Answer:
7.28Explanation:
The pH of a solution can be found by using the formula
[tex]pH = - log [ { H_3O}^{+}][/tex]
From the question we have
[tex]ph = - log(5.2 \times {10}^{ - 8} ) \\ = 7.28399[/tex]
We have the final answer as
7.28Hope this helps you
Which best defines the term drug
Answer:
a medicine or other substance which has a physiological effect when ingested or otherwise introduced into the body.
Explanation:
61. Using the symbol of the previous noble gas to indicate the core
electrons, write the electron configuration for each of the fol-
lowing elements.
a. scandium, Z= 21 c. lanthanum, Z= 57
b. yttrium, Z = 39
d. actinium, Z= 89
Answer:
Scandium, with atomic number of 21 = [Ar]3d¹4s²
Yttrium, with atomic number of 39 = [Kr]4d¹5s²
Lanthanum, with atomic number of 57 = [Xe]5d¹6s²
Actinium, with atomic number of 89 = [Rn]6d¹7s²
Explanation:
The electronic configuration of atoms of elements describes how electrons are arranged in the atomic orbitals of the atom. The electron configurations of atoms in standard notation is usually written sequentially with all electron-containing atomic subshells (s, p, d and f) and the number of electrons they contain in superscript. For example, the electron configuration of Neon is 1s²2s²2p⁶. However, an abbreviated notation can be used especially for elements having large atomic numbers. The symbol of the previous noble gas in square brackets indicating the core electrons is written before the outermost shell electrons of the atom. For example, the abbreviated electron configuration of sodium is [Ne]3s¹.
The electronic configuration of the given elements are shown below:
Scandium, with atomic number of 21 = [Ar]3d¹4s²
Yttrium, with atomic number of 39 = [Kr]4d¹5s²
Lanthanum, with atomic number of 57 = [Xe]5d¹6s²
Actinium, with atomic number of 89 = [Rn]6d¹7s²
Determine which of these properties would distinguish these two substances: (a) boiling point; (b) combustion analysis results; (c) molecular weight; (d) density at a given temperature and pressure. You can check on the properties of these two compounds
Answer:
(a) boiling point
(d) density at a given temperature and pressure.
Explanation:
Isomers are compounds that have the same molecular formula but different structural formulas. They differ in chemical and physical properties depending on the type of isomerism displayed by the compounds.
The compounds stated here are structural or constitutional isomers hence they possess different boiling points and densities at a given temperature and pressure owing to structural differences in the molecules.
Since they have the same molecular formula, they must yield the same result during combustion analysis and they must have the same molecular weight.
What is the chemical equation for F2 + At- -->
Answer:
F₂ + 2At --> 2AtF
Explanation:
Astatine is a halogen but is not diatomic. It's possible oxidation states are 1⁺, 1⁻, or 5⁺. Fluorine only has the possible oxidation states of 1⁺ or 1⁻.
Glycerol. C3HgO3, is a substance used extensively in the manufacture of cosmetics, foodstuffs, antifreeze, and plastics. Glycerol is a water-soluble liquid
with a density of 1.2656 g/mL at 15 °C. Calculate the molarity of a solution of glycerol made by dissolving 50.000 mL glycerol at 15 °C in enough water to
make 250.00 mL of solution. The molecular weight of C3HgO3 is 92.094 amu.
O A 0.6871
O B. 3.600
O C. 63.28
O 0.92.10
O E. 2.749
Answer: The correct option is E.) 2.749 M.
Explanation:
Density is defined as the ratio of mass and volume of a substance.
[tex]\text{Density}=\frac{\text{Mass}}{\text{Volume}} [/tex] ......(1)
Given values:
Volume of glycerol = 50.0 mL
Density of glycerol = 1.2656 g/mL
Putting values in equation 1, we get:
[tex]\text{Mass of glycerol }=(1.2656g/mL\times 50.0mL)=63.28g[/tex]
Molarity is defined as the amount of solute expressed in the number of moles present per liter of solution. The units of molarity are mol/L. The formula used to calculate molarity:
[tex]\text{Molarity of solution}=\frac{\text{Given mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (mL)}}[/tex] .....(2)
Given values:
Given mass of glycerol = 63.28 g
Molar mass of glycerol = 92.094 g/mol
Volume of the solution = 250.00 mL
Putting values in equation 2, we get:
[tex]\text{Molarity of solution}=\frac{63.28\times 1000}{92.094\times 250.00}\\\\\text{Molarity of solution}=2.749M[/tex]
Hence, the correct option is E.) 2.749 M.
12. The reaction 2NO, (g) = N20,(g) reaches equilibrium.
How does increasing the pressure on this system affect the amount o
The amount of N20 remains the same.
The amount of N20 increases.
The amount of N20 decreases.
Answer:
The amount of N2O4 increases.
Explanation:
Based on LeCh's principle, a change in the state of an equilibrium produce an effect in the system that try to restore the initial equilibrium.
For example, in the problem, the change is the increasing in the pressure. The system will try to decrease the pressure of the system. To decrease the pressure the system needs to decrease the moles of gas. As 2 moles of NO2 produce 1 mole of N2O4, the system will:
Shift to the right increasing the amount of N2O4 and decreasing the amount of NO2. Right option is:
The amount of N2O4 increases.Extension: Cedric has been in the hospital for 15 weeks, how many minutes is that? Use
conversion factors with units to solve the problem and show your work
Answer:
151200 minutes.
Explanation:
From the question given above, the following data were obtained:
Time (in week) = 15 weeks
Time (in min) =?
Next, we shall convert 15 weeks to days. This can be obtained as follow:
1 week = 7 days
Therefore,
15 weeks = 15 weeks × 7 days / 1 week
15 weeks = 105 days
Next, we shall convert 105 days to hours. This can be obtained as follow:
1 day = 24 h
Therefore,
105 days = 105 days × 24 h / 1 day
105 days = 2520 h
Finally, we shall convert 2520 h to mins. This can be obtained as follow:
1 h = 60 mins
Therefore,
2520 h = 2520 h × 60 mins / 1 h
2520 h = 151200 mins
Thus, 15 weeks is equivalent to 151200 minutes.
The neutralization of a 0.455 g sample of recrystallized aspirin required 38.6 mL of 0.100 M NaOH solution. An additional 25.0 mL of 0.100 M NaOH was added to the sample to hydrolyze the neutralized aspirin in the solution. The solution was heated. Phenolphthalein was added to the cooled solution and was back-titrated with 11.2 mL of 0.100 M HCl. Which of the following statements is true
A) Before the solution is titrated with HCl it is pink and when the color changes from pink to colorless, the moles of H*(aq) equals the moles of OH"(aq) used in the hydrolysis of the neutralized aspirin.
B) Before the solution is titrated with HCl it is colorless and when the color changes from colorless to pink, the moles of H*(aq) equals the excess moles of OH(aq) added.
C) 25.0 mL of 0.100 M NaOH was added to the sample to hydrolyze the neutralized aspirin in the solution. The titration with HCl allows us to determine the moles of excess OH(aq) added. Once we determine the moles of excess OH(aq), we can determine moles of OH"(aq) used in the hydrolysis of the neutralized aspirin, which is equal to the moles of aspirin in the recrystallized aspirin.
D) We can determine the moles of aspirin in the recrystallized aspirin by titrating with the 0.100 M NaOH to the neutralization point. The purpose of the hydrolysis of the neutralized aspirin and the back-titration with the 0.100 M HCl is to confirm the moles of aspirin in the recrystallized aspirin.
E) Two of the above statements are true.
Answer:
E) Two of the above statements are true.
Explanation:
The options are:
A) Before the solution is titrated with HCl it is pink and when the color changes from pink to colorless, the moles of H*(aq) equals the moles of OH"(aq) used in the hydrolysis of the neutralized aspirin. TRUE. Before the solution is titrated, there is an excess of NaOH (Basic solution, phenolphtalein is pink). Then, at equivalence point, after the addition of HCl, the pH is acidic and phenolphtalein is colorless.
B) Before the solution is titrated with HCl it is colorless and when the color changes from colorless to pink, the moles of H*(aq) equals the excess moles of OH(aq) added. FALSE. As was explained, before the titration, the solution is pink.
C) 25.0 mL of 0.100 M NaOH was added to the sample to hydrolyze the neutralized aspirin in the solution. The titration with HCl allows us to determine the moles of excess OH(aq) added. Once we determine the moles of excess OH(aq), we can determine moles of OH"(aq) used in the hydrolysis of the neutralized aspirin, which is equal to the moles of aspirin in the recrystallized aspirin. TRUE. Aspirin requires an excess of base (NaOH) for a complete dissolution (Hydrolysis). Then, we add H+ as HCl to know the excess moles of OH-. As we know the added moles of OH-, we can find the moles of OH that reacted = Moles of aspirin.
D) We can determine the moles of aspirin in the recrystallized aspirin by titrating with the 0.100 M NaOH to the neutralization point. The purpose of the hydrolysis of the neutralized aspirin and the back-titration with the 0.100 M HCl is to confirm the moles of aspirin in the recrystallized aspirin. FALSE. NaOH can be added directly unyil neutralization point because, initially, aspirin can't be dissolved completely
E) Two of the above statements are true. TRUE
Right option is:
E) Two of the above statements are true.In this exercise it is necessary to identify the true alternatives and the false alternatives. Thus, classifying these alternatives we have:
A) True
B) False
C) True
D) False
E) True
So we can say that: Two of the above statements are true.
The options are:
A) Before the solution is titrated with [tex]HCl[/tex] it is pink and when the color changes from pink to colorless, the moles of [tex]H*(aq)[/tex] equals the moles of [tex]OH"(aq)[/tex] used in the hydrolysis of the neutralized aspirin. TRUE. Before the solution is titrated, there is an excess of [tex]NaOH[/tex] (Basic solution, phenolphtalein is pink). Then, at equivalence point, after the addition of [tex]HCl[/tex], the pH is acidic and phenolphtalein is colorless.
B) Before the solution is titrated with [tex]HCl[/tex] it is colorless and when the color changes from colorless to pink, the moles of [tex]H*(aq)[/tex] equals the excess moles of [tex]OH(aq)[/tex] added. FALSE. As was explained, before the titration, the solution is pink.
C) 25.0 mL of 0.100 M NaOH was added to the sample to hydrolyze the neutralized aspirin in the solution. The titration with [tex]HCl[/tex] allows us to determine the moles of excess [tex]OH(aq)[/tex] added. Once we determine the moles of excess [tex]OH(aq)[/tex], we can determine moles of [tex]OH"(aq)[/tex] used in the hydrolysis of the neutralized aspirin, which is equal to the moles of aspirin in the recrystallized aspirin. TRUE. Aspirin requires an excess of base [tex](NaOH)[/tex] for a complete dissolution (Hydrolysis). Then, we add [tex]H+[/tex] as [tex]HCl[/tex] to know the excess moles of [tex]OH-[/tex]. As we know the added moles of [tex]OH-[/tex], we can find the moles of [tex]OH[/tex] that reacted (Moles of aspirin).
D) We can determine the moles of aspirin in the recrystallized aspirin by titrating with the [tex]0.100 M NaOH[/tex] to the neutralization point. The purpose of the hydrolysis of the neutralized aspirin and the back-titration with the [tex]0.100 M HCl[/tex] is to confirm the moles of aspirin in the recrystallized aspirin. FALSE. [tex]NaOH[/tex] can be added directly unyil neutralization point because, initially, aspirin can't be dissolved completely
E) Two of the above statements are true. TRUE
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A student performs an experiment three times. The results are 4.52 g/mL, 4.54 g/mL, and 4.39 g/mL. Which of the following best describes these results with only the information given in this question?
a. high accuracy
b. high accuracy and high precision
c. high accuracy and low precision
d. high precision
Unit 09: Acids, Bases, and the PH Scale
Answer:
Err... Mate are we suppose to give you resources on this topic, or do we just err respond? if I will give you resources?
Explanation:
The acid-dissociation constants for three acids are shown in the table.
Which is the strongest acid?
The strongest acid as per dissociation constant is hydrochloric acid.
What are acids?Acids are defined as substances which on dissociation yield H+ ions , and these substances are sour in taste. Compounds such as HCl, H₂SO₄ and HNO₃ are acids as they yield H+ ions on dissociation.
According to the number of H+ ions which are generated on dissociation acids are classified as mono-protic , di-protic ,tri-protic and polyprotic acids depending on the number of protons which are liberated on dissociation.
Acids are widely used in industries for production of fertilizers, detergents batteries and dyes.They are used in chemical industries for production of chemical compounds like salts which are produced by neutralization reactions.Acids are also used in titrations.
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The physical properties of a substance containing the bonded atoms y and z ?
the first liquid that comes out of a woman's breast after delivery is called?
The first liquid (milk) that comes out of a woman's breast after delivery is called [tex]\sf\purple{colostrum}[/tex].
[tex]\large\mathfrak{{\pmb{\underline{\orange{Happy\:learning }}{\orange{!}}}}}[/tex]
What is the general trend in electro negativity as you move from left to right across the periodic table
Answer:
On the periodic table, electronegativity generally increases as you move from left to right across a period and decreases as you go down a group. As a result, the most electronegative elements are found on the top right of the periodic table, while the least electronegative elements are found on the bottom left.
Explanation:
Answer:
The Electronegativity increases
Explanation:
;)
3 valance electrons on the 4th shell
Hydrolysis of the compound B5H9 forms boric acid, H3BO3. Fusion of boric acid with sodium oxide forms a borate salt, Na2B4O7. Part A Without writing complete equations, find the mass (in grams) of B5H9 required to form 148 g of the borate salt by this reaction sequence.
Answer:
37.09 g of B₅H₉ is required to form 148 g of borate salt( Na₂B₄O₇ )
Explanation:
Given the data in the question;
B₅H₉ → H₃BO₃ → Na₂B₄O₇
find the mass (in grams) of B5H9 required to form 148 g of the borate salt by this reaction sequence.
S M.W
B₅H₉ 63
H₃BO₃ 62
Na₂B₄O₇ 201
So, moles of Na₂B₄O₇ = 148 / 201 = 0.736
Since Boron will be conserved,
Moles of Boron atoms in Na₂B₄O₇ will be;
⇒ 4 × 0.736 = 2.944
Now, Moles of Boron in Na₂B₄O₇ = Moles of Boron in H₃BO₃ = Moles of Boron in B₅H₉
Hence,
Moles of Boron in B₅H₉ = 2.944
Moles of B₅H₉ = 2.944 / 5 = 0.5888
Mass of B₅H₉ = 0.5888 × 63 = 37.09 g
Therefore, 37.09 g of B₅H₉ is required to form 148 g of borate salt( Na₂B₄O₇ )
Which of the following reactions would result in decreased entropy?
O A. H20(g) → H20(1)
O B. CO2(s) → CO2(9)
O C. 203(9) ► 302(9)
O D. N2204(9) ► 2NO39)
Answer:
A
Explanation:
A P E X
Would an electron in the 1s orbital of lithium require the same energy to move to a higher energy level as an electron in the
1s orbital of silver?
Answer:
See explanation
Explanation:
We must remember that the energy required to move an electron from the 1s orbital to a higher energy level depends on the size of the nuclear charge.
The higher the nuclear charge, the more closely held the 1s electron of the atom is to the nucleus and the more difficult it is to excite this electron.
Hence, it requires more energy to excite the 1s electron of silver having a larger size of nuclear charge than it is to excite a 1s electron in lithium.
An imaginary line dividing the earth's surface into two hemisphere the northern and southern hemisphere, it is locatedat 0⁰, which of the following imaginary lines is being described? a.equator b.latitude c.longitude d.prime meridian
Answer:
A. Equator
Explanation:
The equator is located in the centre of the Earth, dividing the northern and southern hemispheres.
Answer:
Equator because equator divides the earth into Northern and Southern hemisphere.
Identify the calculations possible using only 28.02 g/mol as a conversion factor. Select one or more:
The question is incomplete, the complete question is:
Identify the calculations possible using only 28.02 g/mol as a conversion factor. Select one or more:
(a): Calculate the grams of [tex]N_2[/tex] in 10.58 L of nitrogen gas
(b): Calculate the grams of [tex]N_2[/tex] in [tex]5.03\times 10^{20}[/tex] moles of nitrogen gas
(c): Calculate the moles of [tex]N_2[/tex] molecules in 3.94 grams of nitrogen gas
(d): Calculate the moles of [tex]N_2[/tex] molecules in 4.73 L of nitrogen gas
Answer: The correct options are (b) and (c).
Explanation:
We are given:
Molar mass of [tex]N_2[/tex] = 28.02 g/mol
The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
At STP conditions:
1 mole of gas occupies 22.4 L of volume
For the given options:
(a): Volume is given and to calculate the mass of [tex]N_2[/tex], we need to use both the conversion factors above.
The equation formed will be:
Mass of [tex]N_2[/tex] = [tex]\frac{1mol}{22.4L}\times 10.58L\times 28.02 g/mol[/tex]
(b): Moles are given and to calculate the mass of [tex]N_2[/tex], we need only the first conversion factor.
The equation formed will be:
Mass of [tex]N_2[/tex] = [tex](5.03\times 10^{20}mol)\times 28.02g/mol[/tex]
(c): Mass is given and to calculate the moles of [tex]N_2[/tex] molecules, we need only the first conversion factor.
The equation formed will be:
Moles of [tex]N_2[/tex] molecules = [tex]\frac{3.94 g}{28.02g/mol}[/tex]
(d): Volume is given and to calculate the moles of [tex]N_2[/tex] molecules, we need only the second conversion factor.
The equation formed will be:
Moles of [tex]N_2[/tex] molecules = [tex]\frac{1mol}{22.4L}\times 4.73L[/tex]
Hence, the correct option is (b) and (c)
Using only 28.02 g/mol as a conversion factor, we can:
(b): Calculate the grams of N₂ in 5.03 × 10²⁰ moles of nitrogen gas. (c): Calculate the moles of N₂ molecules in 3.94 grams of nitrogen gas.We want to identify the conversion factors required in a series of calculations.
What is a conversion factor?A conversion factor is an arithmetical multiplier for converting a quantity expressed in one set of units into an equivalent expressed in another.
28.02 g/mol, which is the molar mass of nitrogen, is a conversion factor to convert moles to mass and vice versa.
(a): Calculate the grams of N₂ in 10.58 L of nitrogen gas.We want to convert 10.58 L (volume) to grams (mass). We need to conversion factors:
22.4 L/mol is the conversion factor to convert volume to moles.28.02 g/mol is the conversion factor to convert moles to mass.(b): Calculate the grams of N₂ in 5.03 × 10²⁰ moles of nitrogen gas.We want to convert 5.03 × 10²⁰ moles (moles) to grams (mass). We can do so by just using 28.02 g/mol as the conversion factor.
(c): Calculate the moles of N₂ molecules in 3.94 grams of nitrogen gas.We want to convert 3.94 grams (mass) to moles. We can do so by just using 28.02 g/mol as the conversion factor.
(d): Calculate the moles of N₂ molecules in 4.73 L of nitrogen gas.We want to convert 4.73 L (volume) to moles. The required conversion factor is 22.4 L/mol.
Using only 28.02 g/mol as a conversion factor, we can:
(b): Calculate the grams of N₂ in 5.03 × 10²⁰ moles of nitrogen gas. (c): Calculate the moles of N₂ molecules in 3.94 grams of nitrogen gas.The question is incomplete, the complete question is:
Identify the calculations possible using only 28.02 g/mol as a conversion factor. Select one or more:
(a): Calculate the grams of N₂ in 10.58 L of nitrogen gas.
(b): Calculate the grams of N₂ in 5.03 × 10²⁰ moles of nitrogen gas.
(c): Calculate the moles of N₂ molecules in 3.94 grams of nitrogen gas.
(d): Calculate the moles of N₂ molecules in 4.73 L of nitrogen gas.
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A 100.00 mL volumetric flask weighs 35.9325 g. When an unknown solid is added to it, the flask and sample weigh 48.8565 g. Deionized water is added to the calibration mark. The flask, sample, and water together weigh 140.8321 g. Calculate the density of the unknown, assuming the density of water is 0.998203 g/mL.
Answer:
1.64 g/mL
Explanation:
Step 1: Calculate the mass of the solid
m(solid+flask) = m(solid) + m(flask)
m(solid) = m(solid+flask) - m(flask)
m(solid) = 48.8565 g - 35.9325 g = 12.9240 g
Step 2: Calculate the mass of water
m(solid+flask+water) = m(solid+flask) + m(water)
m(water) = m(solid+flask+water) - m(solid+flask)
m(water) = 140.8321 g - 48.8565 g = 91.9756 g
Step 3: Calculate the volume occupied by 91.9756 g of water
The density of water is 0.998203 g/mL.
91.9756 g × 1 mL/0.998203 g = 92.1412 mL
Step 4: Calculate the volume occupied by the solid
The 100.00 mL are occupied by the solid and the water.
100.00 mL = V(solid) + V(water
V(solid) = 100.00 mL - V(water)
V(solid) = 100.00 mL - 92.1412 mL = 7.86 mL
Step 5: Calculate the density of the solid
12.9240 g of the solid occupy 7.86 mL.
ρ = 12.9240 g/7.86 mL = 1.64 g/mL
Which of the following is considered a nucleon?
proton
neutron
All of the above
None of the above
m
Un cocodrilo se arrastró 25 m hacia la derecha con una velocidad promedio de –1.2 -.
¿Cuántos segundos se arrastró el cocodrilo?
Answer:
El cocodrilo se arrastró durante 20.833 segundos.
Explanation:
El enunciado presenta omisiones y errores conceptuales. La forma correcta es la siguiente: "Un cocodrilo se arrastró 25 metros hacia la derecha con una rapidez promedio de 1.2 metros por segundo. ¿Cuántos segundos se arrastró el cocodrilo?"
Consideremos que el cocodrilo tiene un movimiento rectilíneo uniforme, el tiempo requerido para el recorrido se calcula con la siguiente ecuación cinemática:
[tex]t = \frac{x}{v}[/tex] (1)
Donde:
[tex]x[/tex] - Distancia recorrida, en metros.
[tex]v[/tex] - Rapidez del cocodrilo, en metros por segundo.
[tex]t[/tex] - Tiempo, en segundos.
Si [tex]x = 25\,m[/tex] y [tex]v = 1.2\,\frac{m}{s}[/tex], entonces el tiempo empleado por el cocodrilo es:
[tex]t = \frac{25\,m}{1.2\,\frac{m}{s} }[/tex]
[tex]t = 20.833\,s[/tex]
El cocodrilo se arrastró durante 20.833 segundos.
Which element has a higher first ionization energy than chlorine (Cl)?
A. Argon (Ar)
B. Phosphorus (P)
C. Lithium (Li)
D. Iodine (I)
Answer:
Argon
Explanation:
It has more electron than chlorine
Rank these transition metal ions in order of decreasing number of unpaired electrons.
a. Fe^3
b. Mn^4+
c. V3+
d. Ni^2+
e. Cu^+
Answer: The given transition metal ions in order of decreasing number of unpaired electrons are as follows.
[tex]Mn^{4+} > V^{3+} = Ni^{2+} > Fe^{3+} > Cu^{+}[/tex]
Explanation:
In atomic orbitals, the distribution of electrons of an atom is called electronic configuration.
The electronic configuration in terms of noble gases for the given elements are as follows.
Atomic number of Fe is 26.[tex]Fe^{3+} - [Ar] 3d^{5}[/tex]
So, there is only 1 unpaired electron present in [tex]Fe^{3+}[/tex].
Atomic number of Mn is 25.[tex]Mn^{4+} - [Ar]3d^{3}[/tex]
So, there are only 3 unpaired electrons present in [tex]Mn^{4+}[/tex].
Atomic number of V is 23.[tex]V^{3+} - [Ar] 3d^{2}[/tex]
So, there are only 2 unpaired electrons present in [tex]V^{3+}[/tex].
Atomic number of Ni is 28.[tex]Ni^{2+} - [Ar] 3d^{8}[/tex]
So, there will be 2 unpaired electrons present in [tex]Ni^{2+}[/tex].
Atomic number of Cu is 29.[tex]Cu^{+} - [Ar] 3d^{10}[/tex]
So, there is no unpaired electron present in [tex]Cu^{+}[/tex].
Therefore, given transition metal ions in order of decreasing number of unpaired electrons are as follows.
[tex]Mn^{4+} > V^{3+} = Ni^{2+} > Fe^{3+} > Cu^{+}[/tex]
Thus, we can conclude that given transition metal ions in order of decreasing number of unpaired electrons are as follows.
[tex]Mn^{4+} > V^{3+} = Ni^{2+} > Fe^{3+} > Cu^{+}[/tex]
A suspension is
•A heterogenous mixture where the solid particles are large enough to be filtered out.
•A homogenous mixture where the solid particles are large enough to be filtered out.
•A heterogenous mixture where the solid particles are too small to be filtered out.
•A homogenous mixture where the solid particles are too small to be filtered out
Answer:
A heterogeneous mixture where the solids particles are large enough to be filtered out.
Explanation:
A certain liquid has a normal boiling point of and a boiling point elevation constant . A solution is prepared by dissolving some glycine () in of . This solution boils at . Calculate the mass of that was dissolved. Round your answer to significant digit.
The question is incomplete, the complete question is:
A certain substance X has a normal freezing point of [tex]-6.4^oC[/tex] and a molal freezing point depression constant [tex]K_f=3.96^oC.kg/mol[/tex]. A solution is prepared by dissolving some glycine in 950. g of X. This solution freezes at [tex]-13.6^oC[/tex] . Calculate the mass of urea that was dissolved. Round your answer to 2 significant digits.
Answer: The mass of glycine that can be dissolved is [tex]1.3\times 10^2g[/tex]
Explanation:
Depression in the freezing point is defined as the difference between the freezing point of the pure solvent and the freezing point of the solution.
The expression for the calculation of depression in freezing point is:
[tex]\text{Freezing point of pure solvent}-\text{freezing point of solution}=i\times K_f\times m[/tex]
OR
[tex]\text{Freezing point of pure solvent}=\text{Freezing point of solution}=i\times K_f\times \frac{m_{solute}\times 1000}{M_{solute}\times w_{solvent}\text{(in g)}}[/tex] ......(1)
where,
Freezing point of pure solvent = [tex]-6.4^oC[/tex]
Freezing point of solution = [tex]-13.6^oC[/tex]
i = Vant Hoff factor = 1 (for non-electrolytes)
[tex]K_f[/tex] = freezing point depression constant = [tex]3.96^oC/m[/tex]
[tex]m_{solute}[/tex] = Given mass of solute (glycine) = ?
[tex]M_{solute}[/tex] = Molar mass of solute (glycine) = 75.07 g/mol
[tex]w_{solvent}[/tex] = Mass of solvent = 950. g
Putting values in equation 1, we get:
[tex]-6.4-(-13.6)=1\times 3.96\times \frac{m_{solute}\times 1000}{75.07\times 950}\\\\m_{solute}=\frac{7.2\times 75.07\times 950}{1\times 3.96\times 1000}\\\\m_{solute}=129.66g=1.3\times 10^2g[/tex]
Hence, the mass of glycine that can be dissolved is [tex]1.3\times 10^2g[/tex]
Is Dioxin chemical ionic or covalent and acidic or basic? Explain
Answer:
Learning Objective Identify element pairs which are likely to form ionic or covalent bonds Key Points Ionic compounds are formed from strong electrostatic interactions between ions, which result in higher melting points and electrical conductivity compared to covalent compounds.Dioxins are a group of highly toxic chemical compounds that are harmful to health. They can cause problems with reproduction, development, and the immune system. They can also disrupt hormones and lead to cancer. Known as persistent environmental pollutants (POPs), dioxins can remain in the environment for many years. Covalent compounds have bonds where electrons are shared between atoms. Due to the sharing of electrons, they exhibit characteristic physical properties that include lower melting points and electrical conductivity compared to ionic compounds. Terms electronegativity: The tendency of an atom or molecule to attract electrons and form bonds. octet rule: Atoms lose, gain, or share electrons in order to have a full valence level of eight electrons. Hydrogen and helium are exceptions because they can hold a maximum of two valence electrons. valence electrons: Electrons in the outermost principal energy (valence) level of an atom that can participate in the formation of chemical bonds with other atoms. Two Classes of Compounds Compounds are defined as substances containing two or more different chemical elements. They have distinct chemical structures characterized by a fixed ratio of atoms held together by chemical bonds. Here, we discuss two classes of compounds based on the bond type that holds the atoms together: ionic and covalent. Covalent Compounds Covalent bonds are characterized by the sharing of electrons between two or more atoms. These bonds mostly occur between nonmetals or between two of the same (or similar) elements.Two atoms with similar electronegativity will not exchange an electron from their outermost shell; the atoms instead share electrons so that their valence electron shell is filled. Examples of compounds that contain only covalent bonds are methane (CH4), carbon monoxide (CO), and iodine monobromide (IBr). Ionic Compounds Ionic bonding occurs when there is a large difference in electronegativity between two atoms. This large difference leads to the loss of an electron from the less electronegative atom and the gain of that electron by the more electronegative atom, resulting in two ions. These oppositely charged ions feel an attraction to each other, and this electrostatic attraction constitutes an ionic bond. Ionic bonding occurs between a nonmetal, which acts as an electron acceptor, and a metal, which acts as an electron donor. Metals have few valence electrons, whereas nonmetals have closer to eight valence electrons; to easily satisfy the octet rule, the nonmetal will accept an electron donated by the metal. More than one electron can be donated and received in an ionic bond. Some examples of compounds with ionic bonding include NaCl, KI, MgCl2.Explanation:
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The diagram shows a food chain.
Which term best describes the green plant in the food chain?
antiter
A. Competitor
B. Producer
C. Consumer
D. Predator
Indica, con base en la siguiente ecuación:
HNO3 + H2S
NO + S + H30
a) Los números de oxidación de todos los átomos que forman cada compuesto
o elemento.
b) los átomos cuyo número de oxidación varía.
c) El elemento que se reduce y el que se oxida.
d) El agente oxidante y el agente reductor.
e) El átomo que gana electrones y el átomo que los pierde.
f) Los coeficientes apropiados para balancear la ecuación química.