Select the correct order of solubilities of the following iron compounds in water:
Fe(OH)3 Ksp = 2.8 x 10-39
Fe(OH)2 Ksp = 4.9 x 10-17
FeCO3 Ksp = 3.5 x 10-11

- The order of solubilities is Fe(OH)2 < FeCO3 < Fe(OH)3
- The order of solubilities is Fe(OH)3 < Fe(OH)2 < FeCO3
- The order of solubilities is Fe(OH)3 < FeCO3 < Fe(OH)2
- The order of solubilities is FeCO3 < Fe(OH)3 < Fe(OH)2

Answer:

Explanation:

Therefore, the pH of the HCl solution is 5.

Explanation:

To calculate the pH of a buffer with a known pKa for the conjugate acid, the Henderson-Hasselbach equation can be used to obtain the pH of the buffer:

[tex]pH = pK_a + log_{10}(\frac{[A^-]}{[HA]} )[/tex]

[A-] is the concentration of the conjugate base and [HA] is the concentration of the conjugate acid.

The ideal gas law may be used to calculate the temperature at which 12.3 g of He would need to be cooled to fit a 34.0 l tank at 1.17 atm. According to this rule, the ideal gas constant multiplied by the number of moles in the gas equals the product of an ideal gas's pressure, volume, and temperature.

In order to solve for temperature, we may thus rearrange the equation. PV = nRT, where P is for pressure, V is for volume, n is for moles, R is for the ideal gas constant, and T is for temperature, is the equation. By multiplying both sides of the equation by the inverse of P and dividing both sides by nR, we may find the value of T.This results in the formula T = PV/nR.

The values for P, V, and nR can be substituted for the predetermined conditions. The volume is 34.0 l and the pressure is 1.17 atm. By dividing the mass, 12.3 g, by He's molar mass, 4.00 g/mol, the amount of moles of He may be computed. 0.0821 L*atm/K*mol is the ideal gas constant. Plugging these values into the equation gives us a temperature of about -267.7 K.

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The net ionic equation for the reaction that occurs when aqueous solutions of potassium phosphate and iron(II) nitrate are mixed is:

3Fe2+(aq) + 2PO43-(aq) → Fe3(PO4)2(s)

Therefore, the correct answer is A.

According to the stoichiometry of the combustion reaction of propane for each mole of propane that reacts, 5 moles of oxygen are produced.

Stoichiometry is  defined as the determination of proportions of elements or compounds which are present  in a chemical reaction. The related relations are all  based on law of conservation of mass and law of combining weights and volumes.

Stoichiometry is used in quantitative analysis for measuring concentrations of substances  which are present in the sample.As per the chemical equation C₃H₈ +5 O₂[tex]\rightarrow[/tex]3 CO₂ + 4 H₂O.For every mole of propane that reacts, 5 moles of oxygen are produced.

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Among the given compounds, I would expect the compound F (CH₂CH₂CHCH₃) to rearrange. This expectation is based on the concept of hyperconjugation and the stability of carbocations.

In organic chemistry, carbocations are positively charged carbon species with only six electrons in their valence shell. The rearrangement of a compound occurs when a more stable carbocation can be formed through the shifting of atoms or groups. This rearrangement is driven by the desire to achieve greater stability.

In compound F, the carbon atom adjacent to the positively charged carbon (CH₃⁺) is a primary carbon (attached to only one other carbon atom), making it less stable. By undergoing a rearrangement, this carbon can shift its attachment to the adjacent carbon, creating a secondary carbocation (with two carbon attachments) and a more stable molecule.

The rearrangement would result in the formation of a more stable carbocation, which is energetically favorable. This rearrangement process is known as a 1,2-shift or alkyl shift.

Overall, compound F would be expected to rearrange due to the increased stability offered by the formation of a secondary carbocation, resulting in a more energetically favorable molecular structure.

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Answer:

The empirical formula of the compound is C2H5O.

The new volume of the gas is 56.6 liters when the temperature is raised to 325 K and the pressure is lowered to 1.2 atm.

PV = nRT

Where R is the ideal gas constant. Since the number of moles is constant in this problem, we can simplify the ideal gas law to:

P1V1/T1 = P2V2/T2

Where the subscripts 1 and 2 refer to the initial and final states of the gas, respectively.

We can now plug in the given values for the initial state of the gas:

P1 = 2.3 atm

V1 = 25 L

T1 = 299 K

And the given values for the final state of the gas:

P2 = 1.2 atm

T2 = 325 K

We can then solve for V2:

P1V1/T1 = P2V2/T2

(2.3 atm)(25 L)/(299 K) = (1.2 atm)V2/(325 K)

V2 = (2.3 atm)(25 L)(325 K)/(1.2 atm)(299 K)

V2 = 56.6 L (rounded to three significant figures)

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The specific heat of the object is approximately 0.930 J/g°C.To find the specific heat of an object, we can use the formula:Q = mcΔT,Where Q represents the heat energy transferred, m is the mass of the object, c is the specific heat, and ΔT is the change in temperature.

Given that the mass of the object is 75 g and the temperature change is from 50°C to 93°C, we can plug these values into the formula:

3000 J = (75 g) * c * (93°C - 50°C)

Simplifying the equation:

3000 J = (75 g) * c * 43°C

Now, we can solve for c by dividing both sides of the equation by (75 g * 43°C):

c = 3000 J / (75 g * 43°C)

Calculating this expression:

c ≈ 0.930 J/g°C

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When the products and reactants do not alter over time, we say that a chemical is in equilibrium concentration.  2 mol/ L is the of concentration for each reactant.

When the products and reactants do not alter over time, we say that a chemical is in equilibrium concentration. In other words, a chemical reaction enters a state of equilibrium or equilibrium concentration when the rate of forward reaction equals the rate of backward reaction. CAO=CBO=2m0l/dm³ and KC=10dm³/mol. substituting all the given values we get 2 mol/ L of concentration for each reactant.

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The tests that show positive results for the food sample are Benedict's and Biuret tests only.

Benedict's test is a chemical test used to detect the presence of reducing sugars, such as glucose, in a solution. It involves adding Benedict's reagent, which contains copper ions, to the solution and heating it. If reducing sugars are present, the copper ions are reduced to form a red precipitate.

Biuret test is a chemical test used to detect the presence of protein in a solution. It involves adding Biuret reagent, which contains copper ions, to the solution. If protein is present, the copper ions react with the peptide bonds in the protein to form a violet-colored complex.

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The polar bond is stronger than a nonpolar bond as there is an extra force of attraction present in the polar bonds like positive and negative charges.

Polarity is a concept that describes the difference in the electron density of atoms in a molecule.

The polarity of an atom increase with the increase in electron density difference.

When the electrons are not distributed equally during the bond formation such a type of bond is called a polar bond.

When the electrons are equally distributed during the bond formation such a type of bond is called a nonpolar bond.

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It is incorporated with audio equipment to enhance sound quality. Diamonds are hard and easily vibrate at fast speeds, which results in high-quality sound. High-end recorders and DJ equipment both use it. Nanodiamonds have potential health benefits.

The carbon atoms in diamond are organised in a diamond cubic crystal lattice, making it an allotrope of carbon. Diamond is the material with the highest heat conductivity and hardness among all naturally occurring substances. Diamond is a particularly important component of industrial cutting and polishing equipment due to its unique qualities.

These days, diamond exfoliators and face products are accessible. Diamond dust is now being used in cosmetics, thus the price will undoubtedly be exorbitant. Diamond is used in beauty products to minimize wrinkles, etc.

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If the temperature is increased to 30.0 °C, an additional 39.9 g of solute can be dissolved in the remaining water, for a total of 62.5 g solute in 100 g of water at 30.0 °C.

To solve this problem, we can use the fact that solubility generally increases with temperature. We can first find the amount of solute that has already been dissolved in the 51.0 g of water at 20.0 °C, and then calculate how much more solute can be dissolved in the additional amount of water at 30.0 °C.

From the table, we see that the solubility of the solute at 20.0 °C is 44.3 g/100 g H₂O. This means that 51.0 g of water can dissolve:

(44.3 g solute / 100 g water) × (51.0 g water) = 22.6 g solute

at 20.0 °C.

Next, we can use the solubility at 30.0 °C to find out how much more solute can be dissolved in the remaining water at this temperature. From the table, we see that the solubility of the solute at 30.0 °C is 81.4 g/100 g H₂O.

This means that 100 g of water can dissolve 81.4 g of solute at 30.0 °C. To find out how much solute can be dissolved in the remaining water at 30.0 °C, we can set up the following proportion:

(81.4 g solute / 100 g water) = (x g solute / (100 - 51) g water)

where x is the amount of solute that can be dissolved in the remaining water at 30.0 °C.

Solving for x, we get:

x = (81.4 g solute / 100 g water) × (49.0 g water) = 39.9 g solute

Therefore, if the temperature is increased to 30.0 °C, an additional 39.9 g of solute can be dissolved in the remaining water, for a total of:

22.6 g + 39.9 g = 62.5 g solute in 100 g of water at 30.0 °C.

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The answer is A: Oil.

Answer:

Explanation:

A. Oil

hope it helps!

Answer:

Explanation:

100

m

L

H

+

 is required for complete neutralization.

Assuming, somehow, only

H

+

are in the buret and only

O

H

−

...

1 mg of BeSO₄ should be weighed out to prepare 1 L of 1 ppm Be⁺² solution.

The molar mass of BeSO₄ is:

BeSO₄ = Be + S + 4O

= 9.01 + 32.06 + (4 x 15.99)

= 9.01 + 32.06 + 63.96

= 105.03 g/mol

To prepare a 1 ppm solution of BeSO₄,  1 part of BeSO₄ per million parts of the solution. Since, preparing 1 L of solution, add 1 mg of BeSO₄ to the solution:

1 ppm = 1 mg/L

The number of moles of BeSO₄ required for 1 mg is:

n = m/M

n = 0.001 g / 105.03 g/mol

n = 9.52 x 10^-6 mol

To convert moles of BeSO₄ to grams, use the molar mass:

Mass = n x M

= 9.52 x 10^-6 mol x 105.03 g/mol

= 0.001 g or 1 mg

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Bile increases the surface area of the fats so that it can be digested. Option A

The liver produces bile, a greenish-yellow liquid that is kept in the gallbladder. It is critical for the small intestine's involvement in the breakdown of lipids.

Hormones tell the gallbladder to release bile into the duodenum, which is the first section of the small intestine, when food with fat enters the small intestine. Bile salts, which serve as emulsifiers, are found in bile.

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Freezing, condensation, and deposition are the phase changes that involve the release of energy.

The phase changes that involve the release of energy are exothermic processes, where energy is released from the system into the surroundings. The energy released can be in the form of heat, light, or sound, depending on the nature of the phase change.

Among the common phase changes, the ones that involve the release of energy are:

Freezing: The process of liquid water freezing into ice is an exothermic process, where energy is released in the form of heat.

Condensation: When water vapor condenses into liquid water, energy is released in the form of heat.

Deposition: When water vapor directly changes into solid ice without passing through the liquid phase, energy is released in the form of heat.

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Answer: A

Explanation:

The -ane suffix implies that the compound has only single bonds for carbon-carbon bonds. The but- prefix implies that the compound consists of four carbons. Since 4 bonds are required for each carbon, there will be a total of 10 hydrogen atoms: 3 on each carbon at the end of the chain and 2 for each carbon in the middle of the chain. Thus, butane is A.

The heat energy required to raise the temperature of the vapor q_total = q1 + q2 = 25.76 kJ + 84.39 J = 26.85 kJ.

The heat energy required to convert 66.3 g of liquid SO2 at 201.2 K to gaseous SO2 at 263.1 K is 26.85 kJ.

To solve this problem, we need to calculate the heat energy required to vaporize the given mass of liquid SO2 at its boiling point and then raise the temperature of the resulting vapor to the desired final temperature. The heat energy required for vaporization can be calculated using the molar heat of vaporization of SO2, which is given as 24.9 kJ/mol. The heat energy required to raise the temperature of the vapor can be calculated using the specific heat capacity of liquid SO2, which is given as 1.36 J/g K.

First, we need to calculate the number of moles of SO2 in 66.3 g of liquid SO2 using its molar mass. The molar mass of SO2 is 64.06 g/mol, so:

n = m/M = 66.3 g / 64.06 g/mol = 1.034 mol

The heat energy required for vaporization is then:

q1 = ΔHvap * n = 24.9 kJ/mol * 1.034 mol = 25.76 kJ

Next, we need to calculate the heat energy required to raise the temperature of the resulting vapor from 201.2 K to 263.1 K. The specific heat capacity of liquid SO2 is used because we are raising the temperature of the vapor from the boiling point of liquid SO2.

q2 = n * C * ΔT = 1.034 mol * 1.36 J/g K * (263.1 K - 201.2 K) = 84.39

The total heat energy required is the sum of the heat energy required for vaporization and the heat energy required to raise the temperature of the vapor:

q_total = q1 + q2 = 25.76 kJ + 84.39 J = 26.85 kJ

Therefore, the heat energy required to convert 66.3 g of liquid SO2 at 201.2 K to gaseous SO2 at 263.1 K is 26.85 kJ.

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Answer:

V=mass/Density

Explanation:

Since density is measured as grams/mL or grams/cm^3 and we are interested in converting mass to volume, we need to rewrite the equation.
Therefore, in order to convert the gram to mL, you just need to multiply the mass of the substance in grams with its density to get the volume in liters.

Answer:

Volume equals mass divided by density.

and

Mass equals density times volume.

Hope this helps :)

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The peak at m/z = 58 corresponds to the molecular ion, [M]

The peak at m/z = 43 corresponds to the fragment ion [M-15]

The peak at m/z = 29 corresponds to the fragment ion [M-29]

The peak at m/z = 15 corresponds to the fragment ion [M-43].

The two possible isomers for this molecule is:

iii)  The molecule is likely methylpropane.

The peaks in the mass spectrum are as follows:

Peak at m/z = 58: This corresponds to the molecular ion, [M], which has a mass of 58. This means that the entire molecule has been ionized and has a charge of +1.

Peak at m/z = 43: This represents the fragment ion [M-15], which has lost a methyl group (CH₃) from the molecular ion.

Peak at m/z = 29: This represents the fragment ion [M-29], which has lost a propyl group (C₃H₇) from the molecular ion.

Peak at m/z = 15: This represents the fragment ion [M-43], which has lost both a methyl group and a propyl group from the molecular ion.

There are two possible isomers for a hydrocarbon with the molecular formula C₄H₁₀:

Butane: CH₃CH₂CH₂CH₃

Methylpropane: CH₃CH(CH₃)CH₃

iii) Based on the relative intensities of the peaks at m/z = 43 and m/z = 29, the molecule is likely methylpropane.

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Subaquatic soil can be classified as sediment or soil based on its geological properties and formation processes.

Sediment refers to any material that is transported and deposited by water, wind, ice, or gravity. Sediments can be composed of various materials, such as minerals, rocks, organic matter, and even human-made debris.

Sediments can accumulate in different environments, such as rivers, lakes, oceans, and deserts, and can be deposited in layers over time.

Subaquatic soil can be classified as sediment or soil based on its geological properties and formation processes. If it has primarily formed through sediment deposition, it is more appropriate to classify it as sediment.

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Yes, a chemical reaction will take place if a bar of silver is placed into a solution containing [tex]Cu^{2+}[/tex] ions.

The reaction that will occur is a type of single replacement reaction. The silver metal will react with the copper ions in the solution, causing the copper ions to be reduced and the silver metal to be oxidized. The overall balanced chemical equation for this reaction is:

Ag(s) + [tex]Cu^{2+}[/tex](aq) → Cu(s) + [tex]Ag^+[/tex](aq)

In this equation, Ag represents silver, Cu represents copper, and the (s) and (aq) notations indicate solid and aqueous states, respectively. The arrow indicates the direction of the reaction.

As a result of this reaction, a thin layer of copper metal will be deposited onto the surface of the silver bar, while silver ions will enter the solution. This reaction is often used in electroplating applications, where a layer of one metal is deposited onto the surface of another metal.

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The amount of calcium carbonate in a 50.0g calcium carbonate is 0.5 moles while the amount of carbon in 88.0g propane is 72g.

The amount of a substance in moles can be calculated by dividing the mass of the substance by its molar mass as follows;

moles = mass ÷ molar mass

According to this question, there are 50.0 grams of calcium carbonate. The number of moles of the substance is;

moles = 50g ÷ 100g/mol = 0.5 moles

The amount of carbon in 88.0g propane can be calculated as follows;

36g ÷ 44g × 88 = 72g

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The relationship  between the density (d) of a gas and the rate at which the gas diffuses is r = k/√d.

option B.

Graham's law of diffusion, also known as Graham's law of effusion, states that the rate of diffusion or effusion of a gas is inversely proportional to the square root of its gas density.

In other words, lighter gases diffuse or effuse faster than heavier gases at the same temperature and pressure.

Mathematically, this law is written as;

r ∝ 1/√d

r = k/√d

where;

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The term molefraction is an important method which is used to calculate the concentration of a solution. It is mainly employed to calculate the concentration of a binary solution. Here the molefraction is 1 / 5. The correct option are D, D and B.

Molefraction of any component of a solution is defined as the ratio of the number of moles of that component to the total number of moles of the solution. The sum of molefraction of solute and solvent is one.

Here the molefraction of nitrogen = Moles of nitrogen / Total number of moles

1. 'x' of 'N' = 2 / 5 + 3 + 2 = 0.2 or 1 / 5

2. Molefraction of Argon = 0.60 / 0.40 + 0.04 + 0.60 = 0.57

Partial pressure = Molefraction × Total pressure

0.57 × 6.3 = 3.59 atm

3. 20 cm³ mixture contains:

20 × 1 mole / 22400 m³ = 8.9286 × 10⁻⁴

1 mole occupies 22400 cm³

8.9286 × 10⁻⁴ × 22400 cm³ / 1 mole = 20 cm³

Thus the correct option are D, D and B.

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The pressure of the helium gas (He) in the wet gas mixture is 833.8 mmHg.

In order to find the pressure of the helium gas in the wet gas mixture, we need to use the concept of partial pressures. According to Dalton's Law of Partial Pressures, the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas present in the mixture. In this case, the wet gas mixture contains helium (He) and water vapor (H2O). The pressure of water vapor (H2O) is given as 21.2 mmHg, which means that the partial pressure of water vapor (H2O) in the mixture is 21.2 mmHg. We can now use the total pressure and the partial pressure of water vapor (H2O) to find the partial pressure of helium (He) in the mixture. To do this, we can subtract the partial pressure of water vapor (H2O) from the total pressure:

Partial pressure of helium (He) = Total pressure - Partial pressure of water vapor (H2O)

Partial pressure of helium (He) = 855 mmHg - 21.2 mmHg

Partial pressure of helium (He) = 833.8 mmHg

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