Strong electrolytes identifying

To test the validity of the extended Pitzer equation, correlations of vapor-liquid equilibrium data were carried out for three systems. Since the extended Pitzer equation reduces to the Pitzer equation for aqueous strong electrolyte systems, and is consistent with the Setschenow equation for molecular non-electrolytes in aqueous electrolyte systems, the main interest here is aqueous systems with weak electrolytes or partially dissociated electrolytes. The three systems considered are the hydrochloric acid aqueous solution at 298.15°K and concentrations up to 18 molal the NH3-CO2 aqueous solution at 293.15°K and the K2CO3-CO2 aqueous solution of the Hot Carbonate Process. In each case, the chemical equilibrium between all species has been taken into account directly as liquid phase constraints. Significant parameters in the model for each system were identified by a preliminary order of magnitude analysis and adjusted in the vapor-liquid equilibrium data correlation. Detailed discusions and values of physical constants, such as Henry s constants and chemical equilibrium constants, are given in Chen et al. (11). 

Identify the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte. 

Using the following information, identify the strong electrolyte whose general formula is... 

Identify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte (a) H2O, (b) KCl, (c) HNO3, (d) CH3COOH, (e) C12FI22O11. 

Identify the two effects that lead to a decrease in A with concentration for strong electrolytes. 

In the following sections we will look at how a compound s composition lets us predict whether it is a strong electrolyte, weak electrolyte, or nonelectrolyte. For the moment, you need only to remember that water-soluble ionic compounds are strong electrolytes. Ionic compounds can usually be identified by the presence of both metals and nonmetals [for example, NaCl, FeS04, and A1(N03)3]. Ionic compounds containing the ammonium ion, NH [for example, NH4Br and (NH4)2C03], are exceptions to this rule of thumb. 

Net ionic equations illustrate the similarities between various reactions involving electrolytes. For example. Equation 4.8 expresses the essential feature of the precipitation reaction between any strong electrolyte containing Ph (aq) and any strong electrolyte containing l aq) The ions combine to form a precipitate of PM2. Thus, a net ionic equation demonstrates that more than one set of reactants can lead to the same net reaction. Eor example, aqueous solutions of KI and Mgl2 share many chemical similarities because both contain 1 ions. Either solution when mixed with a Pb(N03)2 solution produces Pbl2(s). The complete ionic equation, on the other hand, identifies the actual reactants that participate in a reaction. 

V TABLE 4.2 lists the strong acids and bases we are most likely to encounter. You need to commit this information to memory in order to correctly identify strong electrolytes and write net ionic equations. The brevity of this list tells us that most acids are weak. (For H2SO4, as we noted earlier, only the first proton completely ionizes.) The only common strong bases are the common soluble metal hydroxides. Most other metal hydroxides are insoluble in water. The most common weak base is NH3, which reacts with water to form OH ions (Equation 4.11). 

Aqueous solutions of three different substances, AX, AY, and AZ, are represented by the three accompanying diagrams. Identify each substance as a strong electrolyte, weak electrolyte, or non-electrolyte. [Section 4. f ]... 

Consider which solutes are strong electrolytes and which are weak electrolytes, and identify the major species in solution. 

The aqueous solutions of three compounds are shown in the diagram. Identify each compound as a nonelectrolyte, a weak electrolyte, and a strong electrolyte. 

First, identify the major species in solution and consider their acidity or basicity. Because HC2H3O2 is a weak electrolyte and NaC2H302 is a strong electrolyte, the major species in the solution are HC2H3O2 (a weak acid), Na (which is neither acidic nor basic), and C2H302 (which is the conjugate base of HC2H3O2). 

Identify strong electrolytes and calculate concentrations of their ions... 

A skill you need to write net ionic equations successfully is the ability to identify the major species in an aqueous solution. For each solute formula (in aqueous solution) written below, (a) classify it as a strong electrolyte, a weak electrolyte, or a... 

Think About It Make sure that you have conectly identified compounds that are ionic and compounds that are molecular. Remember that strong acids are strong electrolytes, weak acids and weak bases are weak electrolytes, and strong bases are strong electrolytes (by virtue of their being soluble ionic compounds). Molecular compounds, with the exceptions of acids and weak bases, are nonelectrolytes. 

Practice Problem A Identify the following compounds as nonelectrolytes, weak electrolytes, or strong electrolytes ethanol (C2H5OH), nitrous acid (HNO2), and sodium hydrogen carbonate (NaHCOs, also known as bicarbonate). 

Strategy Predict the products by exchanging ions and balance the equation. Determine which product will precipitate based on the solubility guidelines in Tables 4.2 and 4.3. Rewrite the equation showing strong electrolytes as ions. Identify and cancel spectator ions. 

Identify each of the following compounds as a nonelectrolyrte, a weak electrolyte, or a strong electrolyte (a) lactose (Ci2H220,i), (b) lactic acid (HC3H5O3), (c) dimethylamine [(CH3)2NH],... 

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