Question 1

How many millilitres of a 9.0 mol L^-1 H₂SO₄ solution are needed to make 0.35 L of a 3.5 mol L^-1 solution?

Accepted Answer

We can use the equation:

M1V1 = M2V2

where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration, and V2 is the final volume.

We want to find the initial volume, V1, of the 9.0 mol/L solution.

Rearranging the equation, we get:

V1 = M2V2/M1

Plugging in the values:

V1 = (3.5 mol/L)(0.35 L)/(9.0 mol/L) = 0.136 L = 136 mL

Therefore, we need 140 mL (rounded to the nearest tenth) of the 9.0 mol/L solution.

The answer is C, 140 mL.

Question 2

What is the concentration of an AlCl₃ solution if 150.mL of the solution contains 450.mg of Cl^- ion?

Accepted Answer

The answer of What is the concentration of an AlCl₃...

Question 3

How many grams of CH₃ OH must be added to water to prepare 150 mL of a solution that is 2.0 mol L^-1 CH₃ OH?

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The answer of How many grams of CH₃ OH must...

Question 4

Balance the chemical equation given below,and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25 °C.The density of nitrogen monoxide at $25 ^ { \circ } \mathrm { C }$ is 1.23 g L^-1. ________ NH₃(g)+ ________ O₂(g)? ________ NO(g)+ ________ H₂O(l)

Accepted Answer

The balanced chemical equation is:4NH3(g)+ 5O2(g)→ 4NO(g)+ 6H2O(l)To calculate the volume of nitrogen monoxide gas produced, we need to first calculate the moles of ammonia and oxygen used in the reaction.Moles of ammonia = 8.00 g / 17.03 g/mol = 0.470 molMoles of oxygen = 12.0 g / 32.00 g/mol = 0.375 molFrom the balanced chemical equation, we can see that 4 moles of ammonia react with 5 moles of oxygen. Therefore, the limiting reactant in this reaction is oxygen.Moles of nitrogen monoxide produced = 0.375 mol * (4 mol NO / 5 mol O2) = 0.300 molVolume of nitrogen monoxide produced = 0.300 mol * 22.4 L/mol = 6.72 LHowever, the density of nitrogen monoxide at 25 °C is 1.23 g L-1. Therefore, the volume of nitrogen monoxide gas produced at 25 °C is:Volume of nitrogen monoxide produced = 6.72 L * (1.23 g L-1 / 1 g L-1) = 8.26 LTherefore, the correct answer is A) 7.32 L.

Question 5

How many millilitres of 0.260 mol L^-1 Na₂S are needed to react with 40.00 mL of 0.315 mol L^-1 AgNO₃? Na₂S(aq)+ 2AgNO₃(aq)→ 2NaNO₃(aq)+ Ag₂S(s)

Accepted Answer

The answer of How many millilitres of 0.260 mol L^-1...

Question 6

How many millilitres of a stock solution of 13.1 mol L^-1 $\mathrm { HNO } _ { 3 }$ would be needed to prepare 0.500 L of 0.500 mol L^-1 $\mathrm { HNO } _ { 3 }$ ?

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The answer of How many millilitres of a stock solution...

Question 7

What is the concentration of NO₃^- ions in a solution prepared by dissolving 25.0 g of Ca(NO₃)₂ in enough water to produce 300.mL of solution?

Accepted Answer

The answer of What is the concentration of NO₃^- ions...

Question 8

How many grams of NaOH (MW = 40.0)are there in 250.0 mL of a 0.275 mol L^-1 NaOH solution?

Accepted Answer

The answer of How many grams of NaOH (MW =...

Question 9

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K₃PO₄ in enough water to make 350.mL of solution?

Accepted Answer

The answer of If the reaction of phosphate ion with...

Question 10

What is the molar concentration of sodium ions in a 0.450 mol L^-1 Na₃PO₄ solution?

Accepted Answer

The answer of What is the molar concentration of sodium...

Question 11

Calculate the concentration (M)of sodium ions in a solution made by diluting 80.0 mL of a 0.174 mol L^-1 solution of sodium sulfide to a total volume of 125 mL.

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The answer of Calculate the concentration (M)of sodium ions in...

Question 12

What is the concentration of HCl in the final solution when 65 mL of a 12 mol L^-1 HCl solution is diluted with pure water to a total volume of 0.15 L?

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The answer of What is the concentration of HCl in...

Question 13

Pure acetic acid ( $\mathrm { HC } _ { 2 }$ $\mathrm { H } _ { 3 }$ $\mathrm { O } _ { 2 }$ )is a liquid and is known as glacial acetic acid.Calculate the molarity of a solution prepared by dissolving 50.00 mL of glacial acetic acid at 25 °C in sufficient water to give 500.0 mL of solution.The density of glacial acetic acid at 25 °C is 1.05 g mL^-1.

Accepted Answer

To find the molarity, first calculate the mass of acetic acid using its volume and density: $50.00 \, \text{mL} \times 1.05 \, \text{g/mL} = 52.5 \, \text{g}$. Then, convert the mass to moles using the molar mass of acetic acid ($60.05 \, \text{g/mol}$): $52.5 \, \text{g} / 60.05 \, \text{g/mol} = 0.874 \, \text{mol}$. Finally, divide the moles by the volume of the solution in liters to find the molarity: $0.874 \, \text{mol} / 0.500 \, \text{L} = 1.75 \, \text{mol/L}$.

Question 14

A stock solution of $\mathrm { HNO } _ { 3 }$ is prepared and found to contain 13.7 mol L^-1 of $\mathrm { HNO } _ { 3 }$ .If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L,what is the concentration of the diluted solution?

Accepted Answer

The answer of A stock solution of \(\mathrm { HNO...

Question 15

A FeCl₃ solution is 0.175 mol L^-1.How many mL of a 0.175 mol L^-1 FeCl₃solution are needed to make 450.mL of a solution that is 0.300 mol L^-1 in Cl^- ion?

Accepted Answer

The answer of A FeCl₃ solution is 0.175 mol L^-1.How...

Question 16

How many moles of Co²⁺ are present in 0.150 L of a 0.200 mol L^-1 solution of CoI₂?

Accepted Answer

The answer of How many moles of Co²⁺ are present...

Question 17

A student dissolved 4.00 g of Co(NO₃)₂ in enough water to make 100.mL of stock solution.He took 4.00 mL of the stock solution and then diluted it with water to give 275.mL of a final solution.How many grams of NO₃^- ion are there in the final solution?

Accepted Answer

The answer of A student dissolved 4.00 g of Co(NO₃)₂...

Question 18

A student prepared a stock solution by dissolving 10.0 g of KOH in enough water to make 150.mL of solution.She then took 15.0 mL of the stock solution and diluted it with enough water to make 65.0 mL of a final solution.What is the concentration of KOH for the final solution?

Accepted Answer

First, we need to calculate the molarity of the stock solution:
moles of KOH = mass/molar mass = 10.0 g/56.11 g/mol = 0.178 mol
Molarity = moles/volume = 0.178 mol/0.150 L = 1.19 mol/L

Next, we can use the dilution formula to find the concentration of the final solution:
M1V1 = M2V2
where M1 = molarity of the stock solution, V1 = volume of the stock solution used, M2 = concentration of the final solution, and V2 = volume of the final solution.

Plugging in the values, we get:
(1.19 mol/L)(15.0 mL) = M2(65.0 mL)
M2 = (1.19 mol/L)(15.0 mL)/(65.0 mL) = 0.274 mol/L

Therefore, the concentration of KOH for the final solution is 0.274 mol/L, which is closest to choice A.

Question 19

How many grams of CaCl₂ are formed when 15.00 mL of 0.00237 mol L^-1 Ca(OH)₂ reacts with excess Cl₂ gas? 2Ca(OH)₂(aq)+ 2Cl₂(g)→ Ca(OCl)₂(aq)+ CaCl₂(s)+ 2H₂O(l)

Accepted Answer

The answer of How many grams of CaCl₂ are formed...

Question 20

There are ________ mol of bromide ions in 0.900 L of a 0.500 mol L^-1 solution of Al $\mathrm { Br } _ { 3 }$ .

Accepted Answer

The answer of There are ________ mol of bromide ions...

Quiz 4: Chemical Reactions and Stoichiometry

How many millilitres of a 9.0 mol L^-1 H₂SO₄ solution are needed to make 0.35 L of a 3.5 mol L^-1 solution?

What is the concentration of an AlCl₃ solution if 150.mL of the solution contains 450.mg of Cl^- ion?

How many grams of CH₃ OH must be added to water to prepare 150 mL of a solution that is 2.0 mol L^-1 CH₃ OH?

Balance the chemical equation given below,and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25 °C.The density of nitrogen monoxide at $25 ^ { \circ } \mathrm { C }$ is 1.23 g L^-1. NH₃(g) + O₂(g) ? NO(g) + H₂O(l)

How many millilitres of 0.260 mol L^-1 Na₂S are needed to react with 40.00 mL of 0.315 mol L^-1 AgNO₃? Na₂S(aq) + 2AgNO₃(aq) → 2NaNO₃(aq) + Ag₂S(s)

How many millilitres of a stock solution of 13.1 mol L^-1 $\mathrm { HNO } _ { 3 }$ would be needed to prepare 0.500 L of 0.500 mol L^-1 $\mathrm { HNO } _ { 3 }$ ?

What is the concentration of NO₃^- ions in a solution prepared by dissolving 25.0 g of Ca(NO₃) ₂ in enough water to produce 300.mL of solution?

How many grams of NaOH (MW = 40.0)are there in 250.0 mL of a 0.275 mol L^-1 NaOH solution?

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K₃PO₄ in enough water to make 350.mL of solution?

What is the molar concentration of sodium ions in a 0.450 mol L^-1 Na₃PO₄ solution?

Calculate the concentration (M)of sodium ions in a solution made by diluting 80.0 mL of a 0.174 mol L^-1 solution of sodium sulfide to a total volume of 125 mL.

What is the concentration of HCl in the final solution when 65 mL of a 12 mol L^-1 HCl solution is diluted with pure water to a total volume of 0.15 L?

A stock solution of $\mathrm { HNO } _ { 3 }$ is prepared and found to contain 13.7 mol L^-1 of $\mathrm { HNO } _ { 3 }$ .If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L,what is the concentration of the diluted solution?

A FeCl₃ solution is 0.175 mol L^-1.How many mL of a 0.175 mol L^-1 FeCl₃solution are needed to make 450.mL of a solution that is 0.300 mol L^-1 in Cl^- ion?

How many moles of Co²⁺ are present in 0.150 L of a 0.200 mol L^-1 solution of CoI₂?

A student dissolved 4.00 g of Co(NO₃) ₂ in enough water to make 100.mL of stock solution.He took 4.00 mL of the stock solution and then diluted it with water to give 275.mL of a final solution.How many grams of NO₃^- ion are there in the final solution?

A student prepared a stock solution by dissolving 10.0 g of KOH in enough water to make 150.mL of solution.She then took 15.0 mL of the stock solution and diluted it with enough water to make 65.0 mL of a final solution.What is the concentration of KOH for the final solution?

How many grams of CaCl₂ are formed when 15.00 mL of 0.00237 mol L^-1 Ca(OH) ₂ reacts with excess Cl₂ gas? 2Ca(OH) ₂(aq) + 2Cl₂(g) → Ca(OCl) ₂(aq) + CaCl₂(s) + 2H₂O(l)

There are ________ mol of bromide ions in 0.900 L of a 0.500 mol L^-1 solution of Al $\mathrm { Br } _ { 3 }$ .

Quiz 4: Chemical Reactions and Stoichiometry

How many millilitres of a 9.0 mol L-1 H2SO4 solution are needed to make 0.35 L of a 3.5 mol L-1 solution?

What is the concentration of an AlCl3 solution if 150.mL of the solution contains 450.mg of Cl- ion?

How many grams of CH3 OH must be added to water to prepare 150 mL of a solution that is 2.0 mol L-1 CH3 OH?

How many millilitres of 0.260 mol L-1 Na2S are needed to react with 40.00 mL of 0.315 mol L-1 AgNO3? Na2S(aq) + 2AgNO3(aq) → 2NaNO3(aq) + Ag2S(s)

How many millilitres of a stock solution of 13.1 mol L-1 HNO3\mathrm { HNO } _ { 3 }HNO3​ would be needed to prepare 0.500 L of 0.500 mol L-1 HNO3\mathrm { HNO } _ { 3 }HNO3​ ?

What is the concentration of NO3- ions in a solution prepared by dissolving 25.0 g of Ca(NO3) 2 in enough water to produce 300.mL of solution?

How many grams of NaOH (MW = 40.0)are there in 250.0 mL of a 0.275 mol L-1 NaOH solution?

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K3PO4 in enough water to make 350.mL of solution?

What is the molar concentration of sodium ions in a 0.450 mol L-1 Na3PO4 solution?

Calculate the concentration (M)of sodium ions in a solution made by diluting 80.0 mL of a 0.174 mol L-1 solution of sodium sulfide to a total volume of 125 mL.

What is the concentration of HCl in the final solution when 65 mL of a 12 mol L-1 HCl solution is diluted with pure water to a total volume of 0.15 L?

A stock solution of HNO3\mathrm { HNO } _ { 3 }HNO3​ is prepared and found to contain 13.7 mol L-1 of HNO3\mathrm { HNO } _ { 3 }HNO3​ .If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L,what is the concentration of the diluted solution?

A FeCl3 solution is 0.175 mol L-1.How many mL of a 0.175 mol L-1 FeCl3 solution are needed to make 450.mL of a solution that is 0.300 mol L-1 in Cl- ion?

How many moles of Co2+ are present in 0.150 L of a 0.200 mol L-1 solution of CoI2?

A student dissolved 4.00 g of Co(NO3) 2 in enough water to make 100.mL of stock solution.He took 4.00 mL of the stock solution and then diluted it with water to give 275.mL of a final solution.How many grams of NO3- ion are there in the final solution?

A student prepared a stock solution by dissolving 10.0 g of KOH in enough water to make 150.mL of solution.She then took 15.0 mL of the stock solution and diluted it with enough water to make 65.0 mL of a final solution.What is the concentration of KOH for the final solution?

How many grams of CaCl2 are formed when 15.00 mL of 0.00237 mol L-1 Ca(OH) 2 reacts with excess Cl2 gas? 2Ca(OH) 2(aq) + 2Cl2(g) → Ca(OCl) 2(aq) + CaCl2(s) + 2H2O(l)

There are ________ mol of bromide ions in 0.900 L of a 0.500 mol L-1 solution of Al Br3\mathrm { Br } _ { 3 }Br3​ .

How many millilitres of a 9.0 mol L^-1 H₂SO₄ solution are needed to make 0.35 L of a 3.5 mol L^-1 solution?

What is the concentration of an AlCl₃ solution if 150.mL of the solution contains 450.mg of Cl^- ion?

How many grams of CH₃ OH must be added to water to prepare 150 mL of a solution that is 2.0 mol L^-1 CH₃ OH?

How many millilitres of 0.260 mol L^-1 Na₂S are needed to react with 40.00 mL of 0.315 mol L^-1 AgNO₃? Na₂S(aq) + 2AgNO₃(aq) → 2NaNO₃(aq) + Ag₂S(s)

How many millilitres of a stock solution of 13.1 mol L^-1 $\mathrm { HNO } _ { 3 }$ would be needed to prepare 0.500 L of 0.500 mol L^-1 $\mathrm { HNO } _ { 3 }$ ?

What is the concentration of NO₃^- ions in a solution prepared by dissolving 25.0 g of Ca(NO₃) ₂ in enough water to produce 300.mL of solution?

How many grams of NaOH (MW = 40.0)are there in 250.0 mL of a 0.275 mol L^-1 NaOH solution?

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K₃PO₄ in enough water to make 350.mL of solution?

What is the molar concentration of sodium ions in a 0.450 mol L^-1 Na₃PO₄ solution?

Calculate the concentration (M)of sodium ions in a solution made by diluting 80.0 mL of a 0.174 mol L^-1 solution of sodium sulfide to a total volume of 125 mL.

What is the concentration of HCl in the final solution when 65 mL of a 12 mol L^-1 HCl solution is diluted with pure water to a total volume of 0.15 L?

A stock solution of $\mathrm { HNO } _ { 3 }$ is prepared and found to contain 13.7 mol L^-1 of $\mathrm { HNO } _ { 3 }$ .If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L,what is the concentration of the diluted solution?

A FeCl₃ solution is 0.175 mol L^-1.How many mL of a 0.175 mol L^-1 FeCl₃solution are needed to make 450.mL of a solution that is 0.300 mol L^-1 in Cl^- ion?

How many moles of Co²⁺ are present in 0.150 L of a 0.200 mol L^-1 solution of CoI₂?

A student dissolved 4.00 g of Co(NO₃) ₂ in enough water to make 100.mL of stock solution.He took 4.00 mL of the stock solution and then diluted it with water to give 275.mL of a final solution.How many grams of NO₃^- ion are there in the final solution?

How many grams of CaCl₂ are formed when 15.00 mL of 0.00237 mol L^-1 Ca(OH) ₂ reacts with excess Cl₂ gas? 2Ca(OH) ₂(aq) + 2Cl₂(g) → Ca(OCl) ₂(aq) + CaCl₂(s) + 2H₂O(l)

There are ________ mol of bromide ions in 0.900 L of a 0.500 mol L^-1 solution of Al $\mathrm { Br } _ { 3 }$ .