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4 years ago

Identify the correct statements associated with titration.

Chemistry

1 answer:

Montano1993 [528]4 years ago

3 0

Answer:

Explanation:

because titration by definition, is used to determine the concentration of one reactant in an aqueous solution, it requires a burette to accurately measure the volume of a solution and endpoints in acid-base titration can be determined by a colour indicator or a pH meter

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Calculate the mole fraction of each component in a solution of 42 g CH3OH, 35 g of chloroform CHCl3, and 50 g C3H7OH

koban [17]

Considering the definition of mole fraction, the mole fraction of each component in the solution is:

CH₃OH: 0.54
CHCl₃: 0.118
C₃H₇OH: 0.342

<h3>Mole fraction</h3>

The molar fraction is a way of measuring the concentration that expresses the proportion in which a substance is found with respect to the total moles of the solution.

<h3>Mole fraction of each component</h3>

In this case, in first place you should know that the molar mass of each component is:

CH₃OH: 32 $\frac{g}{mole}$
CHCl₃: 121.35 $\frac{g}{mole}$
C₃H₇OH: 60 $\frac{g}{mole}$

Now, the number of moles of each compound can be calculated as:

CH₃OH: $\frac{42 g}{32\frac{g}{mole}}$ = 1.3125 moles
CHCl₃: $\frac{35 g}{121.35\frac{g}{mole}}$ = 0.2884 moles
C₃H₇OH: $\frac{50 g}{60\frac{g}{mole}}$ = 0.8333 moles

So, the total moles of the solution can be calculated as:

Total moles = 1.3125 moles + 0.2884 moles + 0.8333 moles

<u><em>Total moles = 2.4342 moles</em></u>

Finally, the more fraction of each component can be calculated as follow:

CH₃OH: $\frac{1.3125 moles}{2.4342 moles}$ = 0.54
CHCl₃: $\frac{0.2884 moles}{2.4342 moles}$ = 0.118
C₃H₇OH: $\frac{0.8333 moles}{2.4342 moles}$ = 0.342

In summary, the mole fraction of each component in the solution is:

CH₃OH: 0.54
CHCl₃: 0.118
C₃H₇OH: 0.342

Learn more about mole fraction:

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4 0

3 years ago

What is the definition of behavior?

Nadusha1986 [10]

Answer:

the definition of behavior is the way in which someone conducts oneself or behaves.

3 0

3 years ago

Read 2 more answers

Pure water at 25°C

Vika [28.1K]

Answer:

<u>The last statement describes the correct inozation of water:</u>

Pure water at 25ºC:

self-ionizes to form an equilibrium system in which:

$[H_3O^+]=[OH^-]=10^{-7}moles/liter$

Explanation:

It has been proven that <em>pure wate</em>r slightly conducts electricity. This fact, explained by the Arrhenius model of acids, would mean that pure water contains ions.

Since such ions are spontaneoulsy produced by the water molecules, this phenomenum is called <em>self-ionization of water</em>.

The equilibrium equation that represents the self-ionization of water is:

$H_2O(l)+H_2O(l)\rightleftharpoons H_3O^+(aq)+OH^-(aq)$

The expression for the equilibrium constant is:

$Keq=[H_3O^+(aq)][OH^-(aq)]$

As per the stoichiometry:

$[H_3O^+(aq)]=[OH^-(aq)]$

The equilibrium constant for the self-ionization of water has been determined at several temperatures. At 25ºC it is equal to 1.0×10⁻¹⁴.

Then by solving the equation you can find the concentrations of the ions:

$[H_3O^+(aq)]\cdot [OH^-(aq)]=10^{-14}$

$[H_3O^+(aq)]=[OH^-(aq)]=x\\\\x^2=10^{-14}\\\\x=\sqrt{10^{-14}}\\\\x=10^{-7}$

$[H_3O^+(aq)]=[OH^-(aq)]=10^{-7}$

Hence, we have proved that pure water self-ionizes to form an equilibrium system in which:

$[H_3O^+]=[OH^-]=10^{-7}moles/liter$

3 0

3 years ago

Read 2 more answers

Write the empirical formula for at least four ionic compounds that could be formed from the following ions: Fe2+,Cr4+,Cl-,O2-

brilliants [131]

<u>Answer:</u> Four ionic compounds formed will be $FeCl_2,FeO,CrCl_4\text{ and }CrO_2$

<u>Explanation:</u>

Ionic compound is formed by the complete transfer of electrons from 1 atom to another atom. The cation is formed by the loss of electrons by metals and anions are formed by gain of electrons by non metals.

We are given:

Two cations having formulas $Fe^{2+}\text{ and } Cr^{4+}$

Two anions having formulas $Cl^-\text{ and }O^{2-}$

By criss-cross method, the oxidation state of the ions gets exchanged and they form the subscripts of the other ions. This results in the formation of a neutral compound.

The four ionic compounds are:

When iron ion and chloride ions combine, it results in the formation of $FeCl_2$ compound. This is named as iron (II) chloride.
When iron ion and oxide ions combine, it results in the formation of $FeO$ compound. This is named as iron (II) oxide.
When chromium ion and chloride ions combine, it results in the formation of $CrCl_4$ compound. This is named as chromium (IV) chloride.
When chromium ion and oxide ions combine, it results in the formation of $Cr_2O_4=CrO_2$ compound. This is named as chromium (IV) oxide.

Hence, the four ionic compounds formed will be $FeCl_2,FeO,CrCl_4\text{ and }CrO_2$

4 0

4 years ago

In Parts I and II of the lab, what happened to the electrons of each element to produce the different colors of light? Explain y

RoseWind [281]

Answer: Electrons must be heated to emitted light. When heat was added to the elements,the electrons absorbs the energy and moves to its excited state. Once the electronstarts to fall back to a lower orbit, it emits energy in the form of light. Thedifferent lights being emitted, depends on their wavelength

Explanation: I did the Quantization of Energy Lab

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4 years ago