Net ionic

A standard method for prepanng sodium cyclopentadienide (CsHsNa) is by the reaction of cyclopentadiene with a solution of NaNH2 in liquid ammonia Write a net ionic equation for this reaction identify the acid and the base and use curved arrows to track the flow of electrons... [Pg.470]

A precipitation reaction occurs when two or more soluble species combine to form an insoluble product that we call a precipitate. The most common precipitation reaction is a metathesis reaction, in which two soluble ionic compounds exchange parts. When a solution of lead nitrate is added to a solution of potassium chloride, for example, a precipitate of lead chloride forms. We usually write the balanced reaction as a net ionic equation, in which only the precipitate and those ions involved in the reaction are included. Thus, the precipitation of PbCl2 is written as... [Pg.139]

The emphasis is on writing and balancing chemical equations for these reactions. All of these reactions involve ions in solution. The corresponding equations are given a special name net ionic equations. They can be used to do stoichiometric calculations similar to those discussed in Chapter 3. [Pg.75]

Write a net ionic equation for any precipitation reaction that occurs when solutions of the following ionic compounds are mixed. [Pg.79]

Click Coached Problems for a self-study module on net ionic equations. [Pg.79]

To write a net ionic equation, you first have to identify the ions. [Pg.79]

For any reaction in water solution, always start with a balanced net ionic equation. [Pg.80]

Although we have introduced net ionic equations to represent precipitation reactions, they have a much wider application. Indeed, we will use them for all kinds of reactions in water solution. In particular all of the chemical equations written throughout this chapter are net ionic equations. [Pg.80]

The approach followed in Chapter 3 to calculate mole-mass relations in reactions is readily applied to solution reactions represented by net ionic equations. [Pg.80]

For the reaction between solutions of sodium hydroxide and hydrogen fluoride, the net ionic equation is... [Pg.83]

Here, as always, spectator ions such as Na+ are not included in the net ionic equation. [Pg.83]

The overall equation is obtained by summing those for the individual steps. Canceling species (OH-, HzO) that appear on both sides, we obtain the net ionic equation... [Pg.83]

The experimental setup for a titration is shown in Figure 4.7. The flask contains vinegar, a water solution of a weak organic add called acetic acid. A solution of sodium hydroxide of known concentration is added from a buret. The net ionic equation for the acid-base reaction that occurs is... [Pg.84]

In a redox reaction, one species loses (i.e., donates) electrons and is said to be oxidized. The other species, which gains (or receives) electrons, is reduced. To illustrate, consider the redox reaction that takes place when zinc pellets are added to hydrochloric acid (Figure 4.8). The net ionic equation for the reaction is... [Pg.86]

An easy way to recognize a redox equation is to note changes in oxidation number of two different elements. The net ionic equation... [Pg.88]

With the aid of Tables 4.1 and 4.2, write net ionic equations for acid-base reactions. (Example 4.6 Problems 29-36) 27,33... [Pg.94]

Decide whether a precipitate will form when the following solutions are mixed. If a precipitate forms, write a net ionic equation for the reaction,... [Pg.96]

Write a balanced net ionic equation for each of the following add-base reactions in water. [Pg.96]

Write balanced net ionic equations for the following reactions in acid solution. [Pg.98]

Assuming that the circles represent cations and squares represent anions, match the incomplete net ionic equations to their pictorial representations... [Pg.99]

Given the following descriptions of reversible reactions, write a balanced net ionic equation (simplest whole-number coefficients) and die equilibrium constant expression (X) for each. [Pg.345]

Classify a species as a Bronsted-Lowry acid or base and explain by a net ionic equation. (Examples 13.1,13.4,13.10 Problems 1-12) Questions and Problems assignable in OWL 2,4,12,34,64... [Pg.376]

Write net ionic equations to explain the acidity or basicity of the various salts listed in Question 79. [Pg.379]

As pointed out in Chapter 13, strong acids ionize completely in water to form H30+ ions strong bases dissolve in water to form OH- ions. The neutralization reaction that takes place when any strong acid reacts with any strong base can be represented by a net ionic equation of the Bronsted- Lowry type ... [Pg.394]

A typical weak acid-strong base titration is that of acetic acid with sodium hydroxide. The net ionic equation for the reaction is... [Pg.396]

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