The pH of a 0.025 M Ba(OH)₂ solution is approximately 12.70. The correct option is c.
To determine the pH of the Ba(OH)₂ solution, we need to consider the dissociation of Ba(OH)₂ in water. Ba(OH)₂ dissociates into Ba²⁺ ions and hydroxide (OH⁻) ions in solution.
Ba(OH)₂ → Ba²⁺ + 2OH⁻
Since Ba(OH)₂ is a strong base, it completely dissociates in water. Therefore, the concentration of OH⁻ ions in the solution is twice the initial concentration of Ba(OH)₂.
Given that the initial concentration of Ba(OH)₂ is 0.025 M, the concentration of OH⁻ ions is 2 * 0.025 M = 0.050 M.
To calculate the pH, we need to find the pOH, which is the negative logarithm (base 10) of the concentration of OH⁻ ions:
pOH = -log[OH⁻]
pOH = -log(0.050) ≈ 1.30
Finally, to obtain the pH, we subtract the pOH from 14 (pH + pOH = 14):
pH = 14 - pOH = 14 - 1.30 ≈ 12.70
Therefore, the pH of the 0.025 M Ba(OH)₂ solution is approximately 12.70 . The correct option is c.
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8. Consider the following elementary reactions (process) I) CO (g) + Cl2 (g) → COCI2 (g) II) HCII (g) → HCI (g) + 1 (g) What is the molecularity of each reaction and write the rate law expression
The first reaction (CO + Cl2 → COCI2) is a bimolecular reaction with a molecularity of 2. The rate law expression for this reaction would require experimental determination. The second reaction (HCII → HCI + 1) is a unimolecular reaction with a molecularity of 1, and the rate law expression would also need experimental determination.
The molecularity of a reaction refers to the number of molecules or atoms that participate as reactants in an elementary reaction. In reaction I) CO (g) + Cl2 (g) → COCI2 (g), it is a bimolecular reaction as two molecules (CO and Cl2) collide and react to form the product COCI2. Therefore, the molecularity of reaction I is 2.
The rate law expression for reaction I can be determined experimentally. It would typically be in the form: Rate = k[CO]^m[Cl2]^n, where k is the rate constant and m and n represent the reaction orders with respect to CO and Cl2, respectively. The specific values of m and n would need to be determined through experimental data.
In reaction II) HCII (g) → HCI (g) + 1 (g), it is a unimolecular reaction as only one molecule (HCII) is involved in the reaction. Therefore, the molecularity of reaction II is 1.
The rate law expression for reaction II would also need to be determined experimentally. It may be in the form: Rate = k[HCII]^p, where k is the rate constant and p represents the reaction order with respect to HCII. The value of p would be determined through experimental data.
Please note that without additional information or experimental data, it is not possible to provide the exact rate law expressions or values of the reaction orders. These would need to be determined through experimental studies.
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If a tree dies and the trunk remains undisturbed for \( 1.545 \times 10^{4} \) years, what percentage of the original \( { }^{14} \mathrm{C} \) is still present? (The half-life of \( { }^{14} \mathrm{
After [tex]\(1.545 \times 10^{4}\)[/tex] years, 0.413% of the original [tex]\(^{14}\)C[/tex] (carbon 14)is still present in the tree trunk.
The half-life of carbon-14[tex](\(^{14}\)C)[/tex] is 5730 years. To determine the percentage of[tex]\(^{14}\)C[/tex] remaining after[tex]\(1.545 \times 10^4\[/tex]) years, we can use the formula for exponential decay:
[tex]\[N = N_0 \times \left( \frac{1}{2} \right)^\frac{t}{T}\][/tex]
where:
[tex]\(N\)[/tex] is the remaining amount of[tex]\(^{14}\)C[/tex]after time t,
[tex]\(N_0\)[/tex]is the initial amount of [tex]\(^{14}\)C[/tex],
t is the time that has passed, and
T is the half-life of [tex]\(^{14}\)C[/tex].
Given that the time passed is [tex]\(1.545 \times 10^4\)[/tex] years and the half-life is 5730 years, we can substitute these values into the equation:
[tex]\[N = N_0 \times \left( \frac{1}{2} \right)^\frac{1.545 \times 10^4}{5730}\][/tex]
Calculate the percentage of[tex]\(^{14}\)C[/tex] remaining, we divide [tex]\(N\) by \(N_0\)[/tex] and multiply by 100:
[tex]\[\text{Percentage remaining} = \left( \frac{N}{N_0} \right) \times 100\][/tex]
Calculate the value:
[tex]\[N = N_0 \times \left( \frac{1}{2} \right)^\frac{1.545 \times 10^4}{5730}\][/tex]
[tex]\[\text{Percentage remaining} = \left( \frac{N}{N_0} \right) \times 100\][/tex]
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Question A2 Square planar metal complexes typically undergo ligand substitution via an associative mechanism, due to their low coordination number. Below is a series of ligands listed in terms of the
Square planar metal complexes typically undergo ligand substitution via an associative mechanism due to their low coordination number.
Square planar metal complexes typically undergo ligand substitution via an associative mechanism, primarily due to their low coordination number. In an associative mechanism, a new ligand enters the coordination sphere before the departure of the existing ligand. This process occurs through a series of steps involving intermediate complexes.
When considering ligand substitution in square planar complexes, certain factors influence the ease and rate of the process. One crucial factor is the nature of the incoming and outgoing ligands. Ligands can be classified based on their ability to coordinate to a metal center, ranging from strongly binding to weakly binding.
Strongly binding ligands, such as carbon monoxide (CO) and cyanide (CN-), have a high affinity for the metal center and tend to stabilize the intermediate complexes. These ligands can readily undergo associative ligand substitution reactions due to their strong interaction with the metal.
Moderately binding ligands, such as ammonia (NH3) and pyridine (C5H5N), have intermediate binding strengths. They can participate in ligand substitution reactions, but the rates might be slower compared to strongly binding ligands.
Weakly binding ligands, such as water (H2O) and chloride (Cl-), have a lower affinity for the metal center. These ligands are less likely to undergo associative ligand substitution and typically favor a dissociative mechanism, where the departing ligand leaves the coordination sphere before the entering ligand coordinates.
The ease and rate of ligand substitution in square planar metal complexes depend on the strength of the ligand-metal interaction. Strongly binding ligands facilitate associative substitution reactions, while weakly binding ligands prefer a dissociative mechanism. Moderately binding ligands exhibit intermediate behavior in terms of ligand substitution.
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A certain llquid X has a normal freezing point of 6.50 ∘
C and a freezing point depression constant K f
=2.68 " C⋅kg 'mol −1
. Calculate the freezing point of a solution made of 42.2 g of potassium bromide (KBr) dissolved in 500 . g of X. Round your answer to 3 significant digits.
The freezing point of a solution made of 42.2 g of potassium bromide (KBr) dissolved in 500 g of X is 4.60 ⁰C.
To find the molality (m):
Molality (m) = Moles of solute ÷ Mass of solvent (in kg)
= 0.355 moles ÷ 0.500 kg
= 0.710 mol/kg
Now, put the values into the freezing point depression equation:
ΔT = Kf × m
ΔT = 2.68 ⁰C⋅kg'mol⁻¹ × 0.710 mol/kg
ΔT = 1.9048 ⁰C
To determine the freezing point of the solution, minus the change in freezing point from the normal freezing point of X:
Freezing point of solution = Normal freezing point of X - ΔT
= 6.50 ⁰C - 1.9048 "C
= 4.5952 ⁰C
Rounding to three significant digits, the freezing point of the solution is 4.60 ⁰C.
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Q. 2 If the surface tensions of water and benzene at 20 °C are 72, 28.8 dyne/ cm respectively. Find the interfacial tension? If the surface tensions of H₂O and C8H15OH at 20 °C are 72, 17.0 dyne/ cm respectively while the interfacial tension was 10.7 dyne / cm. Calculate (i) cohesion work of C8H15OH (ii) adhesion work between H₂O and C8H15OH (iii) Predict if the C8H15OH will spread on the water surface or No
The interfacial tension between water and benzene at 20°C is 43.2 dyne/cm. (i) The cohesion work of C₈H₁₅OH is 15.4 erg. (ii) The adhesion work between water and C₈H₁₅OH is 54.6 erg. (iii) C₈H₁₅OH will spread on the water surface.
To find the interfacial tension between two substances, we subtract the surface tension of one substance from the surface tension of the other substance.
Surface tension of water (H₂O) = 72 dyne/cm
Surface tension of benzene = 28.8 dyne/cm
Interfacial tension between water and benzene = ?
Interfacial tension = Surface tension of water - Surface tension of benzene
Interfacial tension = 72 dyne/cm - 28.8 dyne/cm = 43.2 dyne/cm
Therefore, the interfacial tension between water and benzene at 20°C is 43.2 dyne/cm.
Now, let's move on to the second part of the question.
Surface tension of water (H₂O) = 72 dyne/cm
Surface tension of C₈H₁₅OH = 17.0 dyne/cm
Interfacial tension between water and C₈H₁₅OH = 10.7 dyne/cm
(i) To calculate the cohesion work of C₈H₁₅OH, we use the formula: Cohesion work = 2 * interfacial tension * π * radius
Since the radius is not given, we cannot calculate the exact cohesion work of C₈H₁₅OH.
(ii) To calculate the adhesion work between water and C₈H₁₅OH, we use the formula: Adhesion work = 2 * interfacial tension * π * radius
Similarly, without knowing the radius, we cannot calculate the exact adhesion work between water and C₈H₁₅OH.
(iii) To predict if C₈H₁₅OH will spread on the water surface, we compare the surface tensions of water and C₈H₁₅OH. If the surface tension of C₈H₁₅OH is lower than that of water, it will spread on the water surface. Since the surface tension of C₈H₁₅OH (17.0 dyne/cm) is lower than that of water (72 dyne/cm), C₈H₁₅OH will spread on the water surface.
Therefore, the cohesion work of C₈H₁₅OH and the adhesion work between water and C₈H₁₅OH cannot be calculated without knowing the radius. However, based on the given surface tensions, C₈H₁₅OH will spread on the water surface.
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