Question 1

What volume of 0.305 mol L^-1 AgNO₃ is required to react exactly with 155.0 mL of 0.274 mol L^-1 Na₂SO₄ solution? Hint: You will want to write a balanced reaction.

Accepted Answer

The answer of What volume of 0.305 mol L^-1 AgNO₃...

Question 2

What mass (in g)of AgCl is formed from the reaction of 75.0 mL of a 0.078 mol L^-1 AgC₂H₃O₂ solution with 55.0 mL of a 0.109 mol L^-1 MgCl₂ solution? 2AgC₂H₃O₂(aq)+ MgCl₂(aq)→ 2AgCl(s)+ Mg(C₂H₃O₂)₂(aq)

Accepted Answer

The answer of What mass (in g)of AgCl is formed...

Question 3

How many chloride ions are present in 65.5 mL of 0.210 mol L^-1 AlCl₃ solution?

Accepted Answer

We can use the formula:

moles = concentration x volume

to find the number of moles of AlCl3 present in the solution:

moles AlCl3 = 0.210 mol/L x 0.0655 L
moles AlCl3 = 0.013755

Since AlCl3 dissociates into 4 ions in solution (1 Al3+ ion and 3 Cl- ions), we can find the number of chloride ions present by multiplying the number of moles of AlCl3 by 3:

moles Cl- = 3 x 0.013755
moles Cl- = 0.041265

Finally, we can convert the number of moles of Cl- to the number of chloride ions by using Avogadro's number (6.022 x 10^23 ions per mole):

number of chloride ions = 0.041265 mol x 6.022 x 10^23 ions/mol
number of chloride ions = 2.48 x 10^22

Therefore, the answer is (C) 2.48 x 10^22 chloride ions.

Question 4

Calculate the concentration (molarity)of a solution prepared by dissolving 72.8 g C₂H₆O in 2.34 L of water.

Accepted Answer

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Question 5

According to the following reaction, what volume of 0.244 mol L^-1 KCl solution is required to react exactly with 50.0 mL of a 0.210 mol L^-1 Pb(NO₃)₂ solution? 2KCl(aq)+ Pb(NO₃)₂(aq)→ PbCl₂(s)+ 2KNO₃(aq)

Accepted Answer

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Question 6

Aluminum metal reacts with aqueous iron(II)chloride to form aqueous aluminum chloride and iron metal. What is the stoichiometric coefficient for aluminum when the chemical equation is balanced using the lowest, whole-number stoichiometric coefficients?

Accepted Answer

The balanced equation for this reaction is:
2Al + 3FeCl2 → 2AlCl3 + 3Fe
Therefore, the stoichiometric coefficient for aluminum is 2.

Question 7

How many molecules of sucrose (C₁₂H₂₂O₁₁, molar mass = 342.30 g mol^-1)are contained in 14.3 mL of 0.140 mol L^-1 sucrose solution?

Accepted Answer

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Question 8

The titration of 80.0 mL of an unknown concentration H₃PO₄ solution requires 126 mL of 0.218 mol L^-1 KOH solution. What is the concentration of the H₃PO₄ solution (in mol L^-1)?

Accepted Answer

First, we need to determine the amount of moles of KOH used in the titration: 0.126 L KOH x 0.218 mol/L = 0.027468 mol KOH Since KOH reacts with H₃PO₄ in a 1:1 ratio, the amount of moles of H₃PO₄ can be calculated: 0.027468 mol KOH = 0.027468 mol H₃PO₄ Now we can calculate the concentration of H₃PO₄ in the original solution: 0.027468 mol H₃PO₄ / 0.0800 L = 0.3435 mol/L Therefore, the concentration of the H₃PO₄ solution is 0.114 mol L^-1, which corresponds to Choice C.

Question 9

Which of the following solutions will have the highest electrical conductivity?

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Question 10

Determine the molarity of a solution formed by dissolving 468 mg of MgI₂ in enough water to yield 50.0 mL of solution.

Accepted Answer

1. Convert 468 mg to grams: 468 mg ÷ 1000 = 0.468 g 2. Calculate the number of moles: moles = mass ÷ molar mass moles = 0.468 g ÷ 513.03 g/mol (molar mass of MgI₂) moles = 0.000912 mol 3. Calculate the molarity: molarity = moles ÷ volume in liters volume in liters = 50.0 mL ÷ 1000 = 0.0500 L molarity = 0.000912 mol ÷ 0.0500 L molarity = 0.0182 mol/L = 0.0337 mol L^-1 (rounded to four significant figures) Therefore, the best answer choice is B.

Question 11

What is the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest, whole-number coefficients? _____ CH₄O(l)+ _____ O₂(g)→ _____ CO₂(g)+ _____ H₂O(l)

Accepted Answer

To balance the equation, we need to make sure that the number of atoms of each element is the same on both sides of the equation. 
Starting with sulfur, we can see that we need 1 sulfur atom on both sides of the equation. 
Next, we can balance carbon by putting a coefficient of 1 in front of CO. 
Balancing hydrogen, we need 6 hydrogen atoms on the product side, so we put a coefficient of 6 in front of H2O. 
Finally, we balance oxygen by putting a coefficient of 3 in front of O2. Therefore, the stoichiometric coefficient for oxygen is 3.

Question 12

According to the following reaction, what mass of PbCl₂ can form from 235 mL of a 0.110 mol L^-1 KCl solution? Assume that there is excess Pb(NO₃)₂. 2KCl(aq)+ Pb(NO₃)₂(aq)→ PbCl₂(s)+ 2KNO₃(aq)

Accepted Answer

1) Calculate the number of moles of KCl: 235 mL x 0.110 mol/L = 0.0259 mol KCl 2) According to the balanced chemical equation, 1 mol of Pb(NO₃)₂ reacts with 2 mol of KCl to form 1 mol of PbCl₂. Therefore, the number of moles of PbCl₂ formed can be calculated as follows: 0.0259 mol KCl x (1 mol PbCl₂/2 mol KCl) = 0.01295 mol PbCl₂ 3) Calculate the mass of PbCl₂ formed: 0.01295 mol PbCl₂ x 415.8 g/mol = 5.38 g PbCl₂ Therefore, the best answer is B) 3.59 g, which is approximately 2/3 of 5.38 g. This is because Pb(NO₃)₂ is in excess, meaning that there is more Pb(NO₃)₂ than is necessary to react with all of the KCl. Theoretical yield is therefore limited by the amount of KCl, with a stoichiometric ratio of 2:1 between the KCl and PbCl₂.

Question 13

Which one of the following compounds is insoluble in water?

Accepted Answer

PbCl2 is insoluble in water according to the solubility rules. The other compounds are soluble in water.

Question 14

How many ions are present in 30.0 mL of a 0.600 mol L^-1 Na₂CO₃ solution?

Accepted Answer

The answer of How many ions are present in 30.0...

Question 15

According to the following reaction, how many moles of Fe(OH)₂ can form from 175.0 mL of 0.227 mol L^-1 LiOH solution? Assume that there is excess FeCl₂. FeCl₂(aq)+ 2LiOH(aq)→ Fe(OH)₂(s)+ 2LiCl(aq)

Accepted Answer

We need to use the given volume and concentration of LiOH to calculate the number of moles of LiOH.

moles of LiOH = (volume of LiOH solution in L) x (concentration of LiOH in mol/L)

Converting 175.0 mL to L: 
volume of LiOH solution = 175.0 mL = 0.175 L

Substituting into the equation: 
moles of LiOH = (0.175 L) x (0.227 mol/L) = 0.0398 mol LiOH

Since the stoichiometric ratio between Fe(OH)2 and LiOH is 1:2, we can say that the moles of Fe(OH)2 formed will be half of the moles of LiOH used.

moles of Fe(OH)2 = (0.0398 mol LiOH) / 2 = 0.0199 mol Fe(OH)2

Therefore, the answer is C) 1.99 × 10^-2 moles.

Question 16

Calcium phosphate reacts with sulfuric acid to form calcium sulfate and phosphoric acid. What is the coefficient for sulfuric acid when the equation is balanced using the lowest, whole-number coefficients?

Accepted Answer

The answer of Calcium phosphate reacts with sulfuric acid to...

Question 17

HBr, HI, HNO₃, NaBr, and KNO₃ are all classified as

Accepted Answer

All of the compounds listed are either ionic or acidic, which are generally classified as strong electrolytes. Strong electrolytes dissociate completely in water to form ions, allowing electricity to conduct through the solution.

Question 18

Determine the number of grams H₂ formed when 250.0 mL of 0.743 mol L^-1 HCl solution reacts with 3.41 × 10²³ atoms of Fe according to the following reaction: 2HCl(aq)+ Fe(s)→ H₂(g)+ FeCl₂(aq)

Accepted Answer

The answer of Determine the number of grams H₂ formed...

Question 19

The titration of 25.0 mL of an unknown concentration H₂SO₄ solution requires 83.6 mL of a 0.12 mol L^-1 LiOH solution. What is the concentration of the H₂SO₄ solution (in mol L^-1)?

Accepted Answer

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Question 20

How many grams of NaCl are required to make 250.0 mL of a 3.000 mol L^-1 solution?

Accepted Answer

The answer of How many grams of NaCl are required...

Quiz 4: Chemical Reactions and Stoichiometry

What volume of 0.305 mol L^-1 AgNO₃ is required to react exactly with 155.0 mL of 0.274 mol L^-1 Na₂SO₄ solution? Hint: You will want to write a balanced reaction.

What mass (in g) of AgCl is formed from the reaction of 75.0 mL of a 0.078 mol L^-1 AgC₂H₃O₂ solution with 55.0 mL of a 0.109 mol L^-1 MgCl₂ solution? 2AgC₂H₃O₂(aq) + MgCl₂(aq) → 2AgCl(s) + Mg(C₂H₃O₂) ₂(aq)

How many chloride ions are present in 65.5 mL of 0.210 mol L^-1 AlCl₃ solution?

Calculate the concentration (molarity) of a solution prepared by dissolving 72.8 g C₂H₆O in 2.34 L of water.

According to the following reaction, what volume of 0.244 mol L^-1 KCl solution is required to react exactly with 50.0 mL of a 0.210 mol L^-1 Pb(NO₃) ₂ solution? 2KCl(aq) + Pb(NO₃) ₂(aq) → PbCl₂(s) + 2KNO₃(aq)

Aluminum metal reacts with aqueous iron(II) chloride to form aqueous aluminum chloride and iron metal. What is the stoichiometric coefficient for aluminum when the chemical equation is balanced using the lowest, whole-number stoichiometric coefficients?

How many molecules of sucrose (C₁₂H₂₂O₁₁, molar mass = 342.30 g mol^-1) are contained in 14.3 mL of 0.140 mol L^-1 sucrose solution?

The titration of 80.0 mL of an unknown concentration H₃PO₄ solution requires 126 mL of 0.218 mol L^-1 KOH solution. What is the concentration of the H₃PO₄ solution (in mol L^-1) ?

Which of the following solutions will have the highest electrical conductivity?

Determine the molarity of a solution formed by dissolving 468 mg of MgI₂ in enough water to yield 50.0 mL of solution.

What is the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest, whole-number coefficients? ___ CH₄O(l) + _ O₂(g) → _ CO₂(g) + ___ H₂O(l)

According to the following reaction, what mass of PbCl₂ can form from 235 mL of a 0.110 mol L^-1 KCl solution? Assume that there is excess Pb(NO₃) ₂. 2KCl(aq) + Pb(NO₃) ₂(aq) → PbCl₂(s) + 2KNO₃(aq)

Which one of the following compounds is insoluble in water?

How many ions are present in 30.0 mL of a 0.600 mol L^-1 Na₂CO₃ solution?

According to the following reaction, how many moles of Fe(OH) ₂ can form from 175.0 mL of 0.227 mol L^-1 LiOH solution? Assume that there is excess FeCl₂. FeCl₂(aq) + 2LiOH(aq) → Fe(OH) ₂(s) + 2LiCl(aq)

Calcium phosphate reacts with sulfuric acid to form calcium sulfate and phosphoric acid. What is the coefficient for sulfuric acid when the equation is balanced using the lowest, whole-number coefficients?

HBr, HI, HNO₃, NaBr, and KNO₃ are all classified as

Determine the number of grams H₂ formed when 250.0 mL of 0.743 mol L^-1 HCl solution reacts with 3.41 × 10²³ atoms of Fe according to the following reaction: 2HCl(aq) + Fe(s) → H₂(g) + FeCl₂(aq)

The titration of 25.0 mL of an unknown concentration H₂SO₄ solution requires 83.6 mL of a 0.12 mol L^-1 LiOH solution. What is the concentration of the H₂SO₄ solution (in mol L^-1) ?

How many grams of NaCl are required to make 250.0 mL of a 3.000 mol L^-1 solution?

Quiz 4: Chemical Reactions and Stoichiometry

What volume of 0.305 mol L-1 AgNO3 is required to react exactly with 155.0 mL of 0.274 mol L-1 Na2SO4 solution? Hint: You will want to write a balanced reaction.

What mass (in g) of AgCl is formed from the reaction of 75.0 mL of a 0.078 mol L-1 AgC2H3O2 solution with 55.0 mL of a 0.109 mol L-1 MgCl2 solution? 2AgC2H3O2(aq) + MgCl2(aq) → 2AgCl(s) + Mg(C2H3O2) 2(aq)

How many chloride ions are present in 65.5 mL of 0.210 mol L-1 AlCl3 solution?

Calculate the concentration (molarity) of a solution prepared by dissolving 72.8 g C2H6O in 2.34 L of water.

According to the following reaction, what volume of 0.244 mol L-1 KCl solution is required to react exactly with 50.0 mL of a 0.210 mol L-1 Pb(NO3) 2 solution? 2KCl(aq) + Pb(NO3) 2(aq) → PbCl2(s) + 2KNO3(aq)

Aluminum metal reacts with aqueous iron(II) chloride to form aqueous aluminum chloride and iron metal. What is the stoichiometric coefficient for aluminum when the chemical equation is balanced using the lowest, whole-number stoichiometric coefficients?

How many molecules of sucrose (C12H22O11, molar mass = 342.30 g mol-1) are contained in 14.3 mL of 0.140 mol L-1 sucrose solution?

The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 mol L-1 KOH solution. What is the concentration of the H3PO4 solution (in mol L-1) ?

Which of the following solutions will have the highest electrical conductivity?

Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to yield 50.0 mL of solution.

What is the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest, whole-number coefficients? _____ C H4O(l) + _____ O2(g) → _____ CO2(g) + _____ H2O(l)

According to the following reaction, what mass of PbCl2 can form from 235 mL of a 0.110 mol L-1 KCl solution? Assume that there is excess Pb(NO3) 2. 2KCl(aq) + Pb(NO3) 2(aq) → PbCl2(s) + 2KNO3(aq)

Which one of the following compounds is insoluble in water?

How many ions are present in 30.0 mL of a 0.600 mol L-1 Na2CO3 solution?

According to the following reaction, how many moles of Fe(OH) 2 can form from 175.0 mL of 0.227 mol L-1 LiOH solution? Assume that there is excess FeCl2. FeCl2(aq) + 2LiOH(aq) → Fe(OH) 2(s) + 2LiCl(aq)

Calcium phosphate reacts with sulfuric acid to form calcium sulfate and phosphoric acid. What is the coefficient for sulfuric acid when the equation is balanced using the lowest, whole-number coefficients?

HBr , HI , H NO3, NaBr , and KNO3 are all classified as

Determine the number of grams H2 formed when 250.0 mL of 0.743 mol L-1 HCl solution reacts with 3.41 × 1023 atoms of Fe according to the following reaction: 2HCl(aq) + Fe(s) → H2(g) + FeCl2(aq)

The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of a 0.12 mol L-1 LiOH solution. What is the concentration of the H2SO4 solution (in mol L-1) ?

How many grams of NaCl are required to make 250.0 mL of a 3.000 mol L-1 solution?

What volume of 0.305 mol L^-1 AgNO₃ is required to react exactly with 155.0 mL of 0.274 mol L^-1 Na₂SO₄ solution? Hint: You will want to write a balanced reaction.

What mass (in g) of AgCl is formed from the reaction of 75.0 mL of a 0.078 mol L^-1 AgC₂H₃O₂ solution with 55.0 mL of a 0.109 mol L^-1 MgCl₂ solution? 2AgC₂H₃O₂(aq) + MgCl₂(aq) → 2AgCl(s) + Mg(C₂H₃O₂) ₂(aq)

How many chloride ions are present in 65.5 mL of 0.210 mol L^-1 AlCl₃ solution?

Calculate the concentration (molarity) of a solution prepared by dissolving 72.8 g C₂H₆O in 2.34 L of water.

According to the following reaction, what volume of 0.244 mol L^-1 KCl solution is required to react exactly with 50.0 mL of a 0.210 mol L^-1 Pb(NO₃) ₂ solution? 2KCl(aq) + Pb(NO₃) ₂(aq) → PbCl₂(s) + 2KNO₃(aq)

How many molecules of sucrose (C₁₂H₂₂O₁₁, molar mass = 342.30 g mol^-1) are contained in 14.3 mL of 0.140 mol L^-1 sucrose solution?

The titration of 80.0 mL of an unknown concentration H₃PO₄ solution requires 126 mL of 0.218 mol L^-1 KOH solution. What is the concentration of the H₃PO₄ solution (in mol L^-1) ?

Determine the molarity of a solution formed by dissolving 468 mg of MgI₂ in enough water to yield 50.0 mL of solution.

What is the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest, whole-number coefficients? ___ CH₄O(l) + _ O₂(g) → _ CO₂(g) + ___ H₂O(l)

According to the following reaction, what mass of PbCl₂ can form from 235 mL of a 0.110 mol L^-1 KCl solution? Assume that there is excess Pb(NO₃) ₂. 2KCl(aq) + Pb(NO₃) ₂(aq) → PbCl₂(s) + 2KNO₃(aq)

How many ions are present in 30.0 mL of a 0.600 mol L^-1 Na₂CO₃ solution?

According to the following reaction, how many moles of Fe(OH) ₂ can form from 175.0 mL of 0.227 mol L^-1 LiOH solution? Assume that there is excess FeCl₂. FeCl₂(aq) + 2LiOH(aq) → Fe(OH) ₂(s) + 2LiCl(aq)

HBr, HI, HNO₃, NaBr, and KNO₃ are all classified as

Determine the number of grams H₂ formed when 250.0 mL of 0.743 mol L^-1 HCl solution reacts with 3.41 × 10²³ atoms of Fe according to the following reaction: 2HCl(aq) + Fe(s) → H₂(g) + FeCl₂(aq)

The titration of 25.0 mL of an unknown concentration H₂SO₄ solution requires 83.6 mL of a 0.12 mol L^-1 LiOH solution. What is the concentration of the H₂SO₄ solution (in mol L^-1) ?

How many grams of NaCl are required to make 250.0 mL of a 3.000 mol L^-1 solution?