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elena-14-01-66 [18.8K]
3 years ago
9

Given the atomic mass of select elements, calculate the molar mass of each salt.

Chemistry
1 answer:
arlik [135]3 years ago
3 0

Answer:

See explanation

Explanation:

Molar mass is obtained as the sum of relative atomic masses as follow;

For CaBr = 40.08 + 79.90 = 119.98 g/mol

For BeBr =  9.012 + 79.90 = 88.912 g/mol

For CdBr2 = 112.41 + 2(79.90) = 272.21 g/mol

For CuBr2 = 63.55 + 2(79.90) = 223.35 g/mol

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If PbI2(s) is dissolved in 1.0MNaI(aq) , is the maximum possible concentration of Pb2+(aq) in the solution greater than, less th
fredd [130]

Answer:

\mathbf{s =\sqrt [3]{\dfrac{K_{sp}}{4}}}

Less than the concentration of Pb2+(aq) in the solution in part ( a )

Explanation:

From the question:

A)

We assume that s to be  the solubility of PbI₂.

The equation of the reaction is given as :

PbI₂(s) ⇌ Pb²⁺(aq) + 2I⁻(aq); Ksp = 7 × 10⁻⁹

 [Pb²⁺] =   s

Then [I⁻] = 2s

K_{sp} =\text{[Pb$^{2+}$][I$^{-}$]}^{2} = s\times (2s)^{2} =  4s^{3}\\s^{3} = \dfrac{K_{sp}}{4}\\\\s =\mathbf{ \sqrt [3]{\dfrac{K_{sp}}{4}}}\\\\\text{The mathematical expressionthat can be used to determine the value of  }\mathbf{s =\sqrt [3]{\dfrac{K_{sp}}{4}}}

B)

The Concentration of Pb²⁺  in water is calculated as :

\mathbf{s =\sqrt [3]{\dfrac{K_{sp}}{4}}}

\mathbf{s =\sqrt [3]{\dfrac{7*10^{-9}}{4}}}

\mathbf{s} =\sqrt[3]{1.75*10^{-9}}

\mathbf{s} =\mathbf{1.21*10^{-3}  \ mol/L }

The Concentration of Pb²⁺  in 1.0 mol·L⁻¹ NaI

\mathbf{PbCl{_2}}  \leftrightharpoons    \ \ \ \ \ \ \  \mathbf{Pb^{2+}}   \ \ \ \  \ +   \ \  \ \ \ \ \ \mathbf{2 I^-}

                             \ \ \ \ \ \ \  \ \   \ \  \ \ \ \ \ \ \  \mathbf0}   \ \ \ \  \ \ \ \ \ \   \ \ \ \ \ \mathbf{1.0}

                            \ \ \ \ \ \ \ \ \ \ \ \ \ \    \ \ \ \ \  \mathbf{+x}   \ \ \ \  \    \ \  \ \ \ \ \ \mathbf{+2x}

                            \ \ \ \ \ \ \ \ \ \ \ \ \ \    \ \ \ \ \  \mathbf{+x}   \ \ \ \  \    \ \  \ \ \ \ \ \mathbf{1.0+2x}

The equilibrium constant:

K_{sp} =[Pb^{2+}}][I^-]^2 \\ \\ K_{sp} = s*(1.0*2s)^2 =7*1.0^{-9} \\ \\ s = 7*10^{-9} \ \  m/L

It is now clear that maximum possible concentration of Pb²⁺ in the solution is less than that in the solution in part (A). This happens due to the  common ion effect. The added iodide ion forces the position of equilibrium to shift to the left, reducing the concentration of Pb²⁺.

3 0
3 years ago
The vapor pressure of pure water at 296 K is 2778.5 Pa. The vapor forms an ideal gas. 1) In some oil, the equilibrium concentrat
Murljashka [212]

Explanation:

It is given that vapor pressure of pure water at 296 K is 2778.5 Pa.These vapors will result in the formation of an ideal gas.

Now, as water is covered with oil and contains only 1% molecules of water. Hence, the vapor pressure of this mixture will also be equal to the vapor pressure of pure water.

So, vapor pressure of mixture = 1% vapor pressure of pure water

Therefore, \text{(Vapor pressure)}_{mixture} = \frac{1}{100} \times 2778.5 Pa

                                                 = 27.785 Pa

Thus, we can conclude that the equilibrium vapor pressure of water above the oil layer is 27.785 Pa.

3 0
3 years ago
fish tank initially contains 35 liters of pure water. Brine of constant, but unknown, concentration of salt is flowing in at 5 l
weeeeeb [17]

Answer:

Therefore, the rate of change in the amount of salt is \frac{dx}{dt} =( 5c}{ - \frac{x }{20})

\frac{grams }{min}

Explanation:

Given:

Initial volume of water V = 35 lit

Flowing rate = 5 \frac{Lit}{min}

The rate of change in the amount of salt is given by,

   \frac{dx}{dt} = ( Rate of salt enters tank - rate of sat leaves tank )

Since tank is initially filled with water so we write that,

x(0) = 0

Let amount of salt in the solution is c,

  \frac{dx}{dt} = \frac{5c}{1 } - \frac{x(t) \times 5}{100}

  \frac{dx}{dt} =( 5c}{ - \frac{x }{20}) \frac{grams}{min}

Therefore, the rate of change in the amount of salt is \frac{dx}{dt} =( 5c}{ - \frac{x }{20})

\frac{grams }{min}

7 0
3 years ago
How many moles of methane (CH4) is<br> 6.70 x 1022 atoms of methane?
suter [353]

Answer:

0.1113  mol

Explanation:

Data Given:

no. of atoms of CH₄= 6.70 x 10²² atoms

no. of moles of methane (CH₄) = ?

Solution:

we will find no. of moles of methane (CH₄)

Formula used

          no. of moles = no. of atoms / Avogadro's number

Where

Avogadro's number = 6.022 x 10²³

Put values in above equation

         no. of moles = 6.70 x 10²² atoms / 6.022 x 10²³ (atoms/mol)

         no. of moles = 0.1113  mol

So,

There are 0.1113 moles of methane.

8 0
3 years ago
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