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2 years ago

Calculate the pH of a solution whose H3O+ concentration is 2.1 x 10-3 M. Is the solution acidc, basic, or neutral?

Chemistry

1 answer:

Leona [35]2 years ago

5 0

Answer:

Option A, The pH of the solution is 2.7 and the solution is acidic

Explanation:

As we know,

pH = - log [H3O+]

Substituting the given values, we get

pH = - log [2.1 x 10-3 M]

pH = - (-2.678)

pH = 2.678 or 2.7

The solution is acidic as pH value is less than 7

Hence, option A is correct

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How many types of hybridization does carbon undergo?

Novosadov [1.4K]

Answer:

For carbon the most important forms of hybridization are the sp2- and sp3- hybridization. Besides these structures there are more possiblities to mix dif- ferent molecular orbitals to a hybrid orbital. An important one is the sp- hybridization, where one s- and one p-orbital are mixed together.

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2 years ago

Does anyone know what the formula would be for Rhenium V Biphosphate?

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Explanation:

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2 years ago

What are the physical properties of toothpaste

bogdanovich [222]

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3 years ago

In thermodynamics, we determine the spontaneity of a reaction by the sign of ΔG. In electrochemistry, spontaneity is determined

faltersainse [42]

Answer:

For A: The standard cell potential of the reaction is 4.4 V

For B: The standard Gibbs free energy of the reaction is $-8.50\times 10^5J$

For C: The reaction is spontaneous as written.

Explanation:

For A:

The given chemical reaction follows:

$2Li(s)+Cl_2(g)\rightarrow 2Li^+(aq.)+2Cl^-(aq.)$

The given half reaction follows:

Oxidation half reaction: $Li(s)\rightarrow Li^+(aq.)+e^-;E^o_{Li^+/Li}=-3.04V$ ( × 2)

Reduction half reaction: $Cl_2(g)+2e^-\rightarrow 2Cl^-(aq.);E^o_{Cl_2/2Cl^-}=+1.36V$

The substance having highest positive $E^o$ potential will always get reduced and will undergo reduction reaction.

Here, chlorine will undergo reduction reaction will get reduced.

Substance getting oxidized always act as anode and the one getting reduced always act as cathode.

To calculate the $E^o_{cell}$ of the reaction, we use the equation:

$E^o_{cell}=E^o_{cathode}-E^o_{anode}$

$E^o_{cell}=1.36-(-3.04)=4.4V$

Hence, the standard cell potential of the reaction is 4.4 V

For B:

Relationship between standard Gibbs free energy and standard electrode potential follows:

$\Delta G^o=-nFE^o_{cell}$

where,

n = number of electrons transferred = $2mol\text{ e}^-$

F = Faradays constant = $96500J/V.mol\text{ e}^-$

$E^o_{cell}$ = standard cell potential = 4.4 V

Putting values in above equation, we get:

$\Delta G^o=-2\times 96500\times 4.4=-849200J=-8.50\times 10^5J$

Hence, the standard Gibbs free energy of the reaction is $-8.50\times 10^5J$

For C:

For a reaction to be spontaneous, the standard Gibbs free energy change of the reaction must be negative.

From above, the standard Gibbs free energy change of the reaction is coming out to be negative.

Hence, the reaction is spontaneous as written.

7 0

3 years ago

Is tropism the response of a plant to light, gravity, touching . or water?

solniwko [45]

Answer:

all

Explanation:

it can be from all as some plants are hydrotrophic i.e. they get attracted to water but some get away from water. Same sunflower faces sun from morning to evening but some plants get burnt while in sun.

3 0

3 years ago