Which is a spectator ion in the reaction between these two solutions?

BaBr2(aq) + Na2SO4(aq) →

A. Br– (aq)

B. BaBr2(aq)

C. Ba2+(aq)

D. SO42–(aq)

I don't know how 5°C cooled to 85°C but the answer would be 12.878L

Answer:

At constant pressure the new volume of gas is 12.878 L.

Explanation:

Charles's Law consists of the relationship between the volume and temperature of a certain amount of ideal gas, which is maintained at a constant pressure, by means of a proportionality constant that is applied directly. So the ratio between volume and temperature will always have the same value:

[tex]\frac{V}{T} =k[/tex]

where the temperature is expressed in degrees kelvin (° K)

Then, when considering the two situations 1 and 2, keeping the amount of gas and the temperature constant, the relationship must be met:

[tex]\frac{V1}{T1} =\frac{V2}{T2}[/tex]

In this case, you know:

Replacing:

[tex]\frac{10}{278} =\frac{V2}{358}[/tex]

Solving:

[tex]V2=\frac{10}{278} *358[/tex]

V2=12.878 L

At constant pressure the new volume of gas is 12.878 L.

Answer:

C) reduced

Explanation:

NAD+ becomes reduced when it gains a hydrogen atom, transforming into NADH, which plays a significant role in cellular energy metabolism.

When a molecule of NAD+ (nicotinamide adenine dinucleotide) gains a hydrogen atom, the molecule becomes reduced. This process of gaining an electron (or hydrogen atom) is known as reduction in metabolism. Essentially, NAD+ serves as an important electron carrier within cells and as it accepts electrons, it becomes reduced to its alternate form called NADH. It's important to note that oxidation and reduction reactions often go hand in hand in biological systems, which is why they are typically referred to as redox reactions. In this context, NAD+ is reduced (gains an electron) to form NADH, which then plays a crucial role in energy metabolism within the cell.

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Answer: Adding Hydrogen Gas

Explanation:

The Reduction Reaction that occurs during the refinement of Iron Ore is as follows:

[tex]Fe_3O_4 + H_2  -> 3FeO + H_2O\\\\FeO + H_2   -> Fe + H_2O[/tex]

Since Hydrogen Gas is a reactant in the equation with Iron ore , adding more hydrogen gas will shift the reaction toward the right side, increase the amount of  refined iron produced.

Answer:

The correct answer is increase in temperature.

Explanation:

During heating of the iron ore with the hydrogen gas at high temperature, the production of water and element iron takes place. High temperature is one of the essential condition for this chemical reaction to take place.  

The more the temperature is, the more will be the amount of the production of iron, this is due to the presence of high temperature, which is one of the mediating force for the production of iron. Therefore, an increase in temperature will produce a greater amount of iron.  

A is correct (1 h should be written as 1 s)

I just took this exam. :)

Answer:

Your correct answer is A. 1 h should be written as 1 s.

Explanation:

The Intermolecular forces increase with increasing polarization of bonds. The strength of Intermolecular forces (and therefore impact on boiling points) is ionic > hydrogen bonding > dipole dipole > dispersion. Boiling point increases with molecular weight, and with surface area.

The approximate value of the volume of the gas is 958.3L

Using the ideal gas equation which is a combination of pressure law, Boyle's law and Charles's law.

Mathematically

[tex]PV=nRT[/tex]

we convert the value of temperature from degree Celsius to Kelvin.

To do this, simply add 273.15 to the °C value.

[tex]T=15 + 273.15 = 288.15K[/tex]

From the data given, we can substitute into the equation and solve for v

[tex]PV = nRT\\3.75*V=1.5*8.314*288.15\\3.75V=3593.52\\V=\frac{3593.52}{3.75}\\V=958.27L[/tex]

The approximate value of the volume is 958.3L

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No. Catalyst only reduce the activation energy, but don't change the energy released by the reaction.

A catalyst will alter the enthalpy of a reaction (the amount of heat that is released/absorbed) so it's not going to have the desired effect.

A catalyst is a substance that speeds up a chemical reaction, or lowers the temperature or pressure needed to start one, without itself being consumed during the reaction.

A catalyst increases the rate of a reaction, but does not get consumed in the reaction and does not alter the equilibrium constant.

In other words, a catalyst affects the kinetics of a reaction, but not the thermodynamics.

They work by increasing the rate of reaction through lowering the activation energy.

Hence, a catalyst will alter the enthalpy of a reaction (the amount of heat that is released/absorbed) so it's not going to have the desired effect.

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[H+] = 0.051 M

[SO4=] = 0.051M  

[HSO4-] = 0.16M

HSO4- <==> H+ + SO4= ..... Ka = 1.3x10^-2

Ka = [H+] [SO4=] / [HSO4-]  

1.3x10^-2 = x^2 / (0.21-x)  

Using algebra and solving the quadratic equation to solve for x.  

x = 0.051  

Therefore;

[H+] = [SO4=] = 0.051M  

[HSO4-] = 0.16M

Answer : The concentration of [tex]HSO_4^-[/tex], [tex]SO_4^{2-}[/tex] and [tex]H^+[/tex] are 0.29 M, 0.061 M and 0.061 M respectively.

Explanation :

First we have to calculate the concentration of [tex]HSO_4^-[/tex]

The dissociation of [tex]KHSO_4[/tex] is:

[tex]KHSO_4\rightarrow K^++HSO_4^-[/tex]

As, 1 mole of [tex]KHSO_4[/tex] gives 1 mole of [tex]HSO_4^-[/tex]

So, 0.35 M of [tex]KHSO_4[/tex] gives 0.35 M of [tex]HSO_4^-[/tex]

Now we have to determine the concentration of [tex]SO_4^{2-}[/tex] and [tex]H^+[/tex].

The dissociation of [tex]HSO_4^-[/tex] is:

                          [tex]HSO_4^-\rightleftharpoons H^++SO_4^{2-}[/tex]

Initial conc.      0.35           0       0

At eqm.          (0.35-x)        x        x

The expression of acid dissociation constant will be:

[tex]K_a=\frac{[H^+][SO_4^{2-}]}{[HSO_4^-]}[/tex]

Now put all the given values in this expression, we get:

[tex]1.3\times 10^{-2}=\frac{(x)\times (x)}{(0.35-x)}[/tex]

[tex]x=0.061M[/tex]

Thus, the concentration of [tex]SO_4^{2-}[/tex] = x = 0.061 M

The concentration of [tex]H^+[/tex] = x = 0.061 M

The concentration of [tex]HSO_4^-[/tex] = 0.35 - x = 0.35 - 0.061 = 0.29 M

1.0875 x 10-2 atm

2O3(g) → 3O2(g)

rate = -(1/2)∆[O3]/∆t = +(1/3)∆[O2)/∆t  

The average rate of disappearance of ozone ... is found to  

be 7.25 × 10–3 atm over a certain interval of time.

This means (ignoring time)

∆[O3]/∆t = -7.25 × 10^–3 atm  

(it is disappearing, thus the negative sign)

rate = -(1/2)∆[O3]/∆t  

rate = -(1/2)*(-7.25 × 10^–3 atm)

      = 3.625 × 10^–3 atm  

Now use the other part of the expression:  

rate = +(1/3)∆[O2)∆t  

3.625 × 10–3 atm = +(1/3)∆[O2)/t  

∆[O2)/∆t = (3)*(3.625× 10^–3 atm)

              = 1.0875 x 10-2 atm over the same time interval

From the parameters given, the rate of appearance of O2 is 1.1 * 10^-2.

The equation of the reaction is;

2O3(g) → 3O2(g)

We can see from the equation that; [tex]-\frac{1}{2} \frac{d[O3]}{dt} = \frac{1}{3} \frac{d[O2]}{dt}[/tex]

Hence it follows that;

[tex]-\frac{3}{2} \frac{d[O3]}{dt} = \frac{d[O2]}{dt}[/tex]

Since we already have the rate of disappearance of O3 from the problem as 7.25 × 10^-3, the rate of appearance of O2 is now given by;

[tex]\frac{d[O2]}{dt} = \frac{3}{2} * 7.25 * 10^-3[/tex]

[tex]\frac{d[O2]}{dt} = 1.1 * 10^-2[/tex]

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Answer:

Explanation:

1) Since the two rooms are connected by an open door, you assume pressure equilibrium: the pressure on the two rooms is the same.

2) Since you consider two equal size rooms, both volumes are equal.

3) Assuming ideal gas behavior, pressure (P), temperature (T), volume (V) and number of moles (n) are related by the equation PV = nRT

4) Naming T₁ the lower temperature, T₂ the higher temperature, n₁ the number of moles of air in the room at lower temperature, and n₂ the number of moles of air in the room at higher temperature, you get:

5) That means that the amount of molecules (number of moles) is inversely related to the temperature: the higher the temperature the lower the number of moles, and the lower the temperature the greater the number of moles.

Hence, the answer is that the room that contains more air molecules is the room mantained at a lower temperature.

The room that has the lower temperature is expected to have the greater number of gas molecules since the molecules

Ideal gases are the gases that obey the ideal gas equation. We know that for ideal gases, the temperature of a given mass of gas is inversely proportional to the number of moles of gas hence we can write; n₁ / n₂ = T₂ / T₁.

Since the above is true, it the follows that the room that has the lower temperature is expected to have the greater number of gas molecules since the molecules posses less kinetic energy to escape.

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When an alkane is heated in the presence of chlorine gas, monochlorinated products can be formed.

These products can include stereoisomers. In the case of methane, there are four possible monochlorinated products including stereoisomers. The alkane is not specified in the question, but let's assume it is methane (CH4) as an example. When methane is heated in the presence of chlorine gas (Cl2), a substitution reaction occurs. One of the hydrogen atoms in methane can be replaced by a chlorine atom, resulting in a monochlorinated product. In this case, there are four possible monochlorinated products (CH3Cl, CH2Cl2, CHCl3, CCl4) including different stereoisomers.

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A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass. A 5.25-g sample of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at -4.0°C. Which of the following is its molecular formula?  

1) NO2  

2) N3O6  

3) N2O5  

4) N2O4  

5) NO

There are not too many things that are more insoluble than AgCl. When you actually do this experiment, virtually all of the AgCl sinks to the bottom of the test tube (or whatever container you are doing it in). The CuCl2 is very soluble. It is a gorgeous Forest Green with a very slightly blue tinge so you can tell that you are successful.  

CuCl2 is very soluble.

That makes A incorrect.

AgCl is really insoluble

Looks like B is the answer.

C is just wrong. No complex is formed. The equation is a double replacement.

AgNO3 + HCl ====> AgCl(s) + HNO3 Not a good example but it is correct.

Cu(NO3)2 + 2HCl ===> CuCl2 + 2HNO3

D is not true. Ag will react with the HCl That's how you get AgCl going to the bottom.

E A double replacement need not transfer electrons. In this case it does not. E is incorrect.

Answer:

0.957 atm.

Explanation:

PV = nRT.

where, P is the pressure of the gas in atm.

V is the volume of the container in L.

n is the no. of moles of the gas.

R is the genral gas constant.

T is the temperature of the gas in K.

∵ n = mass/molar mass.

∴ PV = (mass/molar mass)RT

∴ P = (mass/V)(RT/molar mass)

∵ d = mass/V

∴ P = dRT/molar mass

∵ d = 2.51 g/L, R = 0.082 L.atm/mol.K, T = 25°C + 273 = 298 K, molar mass of SO₂ = 64.06 g/mol.

∴ P = dRT/molar mass = (2.51 g/L)(0.082 L.atm/mol.K)(298.0 K)/(64.06 g/mol) = 0.957 atm.

The pressure in the flask is approximately 0.993 atmospheres.

The correct answer is that the pressure in the flask containing SO2 gas at a density of 2.51 g/L at room temperature (25.0°C) can be determined using the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

First, we need to calculate the molar mass of SO2. The molar mass of sulfur (S) is approximately 32.07 g/mol and that of oxygen (O) is approximately 16.00 g/mol. Since SO2 has one sulfur atom and two oxygen atoms, its molar mass is:

[tex]Molar mass of SO2 = 32.07 g/mol (S) + 2 \times 16.00 g/mol (O) = 64.07 g/mol[/tex]

Next, we can use the density (d) of the gas to find the mass (m) of the gas in a container of known volume (V). The density is given as 2.51 g/L, so for a volume of 1 liter, the mass would be:

[tex]m = d \times V = 2.51 g/L \times 1 L = 2.51 g[/tex]

 Now, we can find the number of moles (n) of SO2 using the molar mass (M):

[tex]n = m / M = 2.51 g / 64.07 g/mol = 0.0392 mol[/tex]

The ideal gas constant (R) is 0.0821 L·atm/mol·K. The temperature (T) in Kelvin is room temperature (25.0°C) plus 273.15, which gives:

[tex]T = 25.0 + 273.15 = 298.15 K[/tex]

Now we can rearrange the ideal gas law to solve for pressure (P):

[tex]P = nRT / V[/tex]

Since we are considering a volume of 1 liter, the equation simplifies to:

[tex]P = (0.0392 mol)(0.0821 L\times atm/mol\times K)(298.15 K) / 1 L[/tex]

[tex]P =0.993 atm[/tex]

 Therefore, the pressure in the flask is approximately 0.993 atmospheres.

Answer:

A

Explanation:

This kind of bond is known as an ionic bond and is based on electrostatic forces between two charged molecules/atoms. To achieve stable configuration, sodium (2.8.1) transfers its valence electron to chlorine that also needs one electron to achieve stable configuration (2.8.8), and combine in an ionic bond.

Answer: The correct answer is Option A.

Explanation:

Sodium is the 11th element of the periodic table having electronic configuration of [tex][Ne]3s^1[/tex]

This element will loose 1 electron in order to attain stability and will form [tex]Na^+[/tex] ion.

Chlorine is the 17th element of the periodic table having electronic configuration of [tex][Ne]3s^23p^5[/tex]

This element will gain 1 electron in order to attain stability and will form [tex]Cl^-[/tex] ion.

These two elements form ionic compound by transferring of electrons from sodium atom to chlorine atom.

Hence, the correct answer is Option A.

thanks for the answers ッ. (btw they’re on the bottom of the question if anyone doesn’t see it.

Alpha particles consist of two protons and two neutrons, it is produced during alpha decay and release energy.

Alpha particles are the small part of a matter which carry positive charge in it.

From the definition of the alpha particles, it is clear that it is positively charged particle and no electron is present in it. It mainly consist 2 protons and 2 neutrons in it. It is produced by the decay of very heavy radioactive elements which are unstable and releases energy with alpha particle to gain stability, and this decay is known as alpha - decay.

Hence, option (1), (3) and (5) is correct.

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Answer:

[CH₃OH] to decrease and [CO] to increase.

Explanation:

[CH₃OH] to decrease and [CO] to increase.

I believe it’s called Wisteria

the big number describes the number ratio in a chemical equation

so for example,

2H2 + O2 --> 2H2O means

2 moles of hydrogen reacts with one mole of oxygen to form 2 moles of water

and as you know, the small (subscript) number determines the number of atoms of that element in one molecule of a compound

so I believe that drawing a normal lewis structure ( O=O ) should be correct

Explanation:

For what I understand in the question, the "big number" is called a stoichiometric coefficient and represents the ammount of molecules of the substance that follows it ( in this case O2) involved in a reaction.

In this case there is no reaction but it asks you for the lewis structure of two molecules of oxygen (O2).

The lewis structure of oxygen is: O=O

Two molecules of it can bond by london forces or dative unions forming what is known as a dimer (two molecules of the same substance bonded).

Answer:

B. ethylamine.

Explanation:

So, the compound is ethylamine.

Answer:

5. ΔH = 238.7 kJ; 6 ΔH, = -1504.6 kJ

Step-by-step explanation:

Question 5:

We have three equations:  

(I)  CH₃OH + ³/₂O₂ ⟶ CO₂ + 2H₂O;  ΔH = -726.4 kJ

(II)  C + O₂ ⟶ CO₂;                              ΔH = -393.5 kJ

(III) H₂ + ½O₂ ⟶ H₂O;                         ΔH = -285.8 kJ

From these, we must devise the target equation:  

(IV) C + 2H₂ + ½ O₂ → CH₃OH; ΔH = ?  

The target equation has 1C on the left, so you rewrite Equation (II)..  

(V) C + O₂ ⟶ CO₂;                               ΔH = -393.5 kJ

Equation (V) has 1CO₂ on the right, and that is not in the target equation.  

You need an equation with ½O₂ on the left, so you reverse Equation (I).  

When you reverse an equation, you reverse the sign of its ΔH.  

(VI) CO₂ + 2H₂O ⟶ CH₃OH + ³/₂O₂;  ΔH = 726.4 kJ

Equation (VI) has 2H₂O on the left, and that is not in the target equation.

You need an equation with 2H₂O on the right. Double Equation (III).

When you double an equation, you double its ΔH.  

(VII) 2H₂ + O₂ ⟶ 2H₂O;                        ΔH = -571.6 kJ

Now, you add equations (V), (VI), and (VII), cancelling species that appear on opposite sides of the reaction arrows.

When you add equations, you add their ΔH values.

We get the target equation (IV)  

(V)   C + O₂ ⟶ CO₂;                              ΔH = -393.5 kJ

(VI)  CO₂ + 2H₂O ⟶ CH₃OH + ³/₂O₂ ;  ΔH =  726.4 kJ

(VII) 2H₂ + O₂ ⟶ 2H₂O;                        ΔH = -571.6 kJ

(IV)  C + 2H₂ + ½ O₂ → CH₃OH;             ΔH = -238.7 kJ  

Question 6

We have three equations:  

(I) Mg + ½O₂ → MgO;  ΔH = -601.7 kJ

(II) Mg + S ⟶ MgS;      ΔH = -598.0 kJ

(III) S + O₂ ⟶ SO₂;       ΔH = -296.8 kJ

From these, we must devise the target equation:  

(IV) 3Mg + SO₂ → MgS + 2MgO; ΔH = ?  

The target equation has 1SO₂ on the left, so you reverse Equation(III).

(V) SO₂ ⟶ S + O₂;         ΔH = 296.8 kJ

Equation (V) has 1S on the right, and that is not in the target equation.  

You need an equation with 1S on the left, so you rewrite Equation (II).  

(VI) Mg + S ⟶ MgS;        ΔH = -598.0 kJ

Equation (V) has 1O₂ on the right, and that is not in the target equation.

You need an equation with 1O₂ on the left. Double Equation (I).

(VII) 2Mg + O₂⟶ 2MgO ;  ΔH = -1203.4 kJ  

Now, you add equations (V), (VI), and (VII), cancelling species that appear on opposite sides of the reaction arrows.

We get the target equation (IV)  

(V)   SO₂ ⟶ S + O₂;                    ΔH =    296.8 kJ

(VI)   Mg + S ⟶ MgS;                  ΔH = -  598.0 kJ

(VII) 2Mg + O₂ ⟶ 2MgO;            ΔH = -1203.4 kJ

(IV)  3Mg + SO₂ → MgS + 2MgO; ΔH = -1504.6 kJ

Answer:

        c. 2N₂O₅(g) ⇄ 4 NO₂(g)+ O₂(g), and

        d. N₂O₄(g) ⇄ 2 NO₂(g)

Explanation:

Volume and pressure are inversely related (Boyle's law).

Volume and number of molecules are directly related (Avogadro's principle).

As per Le Chatelier's principle, the reaction will shift toward the side that permits to overcome or minimize the force that disturbs the equilibrium.

With those concepts you can predict which equilibria will shift toward formation of more products if the volume of a reaction mixture at equilibrium increases by a factor of 2

Let's dig into each option.

a. 2 SO₂(g)+ O₂(g) ⇄ 2 SO3(g)

Incorrect.

There are three molecules in the reactant side and two in the product side. so the increase in volume will favor the reverse reaction. This is, the equilibrium will shift to the formation of more reactants, and this is an incorrect choice.

b. NO(g) + O₃(g) ⇄ NO₂(g) + O₂(g)

Incorrect.

There are the same number of molecules in the reactant side and the product side. Hence, the increase of volume will not produce a change in the equlibrium.

c. 2N₂O₅(g) ⇄ 4 NO₂(g)+ O₂(g)

Correct.

There are 2 molecules in the reactant side (left) and four molecules in the product side (right). So, the increase in volume in this system will produce a shift toward the product side.

d. N₂O₄(g) ⇄ 2 NO₂(g)

Correct.

There are more molecules in the product side than in the reactant side, so you predict that the equilibrium will shift toward the formation of more product to overcome the increase of volume.

Equilibrium shift is the shift of the reaction towards the stressed conditions in the reactions. The shift towards the formation of the products will occur in [tex]\rm 2N_{2}O_{5}(g) \rightleftharpoons 4 NO_{2}(g)+ O_{2}(g)[/tex] and [tex]\rm N_{2}O_{4}(g) \rightleftharpoons 2 NO_{2}(g)[/tex].

According to the Le principle the reaction shift towards the site or the reactants and products where the disturbance or the stress is present so that it can be overcome.

In the third equation reaction, [tex]\rm 2N_{2}O_{5}(g) \rightleftharpoons 4 NO_{2}(g)+ O_{2}(g)[/tex]  the number of the molecules on the left side is 2 and on the right side of the product have 4 molecules.  When the volume is increased then the reaction shifts towards the right or the product side.

In the fourth reaction, [tex]\rm N_{2}O_{4}(g) \rightleftharpoons 2 NO_{2}(g)[/tex] the number of the products are more compared to the reactants and hence the increase in the volume will shift the reaction towards the formation of the product.

Therefore, option c. [tex]\rm 2N_{2}O_{5}(g) \rightleftharpoons 4 NO_{2}(g)+ O_{2}(g)[/tex] and option d. [tex]\rm N_{2}O_{4}(g) \rightleftharpoons 2 NO_{2}(g)[/tex] are the reactions that shift towards product formation.

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If you don't wash the thermometer, residual NaOH will react with the HCl solution. This is a highly exothermic reaction and will change the temperature of the solution, and thus throw off your measurement.

Not rinsing and drying the thermometer between measurements in an experiment involving HCl and NaOH solutions could skew results by unintentionally introducing acid or base into the other solution, altering the pH and temperature readings, and potentially the titration results.

In the experimental procedure where you measure the temperature of an HCl solution and then a NaOH solution without rinsing and drying the thermometer, your results may be compromised. This is because there could be a carry-over of acid (HCl) or base (NaOH) from one solution to the other which could potentially affect the pH of the solutions being measured. The pH of a solution is dependent on its hydrogen ion concentration, so any residual acid or base on the thermometer could interact with the other solution, altering its pH and therefore its temperature.

Titration is a technique that uses a solution of known concentration to find the concentration of an unknown solution. In your experiment, if you measured the temperature of the HCl solution and then immediately measured the temperature of the NaOH solution without rinsing and drying the thermometer, you might unintentionally introduce some HCl into the NaOH solution. This could potentially skew your results as the introduction of acid could decrease the pH of the NaOH solution, making it less basic than it actually is, and this could affect the titration results.

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Final answer:

The pH of a 0.160 M ammonia solution can be calculated using the pOH method. The concentration of hydroxide ions in the solution is approximately 1.125 x 10^-4 M, resulting in a pOH of approximately 3.95. The pH of the solution is approximately 10.05.

Explanation:

The pH of a 0.160 M ammonia solution can be calculated using the pOH method. Ammonia is a weak base, so we can use the equation:
pOH = -log[OH-]
pH + pOH = 14

First, we need to find the concentration of hydroxide ions ([OH-]) in the solution. The Kb value for ammonia (NH3) is 1.8 x 10-5.
Given that [NH3] = 0.160 M, we can calculate [OH-] using the Kb expression:
Kb = [NH3][OH-] / [NH4+]
Since [NH4+] can be ignored in this dilute ammonia solution, the equation simplifies to:
Kb = [NH3][OH-].

Now, rearranging the equation to solve for [OH-], we get:
[OH-] = Kb / [NH3]
Substituting the given values into the equation:
[OH-] = (1.8 x 10-5) / (0.160)
[OH-] = 1.125 x 10-4 M

Next, we can calculate the pOH of the solution using the equation:
pOH = -log[OH-]
pOH = -log(1.125 x 10-4)
pOH ≈ 3.95

Finally, we can find the pH using the equation:
pH = 14 - pOH
pH = 14 - 3.95
pH ≈ 10.05

Answers:

1. 282 g/mol

2. (a) pH = 10.0; (b) pKₐ = 5.5; Kₐ = 3 × 10⁻⁶; (c) thymolphthalein

Step-by-step explanation:

1. Molar mass of unknown acid

The equation for the reaction is

HA + NaOH ⟶ NaA + H₂O

(a) Calculate the moles of NaOH

Moles of NaOH = 0.023 64 L NaOH × (0.1 mol NaOH/1 L NaOH)

= 2.364 × 10⁻³ mol NaOH

(b) Moles of HA

Now, you use the molar ratio from the balanced chemical equation to find the moles of unknown acid.

Moles of HA = 2.364 × 10⁻³ mol NaOH × (1 mol HA/1 mol NaOH)

= 2.364 × 10⁻³ mol HA

(c) Molar mass of HA

You know now that 0.5632 g of HA .

MM = mass/moles = 0.5632 g/2.364 × 10⁻³ mol = 238.2 g/mol

2. Titration of acetic acid

(a) Equivalence point

The equivalence point is the pH at the steepest point of the titration curve.

In your titration of vinegar, the equivalence point appears to be at about

pH 10.0.

(b) Half-way point

At the half-way point, you have neutralized half the acid HA and converted it into the sane amount of A⁻, so [HA] = [A⁻].

Kₐ = [H₃O⁺] × [A⁻]/[HA] = [H₃O⁺]

At the half-way point, Kₐ = [H₃O⁺] and pKₐ = pH.

Your equivalence point is at about 21.3 mL, so the half-way point is at 10.7 mL.

The pH at 10.6 mL is about 5.5.

pH = pKₐ = 5.5

Kₐ = 10^(-pKₐ) = 10^(-5.5)  = 3 × 10⁻⁶

(c) Appropriate indicator

An indicator is a weak acid in which the acid form HA is a different colour than the base form A⁻.

The colour change occurs when [HA] = [A⁻] and pH = pKₐ.

Your indicator should have pKₐ ≈ 10 (Kₐ≈ 10⁻¹⁰), so it changes colour at the equivalence point (pH 10).

The best indicator is thymolphthalein, because it has Kₐ = 10⁻¹⁰.

Answer:

A. 11

Explanation:

atoms are made of three types of sub atomic particles - protons, neutrons and electrons

Protons are positively charged, electrons are negatively charged and neutrons are neutral.

Protons and neutrons are located inside the nucleus and electrons orbit around the nucleus in energy shells.

Atoms make up an element and atoms are neutral charged with an equal number of protons and electrons. Neutral atom of sodium would therefore have an equal number of positive charges and negative charges.

Since Na has 11 protons, for it to be neutral it would have 11 electrons

An electrolyte is a compound that conducts an electric current in an aqueous solution or in the molten state. This happens when the substance dissolves in water and forms ions. The dissolved or molten ions can move freely, allowing the solution to conduct electricity.

A compound that conducts an electric current in an aqueous solution or in the molten state is known as an electrolyte. Electrolytes are formed when certain substances dissolve in water and either undergo a physical or a chemical change that yields ions in solution. These substances are important as they conduct electric current in a solution due to the presence of ions.

For example, ionic compounds like NaCl (table salt) disassociate completely in water forming Na+ and Cl- ions, giving the solution the ability to conduct electricity. In another example, covalent compounds like HCl (hydrochloric acid) also conduct electricity in water. This happens because when HCl is dissolved in water, it reacts with water molecules to form ions of H+ and Cl-.

However, the ability to conduct electricity is not limited to aqueous solutions; compounds can also conduct electricity in the molten state. For instance, when table salt is melted, it’s able to conduct electric current because the ionic bonds are broken, freeing the ions and enabling them to move and carry the current.

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That's just an error in the source.

There are 3H₂O on each side of the reaction arrows, so all the water molecules must cancel.

Let the mass be X g

percentage = X/ 6.50 * 100 =2.2%

X= 0.143 g

The mass is 0.143 g

The mass is X g

============================

percentage is X/6.50*100 =2.2%

-----------------------------------------------

X=0.143g

-------------------------------

| The mass is 0.143g |

-------------------------------

In a hydrogen atom, the 3s → 1s transition would result in the emission of the photon with the highest energy, according to the Bohr model. Energy released in photon form is highest when the transition ends at the ground state (n = 1), from the highest available initial energy level.

For a hydrogen atom, the electronic transition that would result in the emission of the photon with the highest energy would be the transition from the highest initial energy level to the lowest final energy level, which is the ground state (n = 1). Comparing the given transitions, 2p → 1s is not listed; hence, we consider the next highest, which would be 3s → 1s.

The energy of a photon emitted during an electron transition is directly proportional to the difference in energy between the two energy levels according to the equation E = hν, where E is the energy of the photon, h is Planck's constant, and ν is the frequency of the photon. Since the ground state has the lowest energy, any transition to it from a higher energy level will release more energy as a photon compared to transitions between higher levels.

The Bohr model is used to predict the energies involved in transitions between energy levels in a hydrogen atom. Emission of photons occurs when an electron falls from a higher energy level (n > m) to a lower one (n < m) and the energy of the emitted photon is equal to the difference in energy between those levels. The transitions that release the most energy are those that end at the n = 1 level, known as the Lyman series.

Specifically, a transition from n = 3 to n = 1 would result in a higher energy photon than those from n = 5 or 6 to levels other than n = 1, as indicated in the choices provided.

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