg

Mass of bacterium atom =m'

Given ; $m' =10\times m$

$m'=10\times 10^{-27} kg=10^{-26} kg$

let the number of atoms in bacterium be N

$m'\times N=M$

$N=\frac{M}{m'}=\frac{10^{-15} kg}{10^{-27} kg}=10^{12}$

The total numbers of atom in bacterium are $10^{12}$ .

5 0

3 years ago

This is the chemical formula for acetone: CH32CO. Calculate the mass percent of carbon in acetone.

olga_2 [115]

Answer:

62.07 %

Explanation:

Chemical Formula = (CH3)2CO = C3H6O

Mass of C = 12 g/mol

Mass of H = 1 g/mol

Mass of O = 12 g/mol

Mass of C3H6O = 3(12) + 6(1) + 16 = 58 g/mol

Total mass of C in Acetone = 12 * 3 = 36 g

Mass Percent of C = Total mass of C / Mass of Acetone * 100

Mass percent = 36 / 58 * 100

Mass percent = 62.07 %

6 0

3 years ago

What mass of silver chloride (m = 143.4) will dissolve in 1.00 l of water? the ksp of agcl is 1.8 × 10–10 ?

trapecia [35]

Given that solubility product of AgCl = 1.8 X 10^-10

Dissociation of AgCl can be represented as follows,

AgCl(s) ↔ Ag+(ag) + Cl-(aq)

Let, [Ag+] = [Cl-] = S

∴Ksp = [Ag+][Cl-] = S^2

∴ S = √Ksp = √(1.8 X 10^-10) = 1.34 x 10^-5 mol/dm3

Now, Molarity of solution = $\frac{\text{weight of solute}}{\text{Molecular weight X volume of solution (l)}}$
∴ 1.34 x 10^-5 = $\frac{\text{weight of AgCl}}{143.4 X 1}$
∴ Weight of AgCl present in solution = 1.92 X 10^-3 g

Thus, mass of AgCl that will dissolve in 1l water = 1.92 x 10^-3 g

7 0

3 years ago