The solubility of aluminum hydroxide at 25°C is approximately 2.8 x 10⁷ g/L (option d).
1: The solubility product constant (Ksp) equation for aluminum hydroxide (Al(OH)₃) is:
Ksp = [Al³⁺][OH⁻]₃
When Al(OH)₃ dissolves, it forms one Al³⁺ ion and three OH⁻ ions. Therefore, [Al³⁺] = s and [OH⁻] = 3s.
Ksp = (s)(3s)³
4.6 x 10⁻³³ = s(27s³)
2: Divide by 27:
s⁴ = (4.6 x 10⁻³³)/27
3: Take the fourth root:
s = (4.6 x 10⁻³³/27)^(1/4)
s = 1.8 x 10⁻⁸ mol/L
4: Now, we need to convert the solubility from mol/L to g/L:
1.8 x 10⁻⁸ mol/L * (26.98 g/mol Al + 3 * 15.999 g/mol O + 3 * 1.007 g/mol H) = 2.8 x 10⁻⁷ g/L
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draw a dash-wedge structure for (2r,4s)-2,4-dibromo-2-chloropentane.
To draw the dash-wedge structure for (2R,4S)-2,4-dibromo-2-chloropentane, we first need to understand the stereochemistry of the molecule.
The prefix (2R,4S) tells us that the two bromine atoms are on the same side (cis) of the molecule, while the chlorine atom is on the opposite side (trans).
Now, let's draw the structure:
1. Start with the structure of pentane:
CH3CH2CH2CH2CH3
2. Replace one of the hydrogen atoms on the second carbon with a chlorine atom:
CH3CH(Cl)CH2CH2CH3
3. Next, we need to add the two bromine atoms, which are both on the same side (cis) of the molecule. We'll add them to carbons 2 and 4:
CH3CH(Cl)CH(Br)CH2(Br)CH3
4. Finally, we need to assign the stereochemistry. Since the bromine and chlorine atoms are both attached to chiral carbons (carbons 2 and 4), we need to use dashes and wedges to show their orientation in 3D space.
The chlorine atom is on the opposite side (trans) of the molecule, so we draw it as a wedge:
Cl
|
CH3C---H
|
CH2
|
CH3C---H
The two bromine atoms are on the same side (cis) of the molecule, so we draw them as dashes:
Br
|
CH3C---H
|
CH(Br)
|
CH3C---H
I hope this helps! Let me know if you have any other questions.
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which compound has only ionic bonds co2 al2o3 h2o2
The compound with only ionic bonds is Al₂O₃.
Ionic bonds occur between metals and non-metals, where electrons are transferred from the metal to the non-metal. In the given compounds, CO₂ has covalent bonds as both carbon and oxygen are non-metals.
H₂O₂ also has covalent bonds since hydrogen and oxygen are both non-metals. However, Al₂O₃ has ionic bonds as aluminum (Al) is a metal, and oxygen (O) is a non-metal.
The aluminum atoms lose electrons to the oxygen atoms, forming positively charged Al³⁺ ions and negatively charged O²⁻ ions. These ions then attract each other, forming the ionic compound Al₂O₃.
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Which salt would form an acidic solution when dissolved in water? The Ka of NH: is 5.6 × 10-10 and the Kb of CN-is 1.6×10- Select the correct answer below ○ NH,CN O Naci O NH, Br O More than one solution will be acidic.
The salt that would form an acidic solution when dissolved in water is NH₄CN.
Why would NH₄CN form an acidic solution when dissolved in water?NH₄CN consists of the ammonium ion (NH⁴⁺) and the cyanide ion (CN⁻). NH⁴⁺ is the conjugate acid of NH₃ (ammonia. Ammonia is commonly recognised as a weak base. CN⁻ is the conjugate base of HCN (hydrogen cyanide), which is a weak acid.
The Ka of NH⁴⁺ is 5.6 × 10-10, which means that NH⁴⁺ is a weak acid. The Kb of CN⁻ is 1.6 × 10-5, which means that CN⁻ is a weak base.
When NH₄CN is dissolved in water, NH⁴⁺ can donate a proton to water to form H3O⁺ (hydronium ion) and NH₃, making the solution acidic.
Therefore, NH₄CN would form an acidic solution when dissolved in water.
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what is the ph of a 0.0005m solution of (amphetamines)2so4(aq) at 25 ºc if the kb of amphetamine is 1.3 x 10–4?
The pH of a 0.0005 M solution of (amphetamines)₂SO₄(aq) at 25°C is approximately 6.89.
To find the pH of a 0.0005 M solution of (amphetamine)₂SO₄(aq) at 25°C, we need to first determine the concentration of the amphetamine ion, then use the Kb value to find the concentration of H₃O⁺ ions, and finally calculate the pH.
1. Determine the concentration of amphetamine ion:
In (amphetamine)₂SO₄, there are 2 amphetamine ions for every 1 sulfate ion. So, the concentration of amphetamine ions is 2 * 0.0005 M = 0.001 M.
2. Use the Kb value to find the concentration of H₃O⁺ ions:
Kb = [H₃O⁺][A⁻]/[AH]
Where A⁻ is the conjugate base of amphetamine and AH is the protonated amphetamine.
Rearranging the equation for [H₃O⁺]:
[H₃O⁺] = Kb * [AH]/[A⁻]
Since [AH] = [A⁻] (due to the stoichiometry of the reaction), we can simplify the equation:
[H₃O⁺] = Kb * [AH]
Now, we can plug in the values:
[H₃O⁺] = (1.3 x 10⁻⁴) * 0.001 M = 1.3 x 10⁻⁷ M
3. Calculate the pH:
pH = -log10[H₃O⁺]
pH = -log10(1.3 x 10⁻⁷) ≈ 6.89
Therefore, the pH of the 0.0005 M solution of (amphetamine)₂SO₄(aq) at 25°C is approximately 6.89.
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When we are on an airplane above the clouds, why does it look like we're passing up each cloud very slowly even though we're going about 500 mph?
Answer:
When we are on an airplane above the clouds, it can appear as if we're passing each cloud slowly because there is no frame of reference to judge our speed. Our eyes can't detect any movement on the ground, and there are no other objects in the sky to provide a sense of speed or motion. Additionally, clouds are often quite large, so it can take several minutes to pass over one even at high speeds. This can create the illusion that we're moving slowly, even though we're actually traveling at several hundred miles per hour. Our brains are not accustomed to seeing objects at such a high altitude and speed, so it can be difficult to accurately judge our motion relative to the clouds.
A precipitation reaction occurs when a solution of potassium carbonate is reacted with aqueous magnesium chloride. Write a balanced total molecular equation for this reaction. Identify the spectator ions in the reaction. Write a balanced net ionic equation for the reaction. Be sure to include states of matter.
The total molecular equation for the precipitation reaction between a solution of potassium carbonate and aqueous magnesium chloride is: K₂CO₃(aq) + MgCl₂ (aq) → MgCO₃ (s) + 2KCl (aq).
The spectator ions in this reaction are K+ and Cl-. The net ionic equation for the reaction is: Mg²+ (aq) + CO₃2- (aq) → MgCO₃ (s).
The reaction involves the precipitation of magnesium carbonate, which is the solid product of the reaction. This occurs when the anion of one reactant, carbonate, is combined with the cation of the other reactant, magnesium.
The spectator ions, which are ions that do not directly participate in the reaction, are K+ and Cl-, which come from the potassium carbonate and magnesium chloride, respectively. The net ionic equation shows the actual reaction taking place between the magnesium cation and the carbonate anion.
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Describe how to prepare 100 ml of 0.200 m acetate buffer, ph 5.00, stating with pure liquid acetic acid and solutions containing 3m hcl and 3mnaoh
To prepare 100 mL of 0.200 M acetate buffer with a pH of 5.00, you'll need to mix appropriate amounts of acetic acid, 3 M HCl, and 3 M NaOH.
1. Calculate the required moles of acetate buffer: 0.200 M * 0.100 L = 0.020 moles.
2. Determine the ratio of acetic acid (CH₃COOH) to sodium acetate (CH₃COONa) using the Henderson-Hasselbalch equation: pH = pKa + log ([CH₃COONa] / [CH₃COOH]). The pKa of acetic acid is 4.74.
3. Calculate the required moles of CH₃COOH and CH₃COONa using the ratio from step 2.
4. Mix the required moles of CH₃COOH with an appropriate amount of 3 M HCl or 3 M NaOH to convert it into CH₃COONa.
5. Adjust the final volume to 100 mL with distilled water.
By following these steps, you'll create 100 mL of 0.200 M acetate buffer at a pH of 5.00 using pure liquid acetic acid, 3 M HCl, and 3 M NaOH.
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a 36.0 g sample contains 14.6 g cl and 21.4 g b. what is the percent composition of boron in this sample?
In the sample provided, boron makes up 59.4% of the total makeup.
What percentage of this sample contains boron?
We must first determine the overall mass of the sample and then the mass of boron in the sample in order to determine the percent composition of boron in the given sample.
Sample mass overall is 36.0 g.
Chlorine mass in the sample is 14.6 g.
The sample's boron weight is 21.4 g.
As a result, the sample's boron content can be determined using the formula:
% composition of boron is calculated as follows: (mass of boron / total mass of sample) x 100%; (21.4 g / 36.0 g) x 100%; % composition of boron = 0.594 x 100%; and % composition of boron = 59.4%
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Equation for free energy change associated with transport across a concentration gradient when a species is charged
The equation ΔG = RTln(C2/C1) + zFΔψ is commonly known as the Nernst equation and is used to calculate the free energy change associated with transport of a charged species across a membrane.
The Nernst equation for free energy change associated with transport across a concentration gradient when a species is charged is given by ΔG = RTln(C2/C1) + zFΔψ, where ΔG is the change in free energy, R is the gas constant, T is the temperature, C1 and C2 are the concentrations of the species on either side of the membrane, z is the charge of the species, F is the Faraday constant, and Δψ is the membrane potential. This equation takes into account both the concentration gradient and the electrical potential across the membrane, and shows that transport of a charged species is dependent on both factors. The concentration gradient is the difference in the concentration of the species on either side of the membrane. If the concentration of the species is higher on one side of the membrane than the other, then the species will tend to move from the side of higher concentration to the side of lower concentration. This movement of the species is known as diffusion.
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Which one of the following species will have a negligible effect on the pH of an aqueous solution? A. Bro B. CI- C. NH" D. CO32- E. CH3C00
The species that will have a negligible effect on the pH of an aqueous solution is CI⁻ (chloride ion). The correct answer is option B.
Chloride ion (Cl⁻) is a conjugate base of a strong acid (HCl), and therefore it is a very weak base. In an aqueous solution, Cl⁻ ion does not readily accept protons (H⁺ ions) from water molecules, and it does not affect the pH of the solution to a significant extent.
On the other hand, the other species listed are either weak bases or weak acids that can affect the pH of the solution to varying degrees.
NH3 is a weak base that can react with water to form NH₄⁺ and OH⁻ ions, and thereby increase the pH of the solution. CO₃²⁻ is a strong base that can accept protons from water molecules to form HCO³⁻ and OH⁻ ions, and thereby increase the pH of the solution. CH₃COO⁻ is a weak acid that can donate protons to water molecules to form H₃O⁺ and acetate ions, and thereby decrease the pH of the solution. Br⁻ is a weaker base than NH³ but still more basic than Cl⁻. Therefore, it can also affect the pH of the solution to some extent, although to a lesser extent than NH₃ or CO₃²⁻.Therefore option B is correct.
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A balloon is inflated to 665 mL volume at 27°C. It is then cooled down to -78.5°C. What
is its volume, assuming the pressure remains constant?
Answer:
431 mL
Explanation:
This is a question about the relationship between the volume and temperature of a gas. The volume of a gas is directly proportional to its temperature in kelvins when the pressure is held constant. This relationship is described by Charles’s Law.
To solve this problem, we need to convert the temperatures from degrees Celsius to kelvins by adding 273.15. So 27°C is equivalent to 300.15 K and -78.5°C is equivalent to 194.65 K.
Let’s call the initial volume of the balloon V1 and its initial temperature T1. The final volume of the balloon will be V2 and its final temperature T2. According to Charles’s Law, the relationship between these variables can be expressed as:
V1/T1 = V2/T2
Substituting the known values into this equation, we get:
665 mL / 300.15 K = V2 / 194.65 K
Solving for V2, we find that the final volume of the balloon is approximately 431 mL.
Select the route that would most likely produce the desired results from the given starting material. Br I. () H2SO4 and heat;(2) HBr II. (1) KOH in ethanol: (2) HBr II. (1)H SO4 and heat: (2) HBr+ peroxides IV. (1) potassium tert-butoxide in tert-butanol; (2) HBr+ peroxides A) I B) II C) IIID. IV
The desired product is HBr, and it can be obtained from Br2 using different methods.
what the route that would most likely produce the desired results from the given starting material? A: Br2 + H2SO4 and heatThis reaction does not produce HBr. Instead, it produces SO2, Br2, and H2O. Therefore, this route would not produce the desired results.
B: Br2 + KOH in ethanolThis reaction produces KBr and H2O, but not HBr. Therefore, this route would not produce the desired results either.
Option D, which involves the use of potassium tert-butoxide in tert-butanol and HBr with peroxides to produce HBr from Br2
C: Br2 + H2SO4 and heat + peroxidesThis reaction produces HBr, but it can be hazardous because peroxides can cause an explosive reaction. Therefore, this route is not recommended unless the peroxides are handled with caution.
D: Br2 + potassium tert-butoxide in tert-butanol + HBr + peroxidesThis reaction produces HBr and is a reliable method for obtaining it. However, it also involves the use of peroxides, which can be hazardous.
Overall, the most suitable route for obtaining HBr from Br2 is Option D, using potassium tert-butoxide in tert-butanol and HBr with peroxides. It is essential to handle the peroxides with caution and follow proper safety procedures to avoid accidents.
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he reaction: 2 n2o5(g) 4 no2(g) o2(g), is first order in n2o5(g). when [n2o5(g)] = 0.025 m, the rate is 7.2 x 10-4 m/min. how long will it take for the rate to drop to 3.6 x 10-4 m/min?
The time will it take for the rate to drop to 3.6 x 10⁻⁴ m/min is given by the time t = 24.1 min.
The pace at which reactants change into products is known as the rate of reaction or reaction rate. It goes without saying that the pace at which chemical reactions take place varies greatly. While certain chemical reactions occur almost instantly, others often take time to achieve their ultimate equilibrium.
This page seeks to educate readers on and clarify the concept of the rate of reaction for a particular chemical molecule.
2N₂O₅(g) → 4NO₂(g) + O₂(g)
2N₂O₅(g) = 0.025M : rate = 7.2 x 10⁻⁴ M/min.
To get rate = 3.6 x 10⁻⁴ M/min how much time
[tex]-r_A=k[N_2O_5][/tex]
7.2 x 10-4 = k x 0.025
k = 288 x 10⁻⁴ min
For rate = 3.6 x 10⁻⁴
288 x 10⁻⁴ [Ca] = 3.6 x 10⁻⁴
Ca = 0.0125 M
[tex]kC_A=-\frac{dC_A}{dt}[/tex]
[tex]C_A=[C_A_o](1-e^{-kt})[/tex]
0.0125 = 0.025([tex]1-e^{-kt}[/tex])
0.5 = [tex]1-e^{-kt}[/tex]
t = 0.693/k
t = 24.1 min
t = 0.693/(288 x 10⁻⁴)
t = 24.1 min.
Therefore, the required time is 24.1 min.
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What is the proeutectoid phase for an iron–carbon alloy in which the mass fractions of total ferrite and total cementite are 0.90 and 0.1, respectively?
The proeutectoid phase for an iron-carbon alloy with mass fractions of 0.90 total ferrite and 0.10 total cementite is ferrite.
To explain, in an iron-carbon alloy system, the proeutectoid phase is the phase that forms before the eutectoid reaction occurs. The eutectoid reaction happens at 0.76 wt% carbon in the iron-carbon phase diagram.
In this specific alloy, the mass fractions are 0.90 total ferrite and 0.10 total cementite, which means that the alloy has a lower carbon content compared to the eutectoid composition (less than 0.76 wt% carbon).
Since ferrite is the stable phase at lower carbon concentrations, the proeutectoid phase for this alloy is ferrite. The microstructure will mainly consist of ferrite, with some small amounts of cementite dispersed within it.
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what is the ph of a 0.01 m solution of hbf4 , pka = −9. clearly show all your work or reasoning and put a box around your answer.
Hydrogen tetrafluoroborate (HBF4) is a strong acid with a pKa of -9. This means that in water, it will donate a proton to form the hydronium ion (H3O+). To find the pH of a 0.01 M solution of HBF4,
we need to calculate the concentration of H3O+ ions. HBF4 → H+ + BF4- Let x be the concentration of H+ ions produced in the solution.
[tex][H+][BF4-]/[HBF4] = Ka[H+][BF4-]/(0.01) = 10^-9[H+][BF4-] = 10^-11[/tex]
Since HBF4 dissociates completely, the concentration of H+ ions is equal to the concentration of HBF4. Therefore:
[tex][H+] = [HBF4] = 0.01 MpH = -log[H+]pH = -log(0.01)pH = 2[/tex]
Therefore, the pH of a 0.01 M solution of HBF4 is 2.
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Write a Lewis structure and identify the octet-rule exception for each of the following: (select "expanded octet" or "electron deficient octet")
A. PF6LaTeX: -
B. ClO3
C. H3PO3
D. O3LaTeX: -
E. XeF2
The octet rule in chemistry asserts that in order to have an entire outer shell of eight electrons, atoms tend to obtain, lose, or share electrons.
However, there are some cases where this rule does not apply, resulting in compounds with an expanded or electron deficient octet.
A. [tex]PF_{6}[/tex]- has an expanded octet since the central phosphorus atom is bonded to six fluorine atoms, and has a total of 12 valence electrons in its valence shell.
B. [tex]ClO_{3}[/tex]- also has an expanded octet, as the central chlorine atom is bonded to three oxygen atoms and has a total of 10 valence electrons in its valence shell.
C. [tex]H_{3} PO_{3}[/tex]-has an electron deficient octet, as the central phosphorus atom is bonded to only three atoms and has a total of 10 valence electrons in its valence shell.
D. [tex]O_{3}[/tex]- has an electron deficient octet, as each oxygen atom is bonded to two other oxygen atoms, resulting in a central oxygen atom with only six valence electrons in its valence shell.
E. [tex]XeF_{2}[/tex] has an electron deficient octet, as the central xenon atom is bonded to two fluorine atoms and has a total of eight valence electrons in its valence shell.
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consider the titration of 30 ml of 0.45 m hi with 0.75 m rboh. a. what is the ph at the equivalence point? b. what is ph after 5 ml of rboh has been added?
bThe salt sodium formate can be found at the equivalency point. At pH 7.0, a strong acid or base will titrate to their equivalent point. Although the pH at the equivalence point is larger or lower than 7.0 in titrations of weak acids or bases, respectively.
The solution's pH will be (log 5 0.7CH3COOH = 4.76), which is the equivalency point. 0.200 M HBr, a potent acid, serves as the titrant. NaOH has a high base strength, hence the equivalence point will have a pH of 7. As a result, pH = 7 and H = 7.When 0.100M hydroxyacetic acid and 0.0500M KOH are titrated, the pH at the equivalence point is 8.18.
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Use the bond energies in Table 7.2 to calculate the standard enthalpy change (∆H∘) of the following reaction. Your answer should be kJ. a. Cl2(g)⟶2Cl(g) b. 2N(g)⟶N2(g) c. CH4(g)+Cl2(g)⟶CH3Cl(g)+HCl(g) d. CH4(g)+2H2O(g)⟶4H2(g)+CO2(g)
Using the bond energies to calculate the standard enthalpy change (∆H₀) of the following reaction are:
Cl₂(g)⟶2Cl(g) ∆H₀ = 4.02 x 10⁻²² 2N(g)⟶N₂(g) ∆H₀ = 15.64 x 10⁻²²CH₄(g)+Cl₂(g)⟶CH₃Cl(g)+HCl(g) ∆H₀ = - 1.727 x 10⁻²²CH₄(g)+2H₂O(g)⟶4H₂(g)+CO₂(g) ∆H₀ = -6.37 x 10⁻²².Bond Energy, commonly referred to as average bond enthalpy or just bond enthalpy, is a measurement that provides information about how strong a chemical bond is. "The average value obtained from the bond dissociation enthalpies (in the gaseous phase) of all the chemical bonds of a particular type in a given chemical compound," is how the word "bond energy" is defined by the IUPAC. As a result, the average amount of energy needed to break one of these chemical bonds may be thought of as the bond energy of a chemical bond in a specific molecule.
a) Cl₂(g)⟶2Cl(g)
∆H₀ = ( 242 kJmol-1)/Na = 4.02 x 10⁻²²
b) 2N(g)⟶N₂(g)
∆H₀ = ( 942 kJmol-1)/Na = 15.64 x 10⁻²²
c) CH₄(g)+Cl₂(g)⟶CH₃Cl(g)+HCl(g)
∆H₀ =(413+242-328-431)/Na = -1.727 x 10⁻²²
d) CH₄(g)+2H₂O(g)⟶4H₂(g)+CO₂(g)
∆H₀ =(( 4*413)+(4*463)-(4*436)-(2*1072))/Na = -6.37 x 10⁻²².
It is essential to remember that the average value of each chemical bond's individual bond dissociation enthalpies constitutes the bond energy of a chemical bond inside a molecule. The average of the bond dissociation energies of each individual carbon-hydrogen bond, for instance, determines the bond energy of the carbon-hydrogen bond in the methane (CH4) molecule.
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Rank the following compounds in order of increasing strength of intermolecular forces. HF
HCI
H2
F2 Select one:
(A) H2 < HCI < HF < F2
(B) HF < F2 < HCI < H2
(C) H2< F2 < HCI < HE
(D) HCI < HF < < F2 < H2
Compounds in order of increasing strength of intermolecular forces H2 < HCI < HF < F2
The strength of intermolecular forces depends on the type of forces present. Hydrogen bonds are the strongest, followed by dipole-dipole interactions, and then London dispersion forces. H2 and F2 have nonpolar covalent bonds, so they only exhibit London dispersion forces. Since H2 has a smaller molar mass than F2, it has weaker London dispersion forces.
HCl is a polar molecule, resulting in dipole-dipole interactions, which are stronger than London dispersion forces. HF forms hydrogen bonds, which are the strongest intermolecular forces among the given compounds. The presence of F, a highly electronegative element, enables HF to form strong hydrogen bonds, resulting in the highest intermolecular force strength.
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Calculate the mass of glucose ( C6H12O6 ) in a 110 ml sample of a 1.02 m glucose solution.
The mass of glucose in a 110 mL sample of a 1.02 M glucose solution is 20.02 g.
To find the mass of glucose, follow these steps:
1. Convert the volume of the solution to liters: 110 mL = 0.110 L.
2. Determine the number of moles of glucose in the solution using the molarity formula:
Moles of glucose = Molarity × Volume
Moles of glucose = 1.02 M × 0.110 L = 0.1122 mol
3. Calculate the molar mass of glucose (C₆H₁₂O₆) using the periodic table:
Molar mass = (6 × C) + (12 × H) + (6 × O)
Molar mass = (6 × 12.01) + (12 × 1.01) + (6 × 16.00) = 180.18 g/mol
4. Find the mass of glucose by multiplying the number of moles by the molar mass:
Mass of glucose = Moles × Molar mass
Mass of glucose = 0.1122 mol × 180.18 g/mol = 20.02 g
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A weak acid HA is titrated with strong base. Halfway to the equivalence point, the pH of the solution is 7. What is the value of pKa for HA?Express your answer using at least three significant figures. Do not use scientific notation.
The value of pKa for the weak acid HA in this scenario is 7. To determine the value of pKa for a weak acid HA titrated with a strong base halfway to the equivalence point with a pH of 7, follow these steps:
Step:1. Recall that at the halfway point of the titration, [HA] = [A-], where A- is the conjugate base.
Step:2. Use the Henderson-Hasselbalch equation: pH = pKa + log ([A-]/[HA])
Step:3. Since [HA] = [A-], the ratio [A-]/[HA] is equal to 1.
Step:4. Simplify the equation by taking the log of 1, which is 0: pH = pKa + 0
Step:5. In this case, the pH is given as 7, so the equation becomes: 7 = pKa
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enough of a monoprotic weak acid is dissolved in water to produce a 0.0143 m solution. the ph of the resulting solution is 2.66 . calculate the ka for the acid.
The Ka for the monoprotic weak acid is approximately 3.32 x [tex]10^{-5[/tex].
To calculate the Ka for the monoprotic weak acid, follow these steps:
1. Write the dissociation equation for the weak acid (HA) in water: HA <=> H+ + A-
2. Determine the concentration of H+ ions using the given pH. pH = -log[H+]. So, 2.66 = -log[H+]. Solve for [H+]: [H+] = [tex]10^{-2.66[/tex] ≈ 2.18 x [tex]10^{-3[/tex] M
3. Set up an ICE table (Initial, Change, Equilibrium) for the dissociation reaction:
HA <=> H+ + A-
0.0143 - x <=> x + x
0.0143 - x ≈ 0.0143 (since x is small compared to 0.0143)
4. Use the equilibrium expression for Ka: Ka = [H+][A-]/[HA]. Since [H+] = [A-] = x, and [HA] ≈ 0.0143, the equation becomes: Ka = [tex]x^2[/tex] / 0.0143
5. Plug in the value of x ([H+]) calculated in step 2: Ka = (2.18 x [tex](10^{-3} )^2[/tex]/ 0.0143
6. Calculate Ka: Ka ≈ 3.32 x [tex]10^{-5[/tex]
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2. How many grams of Pbl2 can be dissolved in a 500 mL of a 0.050 M Nal solution? Use activities to calculate your answer. Possibly useful information: The temperature is 25 °C. Ksp of Pbl2 is 7.9 x 10-9 at 25 °C. FW of Pbl2 is 461.01 g/mol. FW of Nal is 149.89 g/mol. = = } C ([A]ZĂ + [B]Z+ [C]Z? +...) logy -0.51 Z3 Vu 1+x/305) K2CNaha tkw [H3O+]= V1+Cnaha / Kal
The solubility of [tex]Pbl_{2}[/tex] in a 0.050 M Nal solution can be calculated using the following equation: 0.028 g of [tex]Pbl_{2}[/tex] can dissolve in 500 mL of a 0.050 M Nal solution at 25°C.
Ksp = [[tex]Pb_{2} ^{+}[/tex]][[tex]2I^{-}[/tex]]
where Ksp is the solubility product constant for [tex]Pbl_{2}[/tex], and [[tex]Pb_{2} ^{+}[/tex]] and [[tex]I^{-}[/tex]] are the molar concentrations of [tex]Pb_{2} ^{+}[/tex] and I- ions, respectively, in solution. Since Nal dissociates completely in solution, we can assume that the molar concentration of [tex]I^{-}[/tex] is equal to the molar concentration of Nal.
Let x be the molar solubility of [tex]Pbl_{2}[/tex] in the Nal solution. Then, at equilibrium, the molar concentrations of [tex]Pb_{2} ^{+}[/tex] and I- are both equal to x. Using the expression for Ksp and the molar concentration of Nal, we can write:
Ksp = x * (2x)
0.050 M = [Nal] = [[tex]I^{-}[/tex]] = x
Solving for x, we get:
x = sqrt(Ksp/2) = sqrt(7.9 x [tex]10^{-9/2}[/tex]) = 1.25 x [tex]10^{-4}[/tex] M
The mass of [tex]Pbl_{2}[/tex] that can dissolve in 500 mL of this solution can be calculated as:
mass of [tex]Pbl_{2}[/tex] = molar solubility x volume of solution x FW of [tex]Pbl_{2}[/tex]
mass of [tex]Pbl_{2}[/tex] = (1.25 x [tex]10^{-4}[/tex] M) x (0.500 L) x (461.01 g/mol) = 0.028 g
Therefore, 0.028 g of [tex]Pbl_{2}[/tex] can dissolve in 500 mL of a 0.050 M Nal solution at 25°C.
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What makes up nearly all of the atom's mass?
OA. The sum of all neutrons and electrons
OB. The sum of all protons and electrons
OC. The sum of all isotopes
OD. The sum of all protons and neutrons
SUBMIT
The total of all protons and neutrons is Option D, which is the right response. Protons, neutrons, and electrons are the three fundamental particles that make up an atom.
The nucleus of an atom is made up of protons and neutrons, which are collectively referred to as nucleons and are primarily responsible for an atom's mass. Neutrons weigh 1.6749 x 10-27 kg, whereas protons weigh 1.6726 x 10-27 kg.
Protons and neutrons make up the majority of an atom's mass when added together. However, electrons contribute very little to the mass of the atom due to their much smaller mass of 9.11 x 10-31 kg. As a result, Option D is the right response.
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calculate the poh of a solution that results from mixing 45.8 ml of 0.15 m ethylamine (c2h5nh2) with 16.5 ml of 0.13 m c2h5nh3cl. the kb value for c2h5nh2 is 6.5 x 10-4.
The pH of the solution is 10.32.
What is the pH of the solution?The first step is to write the chemical equation for the reaction between ethylamine and its conjugate acid, ethyl ammonium chloride:
C2H5NH2 + HCl → C2H5NH3+Cl-
Next, we need to determine the initial concentration of ethylamine and the concentration of ethyl ammonium chloride:
initial concentration of C2H5NH2 = 0.15 M x (45.8 mL / 62.3 mL) = 0.110 M
concentration of C2H5NH3+Cl- = 0.13 M x (16.5 mL / 62.3 mL) = 0.035 M
Now we can use the Kb value of ethylamine to calculate the concentration of hydroxide ions:
Kb = [C2H5NH2][OH-] / [C2H5NH3+]
[OH-] = Kb x [C2H5NH3+] / [C2H5NH2] = (6.5 x 10^-4) x (0.035) / (0.110) = 2.085 x 10^-4 M
Finally, we can use the concentration of hydroxide ions to calculate the pOH and then the pH:
pOH = -log[OH-] = -log(2.085 x 10^-4) = 3.68
pH + pOH = 14, so:
pH = 14 - pOH = 14 - 3.68 = 10.32
Therefore, the pH of the solution is 10.32.
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Identify the diatomic molecule that is ionic in its pure state.Identify the molecule or molecules containing polar covalent bonds.Please explain!!!
A diatomic molecule consists of two atoms bonded together. In its pure state, a diatomic molecule that is ionic would be lithium hydride (LiH).
This is because lithium (Li) loses an electron to become positively charged, while hydrogen (H) gains an electron to become negatively charged, resulting in an ionic bond.
Molecules containing polar covalent bonds are those where the atoms have differing electronegativities, causing an uneven distribution of electron density.
Examples of diatomic molecules with polar covalent bonds include hydrogen chloride (HCl), hydrogen fluoride (HF), and hydrogen bromide (HBr). In these cases, the halogens (Cl, F, Br) are more electronegative than hydrogen, leading to a polar bond where the electrons are closer to the halogen atoms.
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chcl3 is 0.4693 are 74.166 cm3 mol−1 and 80.235 cm3 mol−1 mol−1 , respectively. what is the volume of a solution of mass 1.000 kg?
The volume of a solution of CHCl3 with a mass of 1.000 kg is approximately 1.2485 L.
To determine the volume of a solution of CHCl3 with a mass of 1.000 kg, we need to use the density and molar mass of CHCl3 to convert from mass to volume.
First, we can calculate the number of moles of CHCl3 in the solution:
mass of CHCl3 = 1.000 kg = 1000 g
molar mass of CHCl3 = 12.01 + 1.008 x 3 + 35.45 = 119.37 g/mol
moles of CHCl3 = mass of CHCl3 / molar mass of CHCl3 = 1000 / 119.37 = 8.387 mol
Next, we can use the molar volume of gases at standard temperature and pressure (STP) to convert from moles of CHCl3 to volume:
molar volume of gas at STP = 22.414 L/mol
volume of CHCl3 at STP = moles of CHCl3 x molar volume of gas at STP = 8.387 mol x 22.414 L/mol = 188.0 L
However, the density of CHCl3 is not the same as that of an ideal gas at STP. We are given the specific volumes of CHCl3 at 74.166 cm3/mol and 80.235 cm3/mol, for a total solution volume of:
volume of CHCl3 solution = moles of CHCl3 x specific volume of CHCl3 solution
= 8.387 mol x (74.166 cm3/mol + 80.235 cm3/mol) = 1248.5 cm3
Finally, we can convert the volume from cubic centimeters to liters:
volume of CHCl3 solution = 1248.5 cm3 = 1.2485 L
Therefore, the volume of a solution of CHCl3 with a mass of 1.000 kg is approximately 1.2485 L.
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what is the pe value in an acid mine water sample having [fe3 ] = 7.03e-3m and [fe2 ]=3.71e-4m? fe3 e- fe2 pe° = 13.2
The pe value in the acid mine water sample is approximately 12.641.
To calculate the pe value in an acid mine water sample, we can use the Nernst equation:
pe = pe° + (RT/nF) ln([Fe[tex]^{2+}[/tex]]/[Fe[tex]_{3+}[/tex]])
Given that [Fe3+] = 7.03e-3 M and [Fe[tex]^{2+}[/tex]] = 3.71e-4 M, and pe° = 13.2, we can substitute these values into the equation and solve for pe:
pe = 13.2 + (RT/nF) ln(3.71e-4/7.03e-3)
At room temperature (25°C), the gas constant R = 8.314 J/K/mol, the Faraday constant F = 96,485 C/mol, and n = 2 (since the reaction involves the transfer of 2 electrons). Plugging in these values, we get:
pe = 13.2 + (8.314×298/2/96485) ln(3.71e-4/7.03e-3)
= 13.2 + (-0.559)
= 12.641
Therefore, approximately 12.641 is the pe value in the acid mine water sample.
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16.047 g of nh4cl(s) (mw = 53.45, kb nh3 = 1.79 × 10-5) is added to 25 ml of 6 m naoh(aq) (mw = 40). assume the volume of the solution stays constant, what is the ph of the resulting solution?
the pH of the solution after 5.00 mL of 0.125 M HClO4 have been added is 12.98.
The balanced chemical equation for the reaction between KOH and HClO4 is:
KOH + HClO4 -> KClO4 + H2O
From this equation, we can see that the stoichiometry of the reaction is 1:1, which means that 1 mole of HClO4 reacts with 1 mole of KOH.
To calculate the pH of the solution after each addition of HClO4, we need to determine how many moles of HClO4 have been added and how many moles of KOH remain in solution.
At the start of the titration, the number of moles of KOH in the sample is:
moles of KOH = concentration × volume = 0.150 mol/L × 0.0200 L = 0.00300 mol
When we add x moles of HClO4, they will react completely with x moles of KOH. Therefore, the number of moles of KOH remaining in solution after x moles of HClO4 have been added is:
moles of KOH remaining = 0.00300 mol - x mol
The volume of HClO4 required to react completely with all the KOH is given by:
moles of HClO4 = moles of KOH = 0.00300 mol
volume of HClO4 = moles of HClO4 / concentration of HClO4 = 0.00300 mol / 0.125 mol/L = 0.0240 L
So, we need 0.0240 L of 0.125 M HClO4 to react completely with the KOH in the sample.
To calculate the pH after a certain volume of HClO4 has been added, we can use the following steps:
1. Calculate the number of moles of HClO4 that have been added.
2. Calculate the number of moles of KOH remaining in solution.
3. Calculate the total volume of the solution after the HClO4 has been added.
4. Calculate the concentration of the remaining KOH.
5. Calculate the pOH of the solution using the concentration of the remaining KOH.
6. Calculate the pH of the solution using the formula pH = 14 - pOH.
For example, if 5.00 mL of 0.125 M HClO4 have been added, the number of moles of HClO4 added
is:
moles of HClO4 = concentration × volume = 0.125 mol/L × 0.00500 L = 0.000625 mol
The number of moles of KOH remaining in solution is:
moles of KOH remaining = 0.00300 mol - 0.000625 mol = 0.00238 mol
The total volume of the solution after the HClO4 has been added is:
total volume = initial volume + volume of HClO4 = 20.0 mL + 5.00 mL = 25.0 mL = 0.0250 L
The concentration of the remaining KOH is:
concentration of KOH = moles of KOH remaining / total volume = 0.00238 mol / 0.0250 L = 0.0952 mol/L
The pOH of the solution is:
pOH = -log[OH-] = -log(0.0952) = 1.020
The pH of the solution is:
pH = 14 - pOH = 14 - 1.020 = 12.98
Therefore, the pH of the solution after 5.00 mL of 0.125 M HClO4 have been added is 12.98.
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What mass of naobr(s) must be dissolved in 114 ml of 0.255 m HoBr to produce a buffer solution with ph 8.30? Assume no change in volume. ka = 2.3 x 10^-9 for hobr.
0.155 g of NaOBr(s) must be dissolved in 114 mL of 0.255 M HOBr to produce a buffer solution with a pH of 8.30.
We need to determine the ratio of [tex][OBr^-]/[HOBr][/tex] required to prepare a buffer solution with a pH of 8.30. The pKa of HOBr is given as 2.3 x [tex]10^-^9[/tex]. Therefore, we can use the Henderson-Hasselbalch equation to calculate the ratio of [tex][OBr^-]/[HOBr][/tex]:
pH = [tex]pK_a + log([OBr^-]/[HOBr])[/tex]
8.30 = 9.64 + [tex]log([OBr^-]/[HOBr])[/tex]
[tex]log([OBr^-]/[HOBr])[/tex] = -1.34
[tex]([OBr^-]/[HOBr])[/tex] = 4.47 x [tex]10^-^2[/tex]
We need to calculate the moles of HOBr present in 114 mL of 0.255 M HOBr:
moles HOBr = (0.255 mol/L) x (0.114 L) = 0.0291 mol
Since the ratio of[tex][OBr^-]/[HOBr][/tex] is known, we can calculate the moles of [tex]OBr^-[/tex] required to form the buffer solution:
moles [tex]OBr^-[/tex] = [tex][OBr^-]/[HOBr][/tex] x moles HOBr
moles [tex]OBr^-[/tex]= 4.47 x 10^-2 x 0.0291 mol = 1.30 x [tex]10^-^3[/tex] mol
Finally, we need to calculate the mass of NaOBr(s) required to produce 1.30 x[tex]10^-^3[/tex] mol of [tex]OBr^-[/tex]. The molar mass of NaOBr is 118.89 g/mol.
mass NaOBr = moles NaOBr x molar mass NaOBr
mass NaOBr = 1.30 x [tex]10^-^3[/tex] mol x 118.89 g/mol = 0.155 g
Therefore, 0.155 g of NaOBr(s) must be dissolved in 114 mL of 0.255 M HOBr to produce a buffer solution with a pH of 8.30.
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