Big Chemical Encyclopedia

Chemical substances, components, reactions, process design ...

Articles Figures Tables About

Chemical equations total ionic equation

In this chapter we examine some types of chemical reactions. Millions of reactions are known, so it is useful to group them into classes, or types, so that we can deal systematically with these massive amounts of information. We will describe how some compounds behave in aqueous solution, including how well their solutions conduct electricity and whether or not the compounds dissolve in water. We introduce several ways to represent chemical reactions in aqueous solution—formula unit equations, total ionic equations, and net ionic equations—and the advantages and disadvantages of these methods. [Pg.123]

O Briefly compare the relationships among a chemical formula, a total ionic equation, and a net ionic equation. Use sentences or a graphic organizer. [Pg.347]

Total ionic equation An equation for a chemical reaction written to show the predominant form of all species in aqueous solution or in contact with water. [Pg.168]

A molecular equation for an aqueous ionic reaction shows undissociated substances. A total Ionic equation shows all soluble Ionic compounds as separate, solvated ions. Spectator ions appear unchanged on both sides of the equation. By eliminating them, you see the actual chemical change in a net ionic equation. [Pg.115]

Total ionic equation (3.3) A chemical equation in which all ions and molecules present in solution, including spectator ions, are shown. [Pg.635]

Ions that appear In the same form in solution on both sides of the total ionic equation are called spectator ions they undergo no change in the chemical reaction. [Pg.216]

Three types of equations describe an aqueous reaction. A molecular equation shows all substances as intact compounds. A total ionic equation shows ions for all soluble substances. A net ionic equation is more useful because it omits spectator ions (those not involved in the reaction) and shows the actual chemical change taking place. Section 4.2)... [Pg.115]

A total ionic equation tells more than just what happens in a chemical change. It includes spectator ions, or simply spectators. A spectator is an ion that is present at the scene of a reaction but experiences no chemical change. It appears on both sides of the total ionic equation. Na+(aq) and N03 (aq) are spectators in Equation 9.2. To change a total ionic equation into a net ionic equation, you remove the spectators ... [Pg.241]

The simplest balanced chemical equation for a precipitation reaction is a net ionic equation that has ions as the reactants and a neutral solid as the product. In a precipitation reaction, reactant ions combine to form a neutral ionic solid. One reactant carries positive charge and the other carries negative charge, but the product is electrically neutral. Because electrical charge always is conserved, the total positive charge of the reacting cations... [Pg.226]

Net ionic equations (Chapter 9), like all other balanced chemical equations, give the mole ratios of reactants and products. Therefore, any calculations that require mole ratios may be done with net ionic equations as well as with total equations. However, a net ionic equation does not yield mass data directly because part of each soluble ionic compound is not given. For example, we can tell how many moles of silver ion are required to produce a certain number of moles of a product. [Pg.290]

The electrolysis of brine (concentrated NaCl solution) produces hydrogen at the cathode and chlorine at the anode. Write a net ionic equation for each half-reaction and the total reaction. What other chemical is produced in this commercially important process ... [Pg.214]

Net ionic equations allow us to focus on the essence of a chemical reaction in aqueous solutions. On the other hand, if we are dealing with stoichiometric calculations we frequently must deal with formula weights and therefore with the complete formulas of all species. In such cases, formula unit equations are more useful. Total ionic equations provide the bridge between the two. [Pg.136]

First we will use the nomenclature rules that we presented in Chapter 2 to write formulas for all of the compounds involved. Then we construct a balanced chemical equation using complete formula units. Next we must identify any ionic compounds that are present, and we write them as dissociated ions to give the total ionic equation. Finally, to obtain the net ionic equation, we must eliminate any spectator ions from both sides of the equation. [Pg.98]

The input of the problem requires total analytically measured concentrations of the selected components. Total concentrations of elements (components) from chemical analysis such as ICP and atomic absorption are preferable to methods that only measure some fraction of the total such as selective colorimetric or electrochemical methods. The user defines how the activity coefficients are to be computed (Davis equation or the extended Debye-Huckel), the temperature of the system and whether pH, Eh and ionic strength are to be imposed or calculated. Once the total concentrations of the selected components are defined, all possible soluble complexes are automatically selected from the database. At this stage the thermodynamic equilibrium constants supplied with the model may be edited or certain species excluded from the calculation (e.g. species that have slow reaction kinetics). In addition, it is possible for the user to supply constants for specific reactions not included in the database, but care must be taken to make sure the formation equation for the newly defined species is written in such a way as to be compatible with the chemical components used by the rest of the program, e.g. if the species A1H2PC>4+ were to be added using the following reaction ... [Pg.123]

In the case of an - electrolyte dissociating in solution as Aj,+ Bj, < is+Az+ + z/ Bz where v+z+ = v z to ensure electroneutrality, and the total number of particles formed by each molecule is v = v+ + z/, then the only activity that can be measured is that of the complete species, and the individual ions cannot be assigned meaningful chemical potentials. Under these circumstances, a mean activity coefficient is defined through the equation yv = y++ yvs. Since individual ionic chemical potentials are not measurable, it has become conventional to assign to the chemical potential of the hydrogen ion under standard conditions the value of zero, allowing relative chemical potentials for all other ions to be formulated. [Pg.11]

Equation (10) shows that the isomer shift IS is a direct measure of the total electronic density at the probe nucleus. This density derives almost exclusively from 5-type orbitals, which have non-zero electron densities at the nucleus. Band electrons, which have non-zero occurrence probabilities at the nucleus and 5-type conduction electrons in metals may also contribute, but to a lesser extent. Figure 3 shows the linear correlation that is observed between the experimental values of Sb Mossbauer isomer shift and the calculated values of the valence electron density at the nucleus p (0). The total electron density at the nucleus p C ) (Eq. 10) is the sum of the valence electron density p (0) and the core electron density p (0), which is assumed to be constant. This density is not only determined by the 5-electrons themselves but also by the screening by other outer electrons p-, d-, or /-electrons) and consequently by the ionicity or covalency and length of the chemical bonds. IS is thus a probe of the formal oxidation state of the isotope under investigation and of the crystal field around it (high- and low-spin Fe may be differentiated). The variation of IS with temperature can be used to determine the Debye temperature of a compound (see Eq. (13)). [Pg.317]

The previous findings, however, cannof be generalized to the precipitant species or species other than the hardness and its associated ionic species. Eor example, in Equation (10.16), if the above findings were applied to the precipitant Ca(OH)2, its equivalent mass would be Ca(OH)2/2 however, this is not correct— the equivalent mass of Ca(OH)2 in this equation is 2Ca(OH)2/2. To conclude, the equivalent mass of a precipitant species or species other than the hardness and its associated species cannot be generalized as molecular mass divided by the total number of valences of the species but must be deduced from the chemical reaction. [Pg.506]


See other pages where Chemical equations total ionic equation is mentioned: [Pg.611]    [Pg.679]    [Pg.267]    [Pg.847]    [Pg.847]    [Pg.716]    [Pg.464]    [Pg.606]    [Pg.9]    [Pg.25]    [Pg.51]    [Pg.1179]    [Pg.206]    [Pg.515]    [Pg.329]    [Pg.691]    [Pg.61]    [Pg.741]    [Pg.861]   
See also in sourсe #XX -- [ Pg.114 , Pg.114 , Pg.115 , Pg.122 ]

See also in sourсe #XX -- [ Pg.94 ]

See also in sourсe #XX -- [ Pg.114 , Pg.114 , Pg.115 , Pg.118 , Pg.122 ]

See also in sourсe #XX -- [ Pg.120 , Pg.121 , Pg.128 ]




SEARCH



Chemicals equations

Equation total

Equations ionic

Equations total ionic equation

Total ionic equation

© 2024 chempedia.info