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Chapter 3: Problem 32

Phosphoric acid, \(\mathrm{H}_{3} \mathrm{PO}_{4}\), is used to make phosphate fertilizers and detergents and is also used in carbonated beverages. What is the molar mass of \(\mathrm{H}_{3} \mathrm{PO}_{4}\) ?

Short Answer

Expert verified
The molar mass of \(\mathrm{H}_{3} \mathrm{PO}_{4}\) is 98 g/mol.

Step by step solution

01

Identify the Formula

We are given the chemical formula for phosphoric acid, which is \(\mathrm{H}_{3} \mathrm{PO}_{4}\). To find the molar mass, we need to determine the atomic masses of each element in the compound.
02

Determine Atomic Masses

Look up the atomic masses of each element: Hydrogen (H) has an atomic mass of approximately 1 g/mol, Phosphorus (P) has an atomic mass of approximately 31 g/mol, and Oxygen (O) has an atomic mass of approximately 16 g/mol.
03

Calculate the Contribution of Each Element

Calculate the total mass contribution of each element based on its stoichiometric coefficient in the compound:- For \(\mathrm{H}_{3}\): \(3 \times 1 = 3 \text{ g/mol}\)- For \(\mathrm{P}_{1}\): \(1 \times 31 = 31 \text{ g/mol}\)- For \(\mathrm{O}_{4}\): \(4 \times 16 = 64 \text{ g/mol}\)
04

Sum the Contributions

Add the contributions of all the elements to obtain the molar mass of \(\mathrm{H}_{3} \mathrm{PO}_{4}\):\(3 + 31 + 64 = 98 \text{ g/mol}\).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Phosphoric Acid
Phosphoric acid is a chemical compound with the formula \( \mathrm{H}_3\mathrm{PO}_4 \). It is an important industrial chemical used in the manufacture of fertilizers, detergents, and various industrial processes. Interestingly, phosphoric acid is also an additive in food products like carbonated beverages to enhance flavor.
  • Phosphoric acid is often seen as a colorless and odorless liquid.
  • It has corrosive properties, and thus, safety precautions are necessary when handling it.
  • In a laboratory context, the 'formula unit' of phosphoric acid gives us a clear view of its elemental composition, which is vital for calculating properties like molar mass.
Understanding the applications and properties of phosphoric acid gives us context for why we calculate its molar mass, which helps in determining how much substance is needed for chemical reactions.
Atomic Mass
Atomic mass is the mass of an atom expressed in atomic mass units (amu). It approximates the average mass of naturally occurring isotopes of an element. Knowing atomic masses is crucial for calculating the molar mass of compounds.
  • Each element has a unique atomic mass, determined by the number of protons and neutrons in its nucleus.
  • For hydrogen, phosphorus, and oxygen, the atomic masses are approximately 1 g/mol, 31 g/mol, and 16 g/mol, respectively.
  • Using these values, we can determine how much each element contributes to the total mass of a compound like phosphoric acid.
When dealing with compounds, the atomic mass of each constituent element must be considered. This becomes particularly relevant for quantitative chemistry tasks such as stoichiometry.
Chemical Formula
A chemical formula is a concise way of expressing information about the atoms that constitute a particular chemical compound. For phosphoric acid, the chemical formula is \( \mathrm{H}_3\mathrm{PO}_4 \).
  • This formula reveals that each molecule of phosphoric acid contains three hydrogen atoms, one phosphorus atom, and four oxygen atoms.
  • Understanding a chemical formula allows chemists to predict how a substance will behave in various chemical reactions.
  • The subscripts in the formula are essential as they indicate the amount of each type of atom present, which is vital for calculating molar mass and for performing stoichiometric calculations.
By mastering the interpretation of chemical formulas, chemistry students can accurately compute molar masses and engage in chemical reaction predictions.
Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions. It is based on the conservation of mass and atoms in chemical reactions.
  • In stoichiometry, the coefficients in a chemical equation indicate the ratio of moles of each substance involved.
  • To compute an accurate stoichiometric calculation, you need to know the molar masses, derived from atomic masses, of all compounds involved.
  • Taking phosphoric acid as an example, its molar mass (98 g/mol) is crucial in determining the quantities required for or produced by a reaction.
The principles of stoichiometry allow scientists to predict the outcomes of chemical reactions quantitatively, making it possible to design reactions with specific outcomes and control the proportions of products formed.

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Most popular questions from this chapter

A sample of limestone (containing calcium carbonate, \(\mathrm{CaCO}_{3}\) ) weighing \(438 \mathrm{mg}\) is treated with oxalic acid, \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4},\) to give calcium oxalate, \(\mathrm{CaC}_{2} \mathrm{O}_{4}\) $$ \mathrm{CaCO}_{3}(s)+\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(a q) \longrightarrow \mathrm{CaC}_{2} \mathrm{O}_{4}(s)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g) $$ The mass of the calcium oxalate produced is \(469 \mathrm{mg}\). What is the mass percentage of calcium carbonate in this limestone?

Ethylene glycol is used as an automobile antifreeze and in the manufacture of polyester fibers. The name glycol stems from the sweet taste of this poisonous compound. Combustion of \(6.38 \mathrm{mg}\) of ethylene glycol gives \(9.06 \mathrm{mg}\) \(\mathrm{CO}_{2}\) and \(5.58 \mathrm{mg} \mathrm{H}_{2} \mathrm{O} .\) The compound contains only \(\mathrm{C}, \mathrm{H}\) and \(\mathrm{O}\). What are the mass percentages of the elements in ethylene glycol?

Caffeine, the stimulant in coffee and tea, has the molecular formula \(\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{O}_{2} .\) Calculate the mass percentage of each element in the substance. Give the answers to three significant figures.

Acrylonitrile, \(\mathrm{C}_{3} \mathrm{H}_{3} \mathrm{~N},\) is the starting material for the production of a kind of synthetic fiber (acrylics). It can be made from propylene, \(\mathrm{C}_{3} \mathrm{H}_{6},\) by reaction with nitric oxide, NO. \(4 \mathrm{C}_{3} \mathrm{H}_{6}(g)+6 \mathrm{NO}(g) \longrightarrow 4 \mathrm{C}_{3} \mathrm{H}_{3} \mathrm{~N}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{N}_{2}(g)\) How many grams of acrylonitrile are obtained from \(452 \mathrm{~kg}\) of propylene and excess \(\mathrm{NO} ?\)

Morphine, a narcotic substance obtained from opium, has the molecular formula \(\mathrm{C}_{17} \mathrm{H}_{19} \mathrm{NO}_{3} .\) What is the mass percentage of each element in morphine (to three significant figures)?
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