In this question, we have to find the molar concentration of the acid, and the question already provides us with the formula and each required data:
MaVa = MbVb
We have:
Ma = ?
Va = 100 mL
Mb = 1.0 M
Vb = 25 mL
Now we add these values into the formula:
Ma * 100 = 1 * 25
100Ma = 25
Ma = 25/100
Ma = 0.25 M
How many grams of 12% solution can be prepared from 35 g of CaCl2
The question provides the concentration of a solution (12% CaCl2) and requests us to calculate how many grams of this solution could be prepared starting from 35g of CaCl2.
Since the concentration of solution is 12%, considering it refers to % in mass, we can write that 12g of CaCl are necessary to prepare 100 g of solution:
12 g of CaCl2 --------------- 100 g of solution
Thus, we can calculate how much solution could be prepared from 35 g of CaCl2:
12 g of CaCl2 --------------- 100 g of solution
35 g of CaCl2 -------------- x
Solving for x, we have that 291.67 g of solution could be prepared from 35g of CaCl2.
What is the concentration if I have 450 mL of iron (II) chloride (FeCl2) solution that contains9.6 grams of iron (II) chloride solute?
0.168M
Explanations:The formula for calculating the concentration of the solution is expressed as:
[tex]concentration=\frac{mole}{volume}[/tex]Determine the moles of iron(II) chloride
[tex]\begin{gathered} mole\text{ of FeCl}_2=\frac{9.6g}{126.751g\text{/}mol} \\ mole\text{ of FeCl}_2=0.0757moles \end{gathered}[/tex]Given that volume is 0.45L, hence the concentration is expressed as:
[tex]\begin{gathered} concentration=\frac{0.0757}{0.45} \\ concentration=0.168M \end{gathered}[/tex]Hence the concentration of the solution is 0.168M
Consider a gas at (3.420x10^2) kPa in a (7.6100x10^-1) L container at (1.8000x10^1)°C. What will thpressure of the gas be. if it is released into a room with a volume of (1.91x10^4) L and a temperature(1.3000x10^1)°C? Express your answer to three significant digits.
Answer
P2 = 9.84x10^-3 kPa
Explanation
Given:
Pressure 1 = 3.420x10^2 kPa
Volume 1 = 7.6100x10^-1 L
Temperature 1 = 1.8000x10^1 °C
Volume 2 = 1.91x10^4 L
Temperature 2 = 1.3000x10^1°C
Required: To calculate Pressure 2
Solution
We will use the combined gas law to solve this problem
[tex]\frac{P_1V_1}{T_1}\text{ = }\frac{P_2V_2}{T_2}[/tex]Re-arrange to make the subject P2:
P2 = P1V1T2/V2T1
P2 = (3.420x10^2 x 7.6100x10^-1 x 1.3000x10^1)/(1.91x10^4 x 1.8000x10^1)
P2 = 9.84x10^-3 kPa
Name the type of reaction below:
CaO + H2O →Ca(OH)2
CaO and H2O mix to form Ca(OH)2, a single chemical. It is a combination reaction as a result.
What is combination reaction ?When two or more elements or compounds combine to create a single product, the reaction is known as a direct combination reaction. Equations of the type X + Y. XY are used to depict these reactions.
A combination reaction occurs when two or more components combine to produce a single compound.
Combination reactions occur when two or more reactants come together to create a new product. Synthesis reaction is another name for combination reaction. For instance, hydrogen and chlorine can mix to form hydro-chloride.
Thus, CaO + H2O →Ca(OH)2 this reaction is combination reaction.
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convert 8 mol Na to grams
184g
Explanations:The formula for calculating the mass of a substance is expressed as;
[tex]moles=mass\times molar\text{ mass}[/tex]Given the following parameters
• Moles of Na = 8moles
,• Molar mass of Na = 23g/mol
Substitute the given parameter into the formula
[tex]\begin{gathered} Mass\text{ of Na}=moles\times molar\text{ mass} \\ Mass\text{ }of\text{ Na}=8moles\times\frac{23g}{mol} \\ Mass\text{ of Na}=184g \end{gathered}[/tex]Hence the mass of the sodium is 184g
How many moles of NaOH are in 21.4 mL of 1.29 M NaOH?
Answer:
n = 0.0276 mol
Explanation:
Required: Moles of NaOH
Given:
Volume of NaOH = 21.4 mL
Molarity/concentation = 1.29 M
Solution:
We will use the following equation to solve the problem:
[tex]C\text{ =}\frac{n}{V}[/tex]C is the concentration or molarity in mol/L or M, n is the number of moles in mol and V is the volume in L. Therefore we need to first convert mL to L.
1mL = 0.001 L
therefore 21.4 mL = 0.0214 L
Lets re-arrange the equation:
n = CV
n = 1.29 mol/L x 0.0214 L
n = 0.0276 mol
Balance the following half-reaction in acid (some electrons, e, will be needed to balance it):Fe²+ ——-> FeO4²-
The balanced half-reaction is Fe²⁺ + 2e⁻ --------> FeO₄²⁻
The given reaction is a redox reaction. Balancing a redox reaction is a bit different than solving a normal chemical reaction. The first step is to find the oxidation state of each element in the reactant as well as the product side. By doing so we get,
The oxidation state of Fe - +2
On the product side, we get,
The oxidation state of Fe - +6
The oxidation state of O - -2
The next step is to calculate the difference between the oxidation states.
The difference in oxidation state of Fe - +6 - (+2) = +4
The difference in oxidation state of O - 0 -2 = -2
To balance this reaction, 2 electrons should be added to the reactant side so that the oxidation states of O and Fe get balanced equally. By doing so we get,
Fe²⁺ + 2e⁻ --------> FeO₄²⁻
This is a balanced half-reaction in acid
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If 15.2g of aluminum reacts with 39.1g of chlorine, how many g of AlCl3 forms?
Answer:
74.9g of AlCl3 are formed.
Explanation:
1st) It is necessary to write and balance the chemical reaction:
[tex]2Al+3Cl_2\rightarrow2AlCl_3[/tex]From the balanced reaction, we know that 2 moles of Al react with 3 moles of Cl2 to produce 2 moles of AlCl3.
2nd) With the molar mass of Al and Cl2, we can convert the moles to grams:
- Al molar mass: 27g/mol
- Al conversion:
[tex]2moles*\frac{27g}{1mole}=54g[/tex]- Cl2 molar mass: 71g/mol
- Cl2 conversion:
[tex]3moles\frac{71g}{1mole}=213g[/tex]Now we know that from the balanced reaction, 54g of Al react with 213g of Cl2.
3rd) Now we have to find out which compound is the limiting reactant and which compound is the excess reactant:
[tex]\begin{gathered} 54gAl-213gCl_2 \\ 15.2gAl-x=\frac{15.2gAl*213gCl_2}{54gAl} \\ x=59.96gCl_2 \end{gathered}[/tex]Now we know that the 15.2g of Al will need 59.96g of Cl2, but we only have 39.1g of Cl2, so Cl2 is the limiting reactant and Al is the excess reactant.
4th) With the molar mass of AlCl3, we can convert the moles to grams of AlCl3:
- AlCl3 molar mass: 133g/mol
- AlCl3 conversion:
[tex]2moles*\frac{133g}{1mole}=266g[/tex]266g of AlCl3 are formed from the balanced reaction.
5th) Finally, with the limiting reactant and the grams of AlCl3 that must be produced from the balanced reaction, we can calculate the grams of AlCl3 that will be formed from 15.2g of aluminum:
[tex]\begin{gathered} 54gAl-266gAlCl_3 \\ 15.2gAl-x=\frac{15.2gAl*266gAlCl_3}{54gAl} \\ x=74.9gAlCl_3 \end{gathered}[/tex]So, 74.9g of AlCl3 are formed.
Please please help please please help me please please help
A single bond is made up of 1.0 sigma bond and no pi bonds.
Pi bonds appears from double bonds onwards.
16. Which of the following is directly responsible for acid rain? A. steam vented from a nuclear power plant B. sulfur dioxide released from a coal-fired power plant. C. mining of coal for a coal-fired power plant D. processing of uranium for a nuclear power plant
Answer
B. sulfur dioxide released from a coal-fired power plant.
Explanation
Power plants release the majority of sulfur dioxide and much of the nitrogen oxides when they burn fossil fuels, such as coal, to produce electricity. In addition, the exhaust from cars, trucks, and buses releases nitrogen oxides and sulfur dioxide into the air. These pollutants cause acid rain.
Therefore, what is directly responsible for acid rain is:
B. sulfur dioxide released from a coal-fired power plant.
What is the phase of water at 0.25 atm and 0°C?A. GasB. Solid and liquidC. Solid and gasD. Solid
Explanation:
We have to find the phase of water at 0.25 atm and 0°C. If we look at the phase diagram of water and throw the lines we will find that the phase of water at those conditions is solid.
Answer: d. Solid
Which of the following best describes an ecosystem in the Great Lakes?
The statement " all the living organisms in an area and their physical surroundings " will describes an ecosystem in the Great Lakes.
A biological combination of cooperating organisms and surrounding physical environment can be referred to as an ecosystem.
A system made up of biotic and abiotic elements that work together as a whole is called an ecosystem. All live things are considered to be biotic components, although non-living items are considered to be abiotic components.
Therefore, "all the living organisms in an area and their physical surroundings " will define ecosystem in the Great Lakes.
The given question is incomplete. The complete question is
Which of the following best describes an ecosystem?
A. all the living organisms in an area
B. all the living organisms in an area and their physical surroundings
C. a region with a distinct climate
D. all the living organisms of the same species throughout the world
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A testing chamber holds a 2.50 L sample of neon gas at 325.0 K.If the pressure is measured inside the chamber as 4.00 atm, how many moles of neon are present?0.4530.44200.3750.326
Answer: There are 0.375 moles of neon gas present in the testing chamber.
Explanation:
The question requires us to calculate the number of moles of neon gas, given that the gas is in a 2.50 L chamber at 325.0 K and the pressure inside the chamber is 4.00 atm.
We can solve this problem using the equation for ideal gases, as shown below:
[tex]PV=nRT[/tex]where P is the pressure of the gas (P = 4.00 atm), V is the volume of the gas (V = 2.50 L), n is the number of moles, that we want to calculate, T is the temperature of the gas (T = 325.0 K) and R is the gas constant.
Note that the values of pressure and volume are given in atm and L, respectively. Therefore, we can apply the gas constant in units of L.atm/mol.K:
R = 0.082057 L.atm/K.mol
First, let's rearrange the equation of ideal gases in order to calculate the number of moles of gas:
[tex]PV=nRT\rightarrow n=\frac{PV}{RT}[/tex]Now, applying the values given by the question and the constant R, we'll have:
[tex]n=\frac{(4.00atm)\times(2.50L)}{(0.082057L.atm/K.mol)\times(325.0K)}=0.375mol[/tex]Therefore, there are 0.375 moles of neon gas in the testing chamber under the conditions given by the question.
Write a net ionic equation for this reaction.Express your answer as a chemical equation. Identify all of the phases in your answer.ANSWER:
Given the reaction:
[tex]2HNO_3+Ca(OH)_2\to Ca(NO_3)_2+2H_2O[/tex]We're going to write a net ionic equation for this reaction as follows:
1. First, write the total ionic equation:
[tex]^{}Ca^{2+}_{aq}+2OH^-_{aq}+2H^+_{aq_{}}+2NO^-_3\to^{}Ca^{2+}_{aq}+2NO^-_3+2H_2O[/tex]2. Now, we could cancel the same type of ions that are in both sides of the reaction. Therefore, the net ionic equation is:
[tex]H^+_{aq}+^{}OH^-_{aq}\to H_2O_{(l)}[/tex]I have 5 questions that need help to answer 1) What are covalent bonds and how do they form ? 2) How do you know which elements and how many of each are in a compound ?
3) How can you find how many valence electrons an atom has ?
4) How many valence electrons do atoms need to be happy? Which elements are the exceptions?
A covalent bond is one that is formed by two non-metal elements that, due to their low electronegativity difference, neither has the energy to steal the electrons from the other, so they share electrons with each other.
Covalent bonds form when the electronegativity difference between two elements is less than 1.7. In addition, the number of elements must be such that by sharing their electrons, all elements comply with the octet rule, that is, each element shares and completes 8 valence electrons.
When the combustion engine was invented it had many positive effects on society. In 1938
scientists concluded that burning fossil fuels would cause which disastrous effect to the
environment?
A. climate change
B. the ozone layer to dissipate
C. increased deforestation
D. increased flooding
answer: The burning of fossil fuels leads to climate change so the correct answer is option D
Explanation: Burning fossil fuels releases a large amount of co2 into the atmosphere. C02 is a greenhouse gas so it traps the sun's heat this, in turn, heats up our atmosphere which leads to climate change.
now option B is wrong because the ozone layer is depleted due to ozone-depleting substances which when it comes to contact with ozone damage it and option c is due to human activities
finally, option d is due to climate change and this is an indirect effect of burning fossil fuels.
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what type of reaction is Propane + O2 - Co2 + H2O
Answer: This is a perfect example of a combustion reaction because we have a carbon based compound reaction with oxygen gas to produce carbon dioxide and water. Hopefully this helps!
Explanation:
If the initial concentration of a 400 ml solution is 7% and the solution is diluted down to a concentration of 4.5%, what will the new volume of the solution be?
We have that the dilution equation of concentrated solutions will be equal to:
[tex]C_1V_1=C_2V_2[/tex]where,
C1 is the initial concentration of the solution = 7%
V1 is the initial volume = 400mL
C2 is the final concentration = 4.5%
V2 is the final volume = ?
We clear Ve and replace the known data:
[tex]\begin{gathered} V_2=\frac{C_1V_1}{C_2} \\ V_2=\frac{7\%\times400mL}{4.5\%}=622mL \end{gathered}[/tex]Answer: the new volume of the solution will be 622 mL
A person has a sample of gas with a volume of 9.02L and a temperature of 585.57k. If the volume of the container is reduced to 2.24L, what will the new temperature of the gas be in Kelvin?
Step 1 - Understanding the relation between volume and temperature for a gas sample
There are three main variables that can change the state of a gas sample: temperature, pressure and volume. If the pressure (P) is kept constant, the volume (V) becomes proportional to the temperature (T) in K:
[tex]\frac{V_1}{T_1}=\frac{V_2}{T_2}[/tex]Step 2 - Substituting the values in the equation above
We know, from the exercise, that V1 = 9.02 L and T1 = 585.57 K, and V2=2.24 L. Substituting these values in the equation above:
[tex]\begin{gathered} \frac{9.02}{585.57}=\frac{2.24}{T_2} \\ \\ T_2=\frac{2.24\times585.57}{9.02}= \end{gathered}[/tex]Using the ΔH -48.8 kJ/mmol, calculate the enthalpy change if you neutralized six moles of HCl with an equal number of moles NaOH to one decimal place.
-292.8J/mmol
Explanations:Given the reaction of NaCl and NaOH expressed by the chemical equation:
[tex]6HCl+6NaOH\rightarrow6NaCl+6H_2O[/tex]Amount of heat released when one mole of strong acid reacts with one mole of the strong base is -48.8 kJ/mmol.
If 6 moles of the sample acid reacts with 6 moles of NaOH, the required enthalpy cheange is expressed as:
[tex]\begin{gathered} Amount\text{ of heat released }=6\times-48.8 \\ Amount\text{ of heat released}=-292.8kJ\text{/mmol} \end{gathered}[/tex]Hence the enthalpy change if you neutralized six moles of HCl with an equal number of moles NaOH is -292.8J/mmol
What mass of oxygen is needed to burn 54.0 g of butane
Answer
The mass of oxygen needed to burn 54.0g of butane is 193.24 g
Explanation
Given:
Mass of butane = 54.0 g
What to find:
The mass of oxygen needed to burn 54.0g of butane.
Step-by-step solution:
Step 1: Write the balanced chemical equation for the reaction.
2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O
Step 2: Convert 54.0 g of butane to moles
Molar mass of C₄H₁₀ = 58.12 g/mol
[tex]Moles=\frac{Mass}{Molar\text{ }mass}=\frac{54.0\text{ }g}{58.12\text{ }g\text{/}mol}=0.9291\text{ }mol[/tex]Step 3: Use the mole ratio in step one and the mole of C₄H₁₀ in step 2 to calculate the mole of oxygen.
[tex]\begin{gathered} 13\text{ }mol\text{ }O_2=2\text{ }mol\text{ }C_4H_{10} \\ \\ x=0.9291\text{ }mol\text{ }C_4H_{10} \\ \\ x=\frac{0.9291\text{ }mol\text{ }C_4H_{10}}{2\text{ }mol\text{ }C_4H_{10}}\times13\text{ }mol\text{ }O_2 \\ \\ x=6.03915\text{ }mol\text{ }O_2 \end{gathered}[/tex]Step 4: Convert the moles of O₂ in step 3 to mass in grams.
Molar mass of O₂ = 31.998 g/mol
[tex]\begin{gathered} Mass=Moles\times Molar\text{ }mass \\ \\ Mass=6.03915mol\times31.998g\text{/}mol \\ \\ Mass=193.24\text{ }g\text{ }of\text{ }O_2 \end{gathered}[/tex]Hence, the mass of oxygen needed to burn 54.0g of butane is 193.24 g
Convert 960 Torr to kPa
Step 1
Torr and kPa are units of pressure
---------
Step 2
The equivalence:
760 torr = 101325 Pa
1 kPa = 1000 Pa
Procedure:
960 Torr x (101325 Pa/760 Torr) = 127989.47 Pa
Then, 127989.47 Pa x (1 kPa/1000 Pa) = 128 kPa approx.
Answer: Pressure = 128 kPa
Which of the following describes a unique property of water that helps sustain marine life? It freezes upward from the bottom unlike other liquids that freeze downward from the top. It has a lower density in its solid state than it does in its liquid state. It shows changes in density at temperatures above 4 °C. It cools faster and heats up faster than most other liquids.
Answer:
It has a lower density in its solid state than it does in its liquid state
Explanation:
Here, we want to get the unique property of water that helps sustain marine life
As we know, the marine environment consists of several zones with different states. However, it is necessary that aquatic lives are supported in all zones.
In cases where we have a solid state of water, which is ice, aquatic organisms are expected to thrive. Now, the density of water matters in these states.
The density of water is lower in the solid state than in the liquid state, which is unusual for most other liquids. This unique property ensures the sustenance of aquatic lives
If something is made of 2.1 g Ni and 0.58 g O, what is the empirical formula?
To know the empirical formula we will determine how many moles of each element we have. To do this, we must look up in the periodic table the atomic weight of each element.
The atomic weight of Ni = 58.6934 g/mol
O = 15.999 g/mol
Now we divide the mass of each element by its atomic weight to determine how many moles are in the sample.
[tex]\begin{gathered} \text{Mol of Ni = }\frac{\text{Mass of Ni}}{\text{Atomic weight}} \\ Mol\text{ of Ni = }\frac{\text{2.1 g}}{58.6934\text{ g/mol}}=0.036\text{ mol of Ni} \end{gathered}[/tex][tex]\begin{gathered} \text{Mol of O = }\frac{Mass\text{ of O}}{\text{Atomic weight}} \\ \text{Mol of O = }\frac{0.\text{58 g}}{15.999\text{ g/mol}}=\text{ 0.036 mol of O} \end{gathered}[/tex]In the sample, there are 0.036 moles of oxygen and 0.036 moles of Ni. The ratio is 1 to 1, so the empirical formula will be: NiO
The mole fraction of NaCl in anaqueous solution is 0.132. Howmany moles of water are present in1 mole of this solution?Molar MassNaCl: 58.44 g/molH2O: 18.016 g/mol
The problem is asking for how many moles of water there are in 1 mol of solution with NaCl. This is telling us that NaCl is dissolved in water.
There are 0.132 moles of NaCl and summing the moles of water, we're going to obtain 1 mol of solution. You can see it, like this:
[tex]\text{0}.132\text{ moles NaCl+X moles water = 1 mol solution.}[/tex]We just have to clear for 'X moles water', and we obtain:
[tex]X\text{ moles water = 1-0.132 = 0.868 moles water.}[/tex]The answer is that we have 0.868 moles of water in the solution.
QUESTION 2How many moles are in 37.16 g of calcium sulfate,CaSO4
In order to find the number of moles in a given mass of any compound, we need to use the molar mass of this compound, which is the total mass present in 1 mol of the compound. The molar mass of CaSO4 is 136.14g/mol
136.14 grams = 1 mol of CaSO4
37.16 grams = x moles of CaSO4
136.14x = 37.16
x = 37.16/136.14
x = 0.27 moles of CaSO4
In 37.16 grams, we will have 0.27 moles of CaSO4
Lakeshea analyzed 6.234 grams of a substance and found it to be composed of 4.980 g of carbon and 1.254 g of hydrogen. In the next lab group, Niles analyzed another sample of the same substance and found 4.004 g of carbon.
A) How much hydrogen did Niles find in his sample
B) What is the justification(what law: Conservation of mass, Definite Proportions, Multiple Proportions) for your answer?
Lakeshea analyzed 6.234 grams of a substance and found it to be composed of 4.980 g of carbon and 1.254 g of hydrogen. Niles analyzes another sample of the same substance containing 4.004 g of carbon. A) hydrogen did Niles find in his sample is 2.23 g. B) The justification is the law of conservation of mass.
According to the law of mass of conservation of mass : mass neither be created nor be destroyed. so, that if sample is of 6.234 g contain 4.980 g carbon and 1.254 g hydrogen then the same sample if contain 4.004 g of carbon then the hydrogen will be 2.23 g of hydrogen.
Thus, Lakeshea analyzed 6.234 grams of a substance and found it to be composed of 4.980 g of carbon and 1.254 g of hydrogen. Niles analyzes another sample of the same substance , containing 4.004 g of carbon. A) hydrogen did Niles find in his sample is 2.23 g. B) The justification is the law of conservation of mass.
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neutral atoms contain equal numbers of
Answer:
protons and electrons
Explanation:
4 N2H3CH3 (l) + 5 N2O4 (l) →12 H2O(g) + 9 N2(g) + 4 CO2 (g)The enthalpy of formation for liquid methylhydrazine is +53 kJ/mol and the enthalpy of formation for liquid dinitrogen tetroxide is -20 kJ/mol. Calculate ∆H° for this reaction, ignore significant digits for this question.
Answer
[tex]\Delta H_{rxn}\operatorname{\degree}=-4791.6\text{ }kJ\text{/}mol[/tex]Explanation
The given chemical equation for the reaction is:
[tex]4N_2H_3CH_3(l)+5N_2O_4(l)\text{ }→\text{ }12H_2O\left(g\right)+9N_2\left(g\right)+4CO_2(g)[/tex]From the given table and question, the enthalpies of formation of the reactants ad products are:
[tex]\begin{gathered} ∆H_f°(N_2H_3CH_{3(l)})=+53\text{ }kJ\text{/}mol \\ \\ ∆H_f°(N_2O_{4(l)})=-20\text{ }kJ\text{/}mol \\ \\ ∆H_f°(H_2O_{(g)})=-258.8\text{ }kJ\text{/}mol \\ \\ ∆H_f°(N_{2(g)})=0\text{ }kJ\text{/}mol \\ \\ ∆H_f°(CO_{2(g)})=-393.5\text{ }kJ\text{/}mol \end{gathered}[/tex]The ∆H° for this reaction can be calculated using the formula below:
[tex]\Delta H_{rxn}\degree=ΔH_f^{\degree}(products)-ΔH_f^{\degree}(reactants)[/tex]Put the each enthalpy of formation of the reactants and the products into the formula:
[tex]\begin{gathered} \Delta H_{rxn}\degree=[12(-258.8)+9(0)+4(-393.5)]-[4(+53)+5(-20)] \\ \\ \Delta H_{rxn}\degree=[-3105.6+0-1574]-[212-100] \\ \\ \Delta H_{rxn}\degree=-4679.6-112 \\ \\ \Delta H_{rxn}\degree=-4791.6\text{ }kJ\text{/}mol \end{gathered}[/tex]Therefore, the ∆H° for this reaction is -4791.6 kJ/mol.
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Rb+
Fe2+
H-
Al3+
Cl-
O2-
Using the ions above, write the formulas and give the names for 5 possible ionic compounds involving these ions.
The formulas and and the names for 5 possible ionic compounds involving these ions are :
Rb₂O, Rubidium Oxide
FeCl₂, Iron(II)chloride
Al(OH)₃ , Aluminum hydroxide
LiH, Lithium Hydride
NaCl, Sodium chloride
1) The Rb₂O is called as Rubidium oxide. rubidium oxide is an ionic compound. Ionic compound formed between a positive ion called cation and a negative ion called anion . ionic bond is formed with the complete transfer of electrons. In Rubidium oxide : the cation is Rb⁺ and the anion is O²⁻.
2) The FeCl₂ is called as iron(II)chloride. iron(II)chloride is an ionic compound. in iron(II)chloride : the cation is Fe²⁺ and the anion is Cl⁻.
3) Al(OH)₃ is aluminum hydroxide . In aluminum hydroxide : the cation is present as Al³⁺ and anion is present as OH⁻.
4) LiH is lithium hydride . the cation is Li⁺ and the anion is H⁻.
5) NaCl is sodium chloride. cation is Na⁺ and anion is Cl⁻
Thus, The formulas and and the names for 5 possible ionic compounds involving these ions. Rb₂O, Rubidium Oxide
FeCl₂, Iron(II)chloride
Al(OH)₃ , Aluminum hydroxide
LiH, Lithium Hydride
NaCl, Sodium chloride
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