The milliliters of 1.6 M NaHCO 3 that must be poured on the spill to react completely with 88 mL of 2.6 M H 2 SO 4 is to be calculated. Concept introduction: Strong acids and strong bases are the substance that dissociates completely into its ions when dissolved in the solution. They dissociate completely in water to release H + ions and OH − ions. Weak acids and weak bases are the substance that does not dissociate completely into its ions when dissolved in the solution. They dissociate partially in water to release H + ions and OH − ions. Sulfuric acid ( H 2 SO 4 ) is a strong acid and sodium bicarbonate ( NaHCO 3 ) is a weak base. Sulfuric acid ( H 2 SO 4 ) dissociates completely into ions and the sodium bicarbonate ( NaHCO 3 ) dissociates to some extent into ions. They both react to form sodium sulfate, carbon dioxide, and a water molecule. The molecular equation for the acid-base reaction of sulfuric acid and sodium bicarbonate is: H 2 SO 4 ( a q ) + 2 NaHCO 3 ( a q ) → Na 2 SO 4 ( a q ) + 2 H 2 O ( l ) + 2 CO 2 ( g )

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Answer 1

Question

Chapter 4, Problem 4.73P

Interpretation Introduction

Interpretation:

The milliliters of $1.6 M NaHCO3$ that must be poured on the spill to react completely with $88 mL$ of $2.6 M H2SO4$ is to be calculated.

Concept introduction:

Strong acids and strong bases are the substance that dissociates completely into its ions when dissolved in the solution. They dissociate completely in water to release $H+$ ions and $OH−$ ions.

Weak acids and weak bases are the substance that does not dissociate completely into its ions when dissolved in the solution. They dissociate partially in water to release $H+$ ions and $OH−$ ions.

Sulfuric acid $(H2SO4)$ is a strong acid and sodium bicarbonate $(NaHCO3)$ is a weak base. Sulfuric acid $(H2SO4)$ dissociates completely into ions and the sodium bicarbonate $(NaHCO3)$ dissociates to some extent into ions. They both react to form sodium sulfate, carbon dioxide, and a water molecule.

The molecular equation for the acid-base reaction of sulfuric acid and sodium bicarbonate is:

$H2SO4(aq)+2NaHCO3(aq)→Na2SO4(aq)+2H2O(l)+2CO2(g)$

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Answer 2

Question

Chapter 4, Problem 4.73P

Interpretation Introduction

Interpretation:

The milliliters of $1.6 M NaHCO3$ that must be poured on the spill to react completely with $88 mL$ of $2.6 M H2SO4$ is to be calculated.

Concept introduction:

Strong acids and strong bases are the substance that dissociates completely into its ions when dissolved in the solution. They dissociate completely in water to release $H+$ ions and $OH−$ ions.

Weak acids and weak bases are the substance that does not dissociate completely into its ions when dissolved in the solution. They dissociate partially in water to release $H+$ ions and $OH−$ ions.

Sulfuric acid $(H2SO4)$ is a strong acid and sodium bicarbonate $(NaHCO3)$ is a weak base. Sulfuric acid $(H2SO4)$ dissociates completely into ions and the sodium bicarbonate $(NaHCO3)$ dissociates to some extent into ions. They both react to form sodium sulfate, carbon dioxide, and a water molecule.

The molecular equation for the acid-base reaction of sulfuric acid and sodium bicarbonate is:

$H2SO4(aq)+2NaHCO3(aq)→Na2SO4(aq)+2H2O(l)+2CO2(g)$

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Answer 3

Question

Chapter 4, Problem 4.73P

Interpretation Introduction

Interpretation:

The milliliters of $1.6 M NaHCO3$ that must be poured on the spill to react completely with $88 mL$ of $2.6 M H2SO4$ is to be calculated.

Concept introduction:

Strong acids and strong bases are the substance that dissociates completely into its ions when dissolved in the solution. They dissociate completely in water to release $H+$ ions and $OH−$ ions.

Weak acids and weak bases are the substance that does not dissociate completely into its ions when dissolved in the solution. They dissociate partially in water to release $H+$ ions and $OH−$ ions.

Sulfuric acid $(H2SO4)$ is a strong acid and sodium bicarbonate $(NaHCO3)$ is a weak base. Sulfuric acid $(H2SO4)$ dissociates completely into ions and the sodium bicarbonate $(NaHCO3)$ dissociates to some extent into ions. They both react to form sodium sulfate, carbon dioxide, and a water molecule.

The molecular equation for the acid-base reaction of sulfuric acid and sodium bicarbonate is:

$H2SO4(aq)+2NaHCO3(aq)→Na2SO4(aq)+2H2O(l)+2CO2(g)$

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Answer 4

Question

Chapter 4, Problem 4.73P

Interpretation Introduction

Interpretation:

The milliliters of $1.6 M NaHCO3$ that must be poured on the spill to react completely with $88 mL$ of $2.6 M H2SO4$ is to be calculated.

Concept introduction:

Strong acids and strong bases are the substance that dissociates completely into its ions when dissolved in the solution. They dissociate completely in water to release $H+$ ions and $OH−$ ions.

Weak acids and weak bases are the substance that does not dissociate completely into its ions when dissolved in the solution. They dissociate partially in water to release $H+$ ions and $OH−$ ions.

Sulfuric acid $(H2SO4)$ is a strong acid and sodium bicarbonate $(NaHCO3)$ is a weak base. Sulfuric acid $(H2SO4)$ dissociates completely into ions and the sodium bicarbonate $(NaHCO3)$ dissociates to some extent into ions. They both react to form sodium sulfate, carbon dioxide, and a water molecule.

The molecular equation for the acid-base reaction of sulfuric acid and sodium bicarbonate is:

$H2SO4(aq)+2NaHCO3(aq)→Na2SO4(aq)+2H2O(l)+2CO2(g)$

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Answer 5

Chapter 4, Problem 4.73P

Interpretation Introduction

Interpretation:

The milliliters of $1.6 M NaHCO3$ that must be poured on the spill to react completely with $88 mL$ of $2.6 M H2SO4$ is to be calculated.

Concept introduction:

Strong acids and strong bases are the substance that dissociates completely into its ions when dissolved in the solution. They dissociate completely in water to release $H+$ ions and $OH−$ ions.

Weak acids and weak bases are the substance that does not dissociate completely into its ions when dissolved in the solution. They dissociate partially in water to release $H+$ ions and $OH−$ ions.

Sulfuric acid $(H2SO4)$ is a strong acid and sodium bicarbonate $(NaHCO3)$ is a weak base. Sulfuric acid $(H2SO4)$ dissociates completely into ions and the sodium bicarbonate $(NaHCO3)$ dissociates to some extent into ions. They both react to form sodium sulfate, carbon dioxide, and a water molecule.

The molecular equation for the acid-base reaction of sulfuric acid and sodium bicarbonate is:

$H2SO4(aq)+2NaHCO3(aq)→Na2SO4(aq)+2H2O(l)+2CO2(g)$

Answer 6

Chapter 4, Problem 4.73P

Interpretation Introduction

Interpretation:

The milliliters of $1.6 M NaHCO3$ that must be poured on the spill to react completely with $88 mL$ of $2.6 M H2SO4$ is to be calculated.

Concept introduction:

Strong acids and strong bases are the substance that dissociates completely into its ions when dissolved in the solution. They dissociate completely in water to release $H+$ ions and $OH−$ ions.

Weak acids and weak bases are the substance that does not dissociate completely into its ions when dissolved in the solution. They dissociate partially in water to release $H+$ ions and $OH−$ ions.

Sulfuric acid $(H2SO4)$ is a strong acid and sodium bicarbonate $(NaHCO3)$ is a weak base. Sulfuric acid $(H2SO4)$ dissociates completely into ions and the sodium bicarbonate $(NaHCO3)$ dissociates to some extent into ions. They both react to form sodium sulfate, carbon dioxide, and a water molecule.

The molecular equation for the acid-base reaction of sulfuric acid and sodium bicarbonate is:

$H2SO4(aq)+2NaHCO3(aq)→Na2SO4(aq)+2H2O(l)+2CO2(g)$

Answer 7

Chapter 4, Problem 4.73P

Interpretation Introduction

Interpretation:

The milliliters of $1.6 M NaHCO3$ that must be poured on the spill to react completely with $88 mL$ of $2.6 M H2SO4$ is to be calculated.

Concept introduction:

Strong acids and strong bases are the substance that dissociates completely into its ions when dissolved in the solution. They dissociate completely in water to release $H+$ ions and $OH−$ ions.

Weak acids and weak bases are the substance that does not dissociate completely into its ions when dissolved in the solution. They dissociate partially in water to release $H+$ ions and $OH−$ ions.

Sulfuric acid $(H2SO4)$ is a strong acid and sodium bicarbonate $(NaHCO3)$ is a weak base. Sulfuric acid $(H2SO4)$ dissociates completely into ions and the sodium bicarbonate $(NaHCO3)$ dissociates to some extent into ions. They both react to form sodium sulfate, carbon dioxide, and a water molecule.

The molecular equation for the acid-base reaction of sulfuric acid and sodium bicarbonate is:

$H2SO4(aq)+2NaHCO3(aq)→Na2SO4(aq)+2H2O(l)+2CO2(g)$

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 4.1 - (a) Which strong electrolyte is dissolved in water...Ch. 4.1 - (a) Make a drawing similar to that in Follow-up...Ch. 4.1 - What amount (mol) of each ion is in each...Ch. 4.1 - Prob. 4.2BFP Ch. 4.1 - Prob. 4.3AFP Ch. 4.1 - Prob. 4.3BFP Ch. 4.1 - Prob. 4.4AFP Ch. 4.1 - Prob. 4.4BFP Ch. 4.1 - What amount (mol) of each ion is in 1.32 L of 0.55...Ch. 4.1 - What is the molarity of aluminum ion in a solution...

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