The mass percent of N H 4 NO 3 and ( N H 4 ) 2 H P O 4 in a mixture which shows the mass percent of nitrogen to be 33.81 % has to be determined. Concept introduction: Molecular weight : The sum of the atomic weight of each constituent element multiplied by the number of atoms of that element is known as molecular weight of the compound. It can be determined by using the molecular formula. Mass percent: It represents the mass of the constituent element in grams per exactly 100 g of compound. m a s s % = m a s s o f e l e m e n t i n c o m p o u n d m a s s o f c o m p o u n d × 100 %

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Answer 1

Question

Chapter 19, Problem 19.134MP

(a)

Interpretation Introduction

Interpretation:

The mass percent of $NH4NO3$ and $(NH4)2HPO4$ in a mixture which shows the mass percent of nitrogen to be $33.81 %$ has to be determined.

Concept introduction:

Molecular weight:

The sum of the atomic weight of each constituent element multiplied by the number of atoms of that element is known as molecular weight of the compound.

It can be determined by using the molecular formula.

Mass percent:

It represents the mass of the constituent element in grams per exactly $100 g$ of compound.

$mass % = mass of element in compoundmass of compound × 100%$

(b)

Interpretation Introduction

Interpretation:

A $0.965 g$ sample of the mixture was dissolved in enough water to make $50.0mL$ of solution the $pH$ of this solution should be determined.

Concept introduction:

$pH$ and $pOH$ can be calculated using the below mentioned equations;

$pH= -log[H3O+]pOH = -log[OH-]$

The $pH and pOH$ of a water solution at $250C$ are related by the following equation,

$pH+ pOH = 14$

Molarity is the amount of moles of a compound dissolved in an amount of solvent (in liters)

$Molarity (M) = Moles of soluteLiters of solution$

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Answer 2

Question

Chapter 19, Problem 19.134MP

(a)

Interpretation Introduction

Interpretation:

The mass percent of $NH4NO3$ and $(NH4)2HPO4$ in a mixture which shows the mass percent of nitrogen to be $33.81 %$ has to be determined.

Concept introduction:

Molecular weight:

The sum of the atomic weight of each constituent element multiplied by the number of atoms of that element is known as molecular weight of the compound.

It can be determined by using the molecular formula.

Mass percent:

It represents the mass of the constituent element in grams per exactly $100 g$ of compound.

$mass % = mass of element in compoundmass of compound × 100%$

(b)

Interpretation Introduction

Interpretation:

A $0.965 g$ sample of the mixture was dissolved in enough water to make $50.0mL$ of solution the $pH$ of this solution should be determined.

Concept introduction:

$pH$ and $pOH$ can be calculated using the below mentioned equations;

$pH= -log[H3O+]pOH = -log[OH-]$

The $pH and pOH$ of a water solution at $250C$ are related by the following equation,

$pH+ pOH = 14$

Molarity is the amount of moles of a compound dissolved in an amount of solvent (in liters)

$Molarity (M) = Moles of soluteLiters of solution$

Expert Solution & Answer

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Answer 3

Question

Chapter 19, Problem 19.134MP

(a)

Interpretation Introduction

Interpretation:

The mass percent of $NH4NO3$ and $(NH4)2HPO4$ in a mixture which shows the mass percent of nitrogen to be $33.81 %$ has to be determined.

Concept introduction:

Molecular weight:

The sum of the atomic weight of each constituent element multiplied by the number of atoms of that element is known as molecular weight of the compound.

It can be determined by using the molecular formula.

Mass percent:

It represents the mass of the constituent element in grams per exactly $100 g$ of compound.

$mass % = mass of element in compoundmass of compound × 100%$

(b)

Interpretation Introduction

Interpretation:

A $0.965 g$ sample of the mixture was dissolved in enough water to make $50.0mL$ of solution the $pH$ of this solution should be determined.

Concept introduction:

$pH$ and $pOH$ can be calculated using the below mentioned equations;

$pH= -log[H3O+]pOH = -log[OH-]$

The $pH and pOH$ of a water solution at $250C$ are related by the following equation,

$pH+ pOH = 14$

Molarity is the amount of moles of a compound dissolved in an amount of solvent (in liters)

$Molarity (M) = Moles of soluteLiters of solution$

Expert Solution & Answer

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Answer 4

Question

Chapter 19, Problem 19.134MP

(a)

Interpretation Introduction

Interpretation:

The mass percent of $NH4NO3$ and $(NH4)2HPO4$ in a mixture which shows the mass percent of nitrogen to be $33.81 %$ has to be determined.

Concept introduction:

Molecular weight:

The sum of the atomic weight of each constituent element multiplied by the number of atoms of that element is known as molecular weight of the compound.

It can be determined by using the molecular formula.

Mass percent:

It represents the mass of the constituent element in grams per exactly $100 g$ of compound.

$mass % = mass of element in compoundmass of compound × 100%$

(b)

Interpretation Introduction

Interpretation:

A $0.965 g$ sample of the mixture was dissolved in enough water to make $50.0mL$ of solution the $pH$ of this solution should be determined.

Concept introduction:

$pH$ and $pOH$ can be calculated using the below mentioned equations;

$pH= -log[H3O+]pOH = -log[OH-]$

The $pH and pOH$ of a water solution at $250C$ are related by the following equation,

$pH+ pOH = 14$

Molarity is the amount of moles of a compound dissolved in an amount of solvent (in liters)

$Molarity (M) = Moles of soluteLiters of solution$

Expert Solution & Answer

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Answer 5

Chapter 19, Problem 19.134MP

(a)

Interpretation Introduction

Interpretation:

The mass percent of $NH4NO3$ and $(NH4)2HPO4$ in a mixture which shows the mass percent of nitrogen to be $33.81 %$ has to be determined.

Concept introduction:

Molecular weight:

The sum of the atomic weight of each constituent element multiplied by the number of atoms of that element is known as molecular weight of the compound.

It can be determined by using the molecular formula.

Mass percent:

It represents the mass of the constituent element in grams per exactly $100 g$ of compound.

$mass % = mass of element in compoundmass of compound × 100%$

(b)

Interpretation Introduction

Interpretation:

A $0.965 g$ sample of the mixture was dissolved in enough water to make $50.0mL$ of solution the $pH$ of this solution should be determined.

Concept introduction:

$pH$ and $pOH$ can be calculated using the below mentioned equations;

$pH= -log[H3O+]pOH = -log[OH-]$

The $pH and pOH$ of a water solution at $250C$ are related by the following equation,

$pH+ pOH = 14$

Molarity is the amount of moles of a compound dissolved in an amount of solvent (in liters)

$Molarity (M) = Moles of soluteLiters of solution$

Answer 6

Chapter 19, Problem 19.134MP

(a)

Interpretation Introduction

Interpretation:

The mass percent of $NH4NO3$ and $(NH4)2HPO4$ in a mixture which shows the mass percent of nitrogen to be $33.81 %$ has to be determined.

Concept introduction:

Molecular weight:

The sum of the atomic weight of each constituent element multiplied by the number of atoms of that element is known as molecular weight of the compound.

It can be determined by using the molecular formula.

Mass percent:

It represents the mass of the constituent element in grams per exactly $100 g$ of compound.

$mass % = mass of element in compoundmass of compound × 100%$

Answer 7

Chapter 19, Problem 19.134MP

(a)

Interpretation Introduction

Interpretation:

The mass percent of $NH4NO3$ and $(NH4)2HPO4$ in a mixture which shows the mass percent of nitrogen to be $33.81 %$ has to be determined.

Concept introduction:

Molecular weight:

The sum of the atomic weight of each constituent element multiplied by the number of atoms of that element is known as molecular weight of the compound.

It can be determined by using the molecular formula.

Mass percent:

It represents the mass of the constituent element in grams per exactly $100 g$ of compound.

$mass % = mass of element in compoundmass of compound × 100%$

Answer 8

(b)

Interpretation Introduction

Interpretation:

A $0.965 g$ sample of the mixture was dissolved in enough water to make $50.0mL$ of solution the $pH$ of this solution should be determined.

Concept introduction:

$pH$ and $pOH$ can be calculated using the below mentioned equations;

$pH= -log[H3O+]pOH = -log[OH-]$

The $pH and pOH$ of a water solution at $250C$ are related by the following equation,

$pH+ pOH = 14$

Molarity is the amount of moles of a compound dissolved in an amount of solvent (in liters)

$Molarity (M) = Moles of soluteLiters of solution$

Answer 9

(b)

Interpretation Introduction

Interpretation:

A $0.965 g$ sample of the mixture was dissolved in enough water to make $50.0mL$ of solution the $pH$ of this solution should be determined.

Concept introduction:

$pH$ and $pOH$ can be calculated using the below mentioned equations;

$pH= -log[H3O+]pOH = -log[OH-]$

The $pH and pOH$ of a water solution at $250C$ are related by the following equation,

$pH+ pOH = 14$

Molarity is the amount of moles of a compound dissolved in an amount of solvent (in liters)

$Molarity (M) = Moles of soluteLiters of solution$

Answer 10

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Answer 11

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Answer 12

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Answer 13

Ch. 19.1 - Prob. 19.1P Ch. 19.2 - Prob. 19.2P Ch. 19.2 - Prob. 19.3CP Ch. 19.4 - Prob. 19.4P Ch. 19.7 - Prob. 19.5P Ch. 19.8 - Prob. 19.6CP Ch. 19.10 - Prob. 19.7P Ch. 19.13 - Prob. 19.8CP Ch. 19.13 - Prob. 19.9P Ch. 19.14 - Prob. 19.10P

Solution Summary: The author explains how the molar mass of the two components in a mixture which shows the mass percent of nitrogen is determined.

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Chapter 19 Solutions