Question 1

The mixing of which pair of reactants will result in a precipitation reaction?

Accepted Answer

Ba(NO3)2 and Na2CO3 will react to form BaCO3, which is insoluble and will precipitate out of solution. The other choices do not involve the formation of a precipitate.

Question 2

What reagent could not be used to separate Br^- from CO₃^2- when added to an aqueous solution containing both?

Accepted Answer

AgNO3 can be used to selectively precipitate Br- from the solution as insoluble AgBr, leaving CO₃^2- in solution. Ca(NO3)2, Cu(NO3)2, and Fe(NO3)3 all have the potential to form precipitates with both Br- and CO₃^2-, making them unsuitable for selective separation.

Question 3

How many H⁺ ions can the acid H₂SO₄ donate per molecule?

Accepted Answer

Each sulfur in the acid can donate two protons, represented by H⁺. Therefore, there are a total of 6 protons available to be donated. Each H⁺ ion requires 1 proton, so the acid can donate a maximum of 6/2 = 3 H⁺ ions, making the answer C.

Question 4

When dissolved in water,KOH behaves as

Accepted Answer

KOH is a strong base, and when it dissolves in water, it dissociates into K+ and OH- ions. Therefore, it forms K⁺ and OH^- ions, making choice C the correct answer.

Question 5

How many millilitres of 0.152 mol L^-1 $\mathrm { HClO } _ { 4 }$ solution are needed to neutralize 50.00 mL of 0.0793 mol L^-1 NaOH?

Accepted Answer

To neutralize NaOH with HClO4, use the formula: $C_1V_1 = C_2V_2$. Here, $C_1 = 0.0793 \, \text{mol/L}$, $V_1 = 50.00 \, \text{mL}$, $C_2 = 0.152 \, \text{mol/L}$. Solving for $V_2$, $V_2 = \frac{C_1V_1}{C_2} = \frac{0.0793 \times 50.00}{0.152} = 26.1 \, \text{mL}$.

Question 6

Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide: $\mathrm { Pb } ^ { 2 + }$ (aq)+ $2 \mathrm { I } ^ { - }$ (aq)? $\mathrm { PbI } _ { 2 }$ (s) Lead iodide is virtually insoluble in water so that the reaction appears to go to completion.How many millilitres of 3.550 mol L^-1 HI(aq)must be added to a solution containing 0.700 mol of $\mathrm { Pb } \left( \mathrm { NO } _ { 3 } \right) _ { 2 } ^ { ( a q ) }$ to completely precipitate the lead?

Accepted Answer

According to the balanced chemical equation, 1 mole of $\mathrm{Pb(NO_3)_2}$ reacts with 2 moles of HI to produce 1 mole of $\mathrm{PbI_2}$. Therefore, if we have 0.700 mol of $\mathrm{Pb(NO_3)_2}$, we need 2 x 0.700 = 1.400 mol of HI to completely precipitate the lead.

To calculate the volume of 3.550 mol/L HI solution required to provide 1.400 mol of HI, we use the following equation:

Molarity = moles / volume

Rearranging,

Volume = moles / molarity

Volume = 1.400 mol / 3.550 mol/L = 0.394 L = 394 mL

Therefore, the answer is C, 394 mL.

Question 7

What reagent could be used to separate Br^- from CH₃CO₂^-when added to an aqueous solution containing both?

Accepted Answer

AgNO3(aq) can selectively react with Br- to form insoluble AgBr(s). This will cause Br^- to precipitate out of the solution, while leaving CH₃CO₂^- in the aqueous solution. The other reagents listed would not selectively react with either compound.

Question 8

The mixing of which pair of reactants will result in a precipitation reaction?

Accepted Answer

The mixing of potassium sulfate (K2SO4) and barium nitrate (Ba(NO3)2) will result in a precipitation reaction because they will form insoluble barium sulfate (BaSO4) and potassium nitrate (KNO3) according to the following reaction: 
K2SO4(aq) + Ba(NO3)2(aq) → BaSO4(s) + 2KNO3(aq)

Question 9

A solution is prepared by adding 1.40 g of solid NaCl to 50.0 mL of 0.100 mol L^-1 $\mathrm { CaCl } _ { 2 }$ .What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.

Accepted Answer

The answer of A solution is prepared by adding 1.40...

Question 10

Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: $\mathrm { Ag } ^ { + }$ (aq)+ $\mathrm { Cl } ^ { - }$ (aq)? AgCl(s) Silver chloride is virtually insoluble in water so that the reaction appears to go to completion.How many grams of solid NaCl must be added to 25.0 mL of 0.376 mol L^-1 $\mathrm { AgNO } _ { 3 }$ solution to completely precipitate the silver?

Accepted Answer

The balanced chemical equation is:$$\mathrm { Ag } ^ { + }\) (aq)+ $\mathrm { Cl } ^ { - }$ (aq)? AgCl(s)From the stoichiometry of the balanced chemical equation, we can see that 1 mol of $\mathrm { Ag } ^ { + }$ reacts with 1 mol of $\mathrm { Cl } ^ { - }$. Therefore, the number of moles of $\mathrm { Cl } ^ { - }$ required to precipitate all of the $\mathrm { Ag } ^ { + }$ ions in 25.0 mL of 0.376 mol L^-1 $\mathrm { AgNO } _ { 3 }$ solution is:$$25.0 \text{ mL} \times \frac{1 \text{ L}}{1000 \text{ mL}} \times 0.376 \text{ mol/L} = 9.40 \times 10^{-3} \text{ mol}$$The molar mass of NaCl is 58.44 g/mol. Therefore, the mass of NaCl required to provide this number of moles of $\mathrm { Cl } ^ { - }$ ions is:$$9.40 \times 10^{-3} \text{ mol} \times 58.44 \text{ g/mol} = 0.549 \text{ g}$$Therefore, the correct answer is B) 0.549 g.

Question 11

A solution is prepared by mixing 70.0 mL of 0.100 mol L^-1 HCl and 30.0 mL of 0.200 mol L^-1 NaCl.What is the molarity of chloride ion in this solution?

Accepted Answer

The answer of A solution is prepared by mixing 70.0...

Question 12

Which of the following compounds is an Arrhenius base?

Accepted Answer

CsOH is a hydroxide compound, which is a characteristic of Arrhenius bases. The other options do not contain hydroxide ions and therefore are not Arrhenius bases.

Question 13

Which one of the following compounds behaves as an acid when dissolved in water?

Accepted Answer

HI is a strong acid and will dissociate in water to release H+ ions, making the solution acidic. The other three compounds, RaO, C₄H₁₀, and RbOH are all basic and will dissociate to release OH- ions, making the solution basic.

Question 14

Which of the compounds of H₂C₂O_4, Ca(OH)₂,KOH,and HI behave as acids when they are dissolved in water?

Accepted Answer

H₂C₂O₄ (oxalic acid) and HI (hydroiodic acid) are both acids because they release H+ ions when dissolved in water.

Question 15

In an acid-base neutralization reaction,38.74 mL of 0.500 mol L^-1 potassium hydroxide reacts with 50.00 mL of sulfuric acid solution.What is the concentration of the H₂SO₄ solution?

Accepted Answer

The balanced chemical equation for the reaction between potassium hydroxide (KOH) and sulfuric acid (H2SO4) is 2KOH + H2SO4 → K2SO4 + 2H2O. This shows that 2 moles of KOH react with 1 mole of H2SO4. Given that 38.74 mL of 0.500 M KOH is used, the moles of KOH are (38.74 mL) * (0.500 mol/L) = 0.01937 mol. Since the ratio of KOH to H2SO4 is 2:1, the moles of H2SO4 needed are half of that of KOH, which is 0.01937 mol / 2 = 0.009685 mol. The concentration of H2SO4 is then the moles of H2SO4 divided by the volume of the H2SO4 solution in liters, which is 0.009685 mol / 0.05000 L = 0.194 mol/L.

Question 16

Which of the following compounds is an Arrhenius base?

Accepted Answer

According to Arrhenius theory, a base is a substance that produces hydroxide ions (OH-) in aqueous solutions. Among the given compounds, only option B contains NH3 (ammonia) which produces hydroxide ions when dissolved in water. Therefore, option B is the correct answer.

Question 17

Which of the following compounds is an Arrhenius base?

Accepted Answer

The answer of Which of the following compounds is an...

Question 18

When 280.mL of 1.50 × 10^-4mol L^-1 hydrochloric acid is added to 135 mL of 1.75 × 10^-4 mol L^-1 Mg(OH)₂,the resulting solution will be

Accepted Answer

When hydrochloric acid is added to magnesium hydroxide, they react to form magnesium chloride and water. This is an acid-base neutralization reaction. The products of this reaction do not contribute to the acidity or basicity of the resulting solution. Therefore, the resulting solution will be basic, as the excess hydroxide ions from the Mg(OH)2 will dominate the solution.

Question 19

Which of the compounds H₂C₂O₄,Ca(OH)₂,KOH,and HI behave as bases when they are dissolved in water?

Accepted Answer

Ca(OH)₂ and KOH are both hydroxide compounds, which dissociate in water to produce OH- ions, making them bases. H₂C₂O₄ and HI are both acid compounds, which dissociate in water to produce H+ ions, making them acids. HI is a strong acid and does not behave as a base when dissolved in water. Therefore, only Ca(OH)₂ and KOH behave as bases when dissolved in water.

Question 20

What is the molarity of a NaOH solution if 28.2 mL of a 0.355 mol L^-1 H₂SO₄ solution is required to neutralize a 25.0 mL sample of the NaOH solution?

Accepted Answer

The correct answer is A because the molarity of the NaOH solution can be calculated using the formula:Molarity of NaOH = (Molarity of H2SO4 * Volume of H2SO4) / Volume of NaOHSubstituting the given values into the formula, we get:Molarity of NaOH = (0.355 mol L-1 * 28.2 mL) / 25.0 mL = 0.801 mol L-1

Quiz 4: Chemical Reactions and Stoichiometry

The mixing of which pair of reactants will result in a precipitation reaction?

What reagent could not be used to separate Br^- from CO₃^2- when added to an aqueous solution containing both?

How many H⁺ ions can the acid H₂SO₄ donate per molecule?

When dissolved in water,KOH behaves as

How many millilitres of 0.152 mol L^-1 $\mathrm { HClO } _ { 4 }$ solution are needed to neutralize 50.00 mL of 0.0793 mol L^-1 NaOH?

What reagent could be used to separate Br^- from CH₃CO₂^-when added to an aqueous solution containing both?

The mixing of which pair of reactants will result in a precipitation reaction?

A solution is prepared by adding 1.40 g of solid NaCl to 50.0 mL of 0.100 mol L^-1 $\mathrm { CaCl } _ { 2 }$ .What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.

A solution is prepared by mixing 70.0 mL of 0.100 mol L^-1 HCl and 30.0 mL of 0.200 mol L^-1 NaCl.What is the molarity of chloride ion in this solution?

Which of the following compounds is an Arrhenius base?

Which one of the following compounds behaves as an acid when dissolved in water?

Which of the compounds of H₂C₂O_4, Ca(OH) ₂,KOH,and HI behave as acids when they are dissolved in water?

In an acid-base neutralization reaction,38.74 mL of 0.500 mol L^-1 potassium hydroxide reacts with 50.00 mL of sulfuric acid solution.What is the concentration of the H₂SO₄ solution?

Which of the following compounds is an Arrhenius base?

Which of the following compounds is an Arrhenius base?

When 280.mL of 1.50 × 10^-4mol L^-1 hydrochloric acid is added to 135 mL of 1.75 × 10^-4 mol L^-1 Mg(OH) ₂,the resulting solution will be

Which of the compounds H₂C₂O₄,Ca(OH) ₂,KOH,and HI behave as bases when they are dissolved in water?

What is the molarity of a NaOH solution if 28.2 mL of a 0.355 mol L^-1 H₂SO₄ solution is required to neutralize a 25.0 mL sample of the NaOH solution?

Quiz 4: Chemical Reactions and Stoichiometry

The mixing of which pair of reactants will result in a precipitation reaction?

What reagent could not be used to separate Br- from CO32- when added to an aqueous solution containing both?

How many H+ ions can the acid H2SO4 donate per molecule?

When dissolved in water,KOH behaves as

How many millilitres of 0.152 mol L-1 HClO4\mathrm { HClO } _ { 4 }HClO4​ solution are needed to neutralize 50.00 mL of 0.0793 mol L-1 NaOH?

What reagent could be used to separate Br- from CH3CO2- when added to an aqueous solution containing both?

The mixing of which pair of reactants will result in a precipitation reaction?

A solution is prepared by adding 1.40 g of solid NaCl to 50.0 mL of 0.100 mol L-1 CaCl2\mathrm { CaCl } _ { 2 }CaCl2​ .What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.

A solution is prepared by mixing 70.0 mL of 0.100 mol L-1 HCl and 30.0 mL of 0.200 mol L-1 NaCl.What is the molarity of chloride ion in this solution?

Which of the following compounds is an Arrhenius base?

Which one of the following compounds behaves as an acid when dissolved in water?

Which of the compounds of H2C2O4, Ca(OH) 2,KOH,and HI behave as acids when they are dissolved in water?

In an acid-base neutralization reaction,38.74 mL of 0.500 mol L-1 potassium hydroxide reacts with 50.00 mL of sulfuric acid solution.What is the concentration of the H2SO4 solution?

Which of the following compounds is an Arrhenius base?

Which of the following compounds is an Arrhenius base?

When 280.mL of 1.50 × 10-4 mol L-1 hydrochloric acid is added to 135 mL of 1.75 × 10-4 mol L-1 Mg(OH) 2,the resulting solution will be

Which of the compounds H2C2O4,Ca(OH) 2,KOH,and HI behave as bases when they are dissolved in water?

What is the molarity of a NaOH solution if 28.2 mL of a 0.355 mol L-1 H2SO4 solution is required to neutralize a 25.0 mL sample of the NaOH solution?

What reagent could not be used to separate Br^- from CO₃^2- when added to an aqueous solution containing both?

How many H⁺ ions can the acid H₂SO₄ donate per molecule?

How many millilitres of 0.152 mol L^-1 $\mathrm { HClO } _ { 4 }$ solution are needed to neutralize 50.00 mL of 0.0793 mol L^-1 NaOH?

What reagent could be used to separate Br^- from CH₃CO₂^-when added to an aqueous solution containing both?

A solution is prepared by adding 1.40 g of solid NaCl to 50.0 mL of 0.100 mol L^-1 $\mathrm { CaCl } _ { 2 }$ .What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.

A solution is prepared by mixing 70.0 mL of 0.100 mol L^-1 HCl and 30.0 mL of 0.200 mol L^-1 NaCl.What is the molarity of chloride ion in this solution?

Which of the compounds of H₂C₂O_4, Ca(OH) ₂,KOH,and HI behave as acids when they are dissolved in water?

In an acid-base neutralization reaction,38.74 mL of 0.500 mol L^-1 potassium hydroxide reacts with 50.00 mL of sulfuric acid solution.What is the concentration of the H₂SO₄ solution?

When 280.mL of 1.50 × 10^-4mol L^-1 hydrochloric acid is added to 135 mL of 1.75 × 10^-4 mol L^-1 Mg(OH) ₂,the resulting solution will be

Which of the compounds H₂C₂O₄,Ca(OH) ₂,KOH,and HI behave as bases when they are dissolved in water?

What is the molarity of a NaOH solution if 28.2 mL of a 0.355 mol L^-1 H₂SO₄ solution is required to neutralize a 25.0 mL sample of the NaOH solution?