What is the molarity of the solution made by dissolving a 5.67 g of potassium chloride in enough water to make 100 mL of the solution

Hydrochloric acid (HCl) is a strong acid that fully dissociates in an aqueous solution, meaning it releases all of its hydrogen ions, making the solution highly acidic. Unlike weak acids, it does not create a buffered solution when reacted with a strong base. Adding HCl to a solution typically lowers the pH level due to the increase in hydrogen ion concentration.

A strong acid like HCl (hydrochloric acid) fully dissociates in an aqueous solution. This essentially means that virtually every HCl molecule that dissolves in water will undergo a reaction; donating H* (hydrogen ions) and becoming highly acidic. Acids that react completely in this way are known as strong acids.

Conversely, a weak acid does not fully dissociate in solution and some of its hydrogen ions remain bonded within the compound. For instance, acetic acid, the main component in vinegar is a weak acid.

When HCl reacts with a strong base, it can produce a salt and water, but it does not create a buffered solution. It's also important to note that adding a strong acid to an aqueous solution usually lowers (not raises) the pH due to the increase in hydrogen ion concentration.

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When reporting the mass of the NaCl sample, consider the number of significant figures. The precision of the measurement equipment determines the appropriate number of significant figures to report.

When reporting the measurement of the mass of the NaCl sample, you should consider the significant figures. Significant figures are the digits in a number that carry meaning and contribute to its precision. In general, you should report your measurement to the same number of significant figures as the least precise measurement involved in the calculation.

In the given question, there is no specific information provided about the NaCl sample and the precision of the measurement. Therefore, it is not possible to determine the accurate number of significant figures to report. However, it is important to determine the precision of the equipment used to measure the mass and report the measurement accordingly.

To achieve a 60-gallon mixture with an octane rating of 120, the student should use 20 gallons from the tank with an octane rating of 80.

The student's question involves calculating the amount of gasoline to use from each tank to create a mixture with a desired octane rating. This is a problem that can be solved using the concept of weighted averages. Here, we need to find the number of gallons of gas with an octane rating of 80 to mix with gas with an octane rating of 140 to achieve a final mixture of 60 gallons with an octane rating of 120.

Let the amount of gasoline used from the tank with octane rating 80 be x gallons, and hence the amount used from the tank with octane rating of 140 will be (60 - x) gallons. We can write the following equation based on the weighted average of octane ratings:

80x + 140(60 - x) = 120(60)

Solving the equation:

Multiply out the terms: 80x + 8400 - 140x = 7200.

Combine like terms: -60x + 8400 = 7200.

Subtract 8400 from both sides: -60x = -1200.

Divide both sides by -60: x = 20.

So, the student should use 20 gallons from the tank with an octane rating of 80 to obtain a 60-gallon mixture with an octane rating of 120.

Answer:

Buoyant force has to be greater than the weight of the object

Explanation:

According to Archimedes principle, the upward buoyant force is equal to the weight of the liquid displaced if an object is fully or partially immersed in a liquid. When an object is immersed in water, two forces act on it :

1. Buoyant force or upthrust, an upward force, which opposes the weight of an object inside water.          

2. Gravitational force, which act in downward direction always.

The floating or sinking of an object depend on the amount of buoyant force. If the buoyant force is greater than the weight of the object, it will float and if the buoyant force is less than the weight of the object, it will sink in liquid.

Hence, the correct option is (c) " buoyant force has to be greater than the weight of the object".

Answer : The correct option is, [tex]6.0\times 10^{-5}M[/tex]

Explanation :  Given,

pOH = 4.22

pOH : It is defined as the negative logarithm of hydroxide ion concentration.

Now we have to calculate the [tex]OH^-[/tex] concentration.

Formula used :

[tex]pOH=-\log [OH^-][/tex]

Now put all the given values in this formula, we get the concentration of hydroxide ion.

[tex]4.22=-\log [OH^-][/tex]

[tex][OH^-]=6.0\times 10^{-5}M[/tex]

Therefore, the [tex]OH^-[/tex] concentration is, [tex]6.0\times 10^{-5}M[/tex]

After three half-lives, 12.5% of the original radioactive parent isotope will remain.

To determine the remaining amount of a radioactive parent isotope after a given number of half-lives, you need to understand the concept of radioactive decay.

A radioactive isotope undergoes decay, reducing its quantity over a set period known as a half-life.

Each half-life represents the time it takes for half of the parent isotope to decay into a daughter isotope.

Explanation and Calculation:

1. Concept of Half-Life:

- A half-life is the time required for half of the radioactive parent isotope to decay.

2. Formula for Remaining Fraction:

- The fraction of the parent isotope remaining after n half-lives can be calculated using the formula:

[tex]\[ \left(\frac{1}{2}\right)^n \][/tex]

- Here, n is the number of half-lives.

3. Calculation for Three Half-Lives:

[tex]\text{After 1 half-life:} \\\\\left(\frac{1}{2}\right)^1 = \frac{1}{2} = 0.5 \text{ (50\% remains)}\\\text{After 2 half-lives:} \\\\\left(\frac{1}{2}\right)^2 = \frac{1}{4} = 0.25 \text{ (25\% remains)}\\\text{After 3 half-lives:} \\\\\left(\frac{1}{2}\right)^3 = \frac{1}{8} = 0.125 \text{ (12.5\% remains)}[/tex]

Conclusion:

Thus, after three half-lives, only 12.5% of the original parent isotope remains. This is calculated using the formula [tex]\(\left(\frac{1}{2}\right)^n\)[/tex], where n is the number of half-lives.

The solution with a higher concentration of hydroxide ions (oh-) than hydrogen ions (h+) are base solutions or solutions which are the basic  option B is correct.

A solution which is basic in nature in  aqueous solution  they contain   more OH - ions concentration than that of H + ions concentration. that is they are, in  aqueous solution with a pH greater than 7.

Basic solutions contain ions, with some  conducted  electricity, and it turn red litmus paper blue, and slippery while touching.

They are mostly used in the manufacturing of soaps, toothpaste, paper and rayon as they do not react with skin due to basic in nature.

Basic substances react to aqueous solutions by accepting or gaining of  protons, giving away or releasing the  electrons, or releasing and make free hydroxide ions.

Therefore, they are basic solutions. option B is correct

Learn more about basic solutions, here ;

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The given question is incomplete therefore, the complete question is

a solution with a higher concentration of hydroxide ions (oh-) than hydrogen ions (h+)

A.acid

B. base

C.neutral

The number of molecules resulting from a chemical reaction depends on the balanced chemical equation, which is not provided for the ethanol combustion. We would need this to determine the exact quantities of CO2, H2O, and O2 produced from the reaction involving ethanol.

To determine the number of molecules present after a chemical reaction has gone to completion, we use the balanced chemical equations. However, the initial question does not provide a complete balanced equation for the reactions involving CO2, H2O, C2H5OH (ethanol), and O2 (oxygen). We are provided information about the combustion of methane and the reaction of propane but not the specific reaction for ethanol, which is necessary to determine the exact number of molecules produced in its combustion.

Given the example of the propane combustion, which yields 3 moles of CO2 and 4 moles of H2O from 0.75 mol of propane, we can extend this stoichiometric ratio to determine the number of molecules. The number of molecules produced from the combustion of a known quantity of another substance, like ethanol, would depend on its stoichiometry. Without the balanced equation for ethanol combustion, we cannot calculate the exact quantities of CO2, H2O, and O2 produced. Therefore, the student should provide the complete balanced chemical equation or clarify if the question is about a different reaction than the ones provided.

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The element with an atomic number lower than aluminum and one less valence electron than the Group 16 elements is magnesium, which has an atomic number of 12 and two valence electrons.

The element you're referring to that possesses an atomic number lower than that of aluminum and one less valence electron than the Group 16 elements is magnesium. Magnesium has an atomic number of 12, which is less than that of aluminum (13), and it falls under group 2 (the alkaline earth metals) in the periodic table. Group 16 elements, also known as chalcogens, typically have six valence electrons. Therefore, with magnesium possessing two valence electrons, it has one less than the Group 16 elements if we consider the full shell configuration.

The atomic number signifies the number of protons in an atom's nucleus, providing a key characteristic of an element's identity. In the case of magnesium, this number is 12.

Concerning valence electrons, they are the electrons present in an atom's outer shell and primarily engage in bonding with other atoms. For magnesium, there are two valence electrons.

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Answer:

522.2kJ

Explanation:

Hello,

In this case, based on the given conversion data, we apply the following proportional factor to obtain the corresponding energy in kJ:

[tex]125cal*\frac{4.18kJ}{1cal}=522.2kJ[/tex]

Best regards.

There are [tex]6.12 \times 10^{23}[/tex] atoms of oxygen in 30.5 grams of glucose. There is a little over one mole of oxygen in the given mass of glucose, therefore the number of O atoms should be a little over Avogadro's number.

FURTHER EXPLANATION

To get the number of atoms present in 30.5 g of glucose the following steps must be done:

STEP 1: Convert 30.5 g glucose to moles by dividing the given mass by the formula mass (molar mass).

The molar mass of glucose is 180.156 g/mol obtained as follows:

[tex]formula \ mass \ C_6H_{12}O_6 \ = (6)(12.011) \ + \ (12)(1.008) \ + \ (6)(15.999)\\\boxed {formula \ mass \ C_6H_{12}O_6 \ = 180.156}[/tex]

The mass of 1 mol of glucose is equal t its formula mass in g.

Next, set up the equation below to convert the mass of glucose to moles of glucose.

[tex]moles \ C_6H_{12}O_6 \ = 30.5 \ g (\frac{1 \ mol}{180.156 \ g})\\\\\boxed { moles \ C_6H_{12}O_6 \ = 0.1693 \ mol}[/tex]

STEP 2: Determine how many  moles of oxygen are in the given moles of glucose. The subscripts of the elements in the chemical formula will give the mole ratio: 1 mole of glucose has 6 moles of oxygen atoms.

[tex]moles \ of \ O \ = 0.1693 \ mol \ C_6H_{12}O_6 \ (\frac{6 \ mol \ O}{1 \ mol \ C_6H_{12}O_6})\\\boxed {moles \ of \ O \ = 1.0158 \ mol}[/tex]

STEP 3: Use Avogadro's number to calculate the number of atoms of O

1 mol of O has [tex]6.022 \times 10^{23}[/tex] O atoms

[tex]no. \ of \ O \ atoms \ = 1.0158 \ mol \ O \ \times \frac{6.022 \times 10^{23} \ atoms \ O}{1 \ mol \ O} \\\boxed {no. \ of \ O \ \ atoms \ = 6.117 \times 10^{23} \ atoms}[/tex]

Since the given, 30.5 g has 3 significant figures, the final answer must also have 3 significant figures. Therefore,

[tex]\boxed {atoms \ of \ O \ = 6.12 \times 10^{23} \ atoms}}[/tex]

LEARN MORE

Keywords: moles, Avogadro's number

Answer:

The emission of free carriers or electrons taking place when light falls into a substance is termed as the photoelectric effect. On the basis of the Rutherford model, the light of any energy should possess the tendency to cause the electrons to leave the atom and get emitted.  

The energy obtained from the emitted electrons should be associated with the intensity of the light. However, the energy of the electron is in the real sense only associated with the energy of the light.  

Answer: b

Explanation:

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In the reaction of magnesium metal with hydrochloric acid to produce hydrogen gas and aqueous magnesium chloride, increasing the pressure would not significantly affect the reaction rate, as solids and liquids are not compressible under moderate pressure changes.

The effect of an increase in pressure on the reaction of magnesium metal with a solution of hydrochloric acid (Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq)) depends on the reaction conditions. If this system is at chemical equilibrium—where the rate of the forward reaction is equal to the rate of the reverse reaction—and involves gases, increasing the pressure will favor the direction in which there are fewer moles of gases. According to Le Chatelier's Principle, because the reactant side has solid magnesium and aqueous HCl, while the product side has gaseous hydrogen and aqueous magnesium chloride, increasing the pressure would shift the equilibrium to the left, potentially reducing the rate of the forward reaction.

However, this reaction is not typically presented as an equilibrium in introductory chemistry, and the scenario doesn't imply it is reversible under normal conditions. Therefore, in practice, the reaction rate of a solid and liquid reactant generating gas is usually unaffected by external pressure changes because solids and liquids are not compressible under moderate pressure changes. Thus, the reaction rate is mostly influenced by the surface area of the magnesium, the molarity of the hydrochloric acid, and the temperature of the solution.

Answer: Option (c) is the correct answer.

Explanation:

It is necessary to take precautions while performing an experiment in a laboratory. This is because safety measures in the laboratory can prevent any serious injury.

For example, when accidentally an acid spills on Celia's hand then it is important to inform the teacher about it while Celia washes her arm with soap and water.

Also, when doing an experiment or dealing with acids the we should be wearing lab coat, safety goggles, closed shoes and safety gloves.

Thus, we can conclude that out of the given options, Lee should tell the teacher while Celia washes her arm with soap and water, this should be done next.

Answer: The molar mass of the gas is 2.02 grams.

Explanation:

We are given:

Density of gas = 0.0902 g/L

At STP conditions:

1 mole of gas occupies 22.4 L of volume

And 1 mole of a substance is known as the molecular mass or molar mass of that substance.

To calculate the mass of gas, we use the equation:

[tex]\text{Density of gas}=\frac{\text{Mass of gas}}{\text{Volume of gas}}[/tex]

Putting values in above equation, we get:

[tex]0.0902g/L=\frac{\text{Mass of gas}}{22.4L}\\\\\text{Mass of gas}=2.02g[/tex]

Hence, the molar mass of the gas is 2.02 grams.

The molar mass of an ideal gas can be calculated by multiplying its density (given as 0.0902 g/L) by the molar volume of gas at STP (which is 22.4 L/mol). This gives us a molar mass of approximately 2.02 g/mol.

For an ideal gas at Standard Temperature and Pressure (STP), which is 0°C (273.15K) and 1 atm, one mole of the gas occupies a volume of 22.4 L. This is a well-known fact. Now, molar mass is the mass of one mole of a substance. You're given the density of the gas (0.0902 g/L).

We can use this known volume of a mole of gas at STP and the given density to find the molar mass. The formula to do that would be: Molar mass = Density x Molar volume.

Substitute the values into this equation:

Molar mass = 0.0902 g/L x 22.4 L/mol

Molar mass = 2.02 g/mol

Therefore, the molar mass of the gas is approximately 2.02 g/mol.

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