Weak 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. 

Skill 16.6 Identifying properties of strong and weak electrolyte solutions... 

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

The transition was found to be mediated by nucleation and traveling of sharp fronts (Fig. 11a) that indicates a backward bifurcation, although hysteresis has not been identified directly. Rather, a sharp jump in the contrast (pattern amplitude) with increasing voltage has been detected, with some indications that a low contrast pattern already arises at voltages before the jump occurs in Fig. 1 lb. A preliminary, weakly non-linear analysis has exhibited a bifurcation, which is in fact weakly supercritical at low frequencies. If small changes of the parameters and/or additional effects are included (e.g. flexoelectricity and weak-electrolyte effects) the bifurcation could become a more expressed subcritical one [32, 33]. 

Your goal is to determine which chemical species is solution A, which chemical species is solution B, and so forth, and to enter your conclusions in TABLE 44.1. You may also be asked to identify any precipitates produced, gases evolved, or weak electrolytes formed during your experimentation and to write balanced chemical equations to describe any reactions that you observe. 

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. 

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). 

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). 

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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