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Pachacha [2.7K]
2 years ago
8

Calculate the molarity of a solution prepared by diluting 7.0 mL of 4.0 M solution to a volume of 30 mL.

Chemistry
1 answer:
Finger [1]2 years ago
8 0

Considering the definition of dilution, the molarity of a solution prepared by diluting 7.0 mL of 4.0 M solution to a volume of 30 mL is 0.93 mL.

<h3>What is diluion</h3>

First of all, you have to know that when it is desired to prepare a less concentrated solution from a more concentrated one, it is called dilution.

Dilution is the process of reducing the concentration of solute in solution, which is accomplished by simply adding more solvent to the solution at the same amount of solute.

In a dilution the amount of solute does not change, but as more solvent is added, the concentration of the solute decreases, as the volume (and weight) of the solution increases.

A dilution is mathematically expressed as:

Ci×Vi = Cf×Vf

where

  • Ci: initial concentration
  • Vi: initial volume
  • Cf: final concentration
  • Vf: final volume

<h3>Molarity of the solution in this case</h3>

In this case, you know:

  • Ci= 4 M
  • Vi= 7 mL
  • Cf= ?
  • Vf= 30 mL

Replacing in the definition of dilution:

4 M× 7 mL= Cf× 30 mL

Solving:

(4 M× 7 mL)÷ 30 mL= Cf

<u><em>Cf= 0.93 mL</em></u>

In summary, the molarity of a solution prepared by diluting 7.0 mL of 4.0 M solution to a volume of 30 mL is 0.93 mL.

Learn more about dilution:

brainly.com/question/20113402

brainly.com/question/22762236

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Answer:

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small molecular volumes

Decrease

Explanation:

The percent difference between the ideal and real gas is:

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This difference is considered significant, and is best explained because argon atoms have relatively <em>small molecular volumes. </em>That produce an increasing in intermolecular forces deviating the system of ideal gas behavior.

Therefore, an increasing in volume will produce an ideal gas behavior. Thus:

If the volume of the container were increased to 2.00 L, you would expect the percent difference between the ideal and real gas to <em>decrease</em>

<em />

I hope it helps!

5 0
3 years ago
There are some data that suggest that zinc lozenges can significantly shorten the duration of a cold. If the solubility of zinc
zhuklara [117]

Answer:

K_{sp} of Zn(CH_{3}COO)_{2} is 0.0513

Explanation:

Solubility equilibrium of Zn(CH_{3}COO)_{2}:

Zn(CH_{3}COO)_{2}\rightleftharpoons Zn^{2+}+2CH_{3}COO^{-}

Solubility product of Zn(CH_{3}COO)_{2} (K_{sp}) is written as-            K_{sp}=[Zn^{2+}][CH_{3}COO^{-}]^{2}

Where [Zn^{2+}] and [CH_{3}COO^{-}] represents equilibrium concentration (in molarity) of Zn^{2+} and CH_{3}COO^{-} respectively.

Molar mass of Zn(CH_{3}COO)_{2} = 183.48 g/mol

So, solubility of Zn(CH_{3}COO)_{2} = \frac{43.0}{183.48}M = 0.234M

1 mol of Zn(CH_{3}COO)_{2} gives 1 mol of Zn^{2+} and 2 moles of CH_{3}COO^{-} upon dissociation.

so,   [Zn^{2+}] = 0.234 M and [CH_{3}COO^{-}] = (2\times 0.234)M=0.468M

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8 0
3 years ago
A solution is prepared by mixing 200.0 g of water, H2O, and 300.0 g of
VikaD [51]

Answer:

Mole Fraction (H₂O)  =  0.6303

Mole Fraction (C₂H₅OH)  =  0.3697

Explanation:

(Step 1)

Calculate the mole value of each substance using their molar masses.

Molar Mass (H₂O): 2(1.008 g/mol) + 15.998 g/mol

Molar Mass (H₂O): 18.014 g/mol

200.0 g H₂O            1 mole
---------------------  x  ------------------  =  11.10 moles H₂O
                                 18.014 g

Molar Mass (C₂H₅OH): 2(12.011 g/mol) + 6(1.008 g/mol) + 15.998 g/mol

Molar Mass (C₂H₅OH): 46.068 g/mol

300.0 g C₂H₅OH              1 mole
----------------------------  x  --------------------  =  6.512 moles C₂H₅OH
                                         46.068 g

(Step 2)

Using the mole fraction ratio, calculate the mole fraction of each substance.

                                            moles solute
Mole Fraction  =  ------------------------------------------------
                               moles solute + moles solvent

                                                  11.10 moles H₂O
Mole Fraction  =  -------------------------------------------------------------
                               11.10 moles H₂O + 6.512 moles C₂H₅OH

Mole Fraction (H₂O)  =  0.6303

                                             6.512 moles C₂H₅OH
Mole Fraction  =  -------------------------------------------------------------
                               11.10 moles H₂O + 6.512 moles C₂H₅OH

Mole Fraction (C₂H₅OH)  =  0.3697

7 0
2 years ago
If 1. 3618 moles of AsF3 are allowed to react with 1. 0000 mole of C2Cl6, what would be the theoretical yield of AsCl3, in moles
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Answer:

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4:3

1.3618 moles: 1.02135 moles(1.3618÷4×3)

C2CI6 is the limting reagent

So the number of moles for AsCI3 is 0.817 moles( number of moles of the limting reagant) ÷3 ×4 (according to ratio by balancing chemical equation)=1.09 moles(3 s.f.)

or

Balanced equation

4AsF3 + 3C2Cl6 → 4AsCl3 + 3C2Cl2F4

Use stoichiometry to calculate the moles of AsCl3 that can be produced by each reactant.

Multiply the moles of each reactant by the mole ratio between it and AsCl3 in the balanced equation, so that the moles of the reactant cancel, leaving moles of AsCl3.

Explanation:

5 0
2 years ago
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