Molar solubility, calculating

Calculate the of the following compounds, given their molar solubilities. [Pg.446]

EXAMPLE 11.12 Calculating molar solubility in the presence of complex formation... [Pg.594]

Self-Test 11.15A Use data from Tables 1 L.4 and 11.5 to calculate the molar solubility of silver bromide in 1.0 M NH3(aq). [Pg.595]

Use the data in Table 11.4 to calculate the molar solubility of each sparingly soluble substance in its respective solution ... [Pg.600]

A classic pharmaceutical science textbook might have defined poor solubility as anything below a solubility of 1 g mL-1 (2 mol L-1 solution for a molecular weight of 500 Da) at pH 6.5 (or pH 7). This classic view is reflected in the Chemical Abstracts SciFinder 2001 solubility range definitions for solubility calculated using Advanced Chemistry Development (ACD) Software Solaris V4.67. These semi-quantitative ranges for molar solubility are very soluble, 1 mol L 1 < solubility soluble, 0.1 mol L 1 < solubility < 1 mol L 1 slightly soluble, 0.01 mol L 1 <... [Pg.222]

Plan (1) Calculate the molar solubility of the slightly soluble salt, which is the number of moles of the salt... [Pg.337]

Note Values for molar solubility and [OH-] were rounded to 2 significant figures after calculating them. [Pg.346]

Plan Calculate the molar solubility of the metal hydroxides, then determine [OH-] and pOH. [Pg.437]

Now we can employ equation 19.4 to calculate the molar solubility of Mg(OH)2 in the buffer solution Molar Solubility Mg(OH)2 = [Mg2+]equii... [Pg.455]

Calculate the molar solubility of calcium carbonate, CaC03 that will dissolve in each of the following. The Ksp for calcium carbonate is 8.7 X 10-9. [Pg.249]

Le Chatelier s principle is a powerful tool for explaining how a reaction at equilibrium shifts when a stress is placed on the system. In this experiment, you can use Le Chatelier s principle to evaluate the relative solubilities of two precipitates. By observing the formation of two precipitates in the same system, you can infer the relationship between the solubilities of the two ionic compounds and the numerical values of their solubility product constants (K ). You will be able to verify your own experimental results by calculating the molar solubilities of the two compounds using the Ksp for each compound. [Pg.70]

Calculate the molar solubilities of the two ionic compounds from their Ksp values. [Pg.70]

Using Numbers Calculate the molar solubilities of the two precipitates using the Ks values. Which of the precipitates is more soluble ... [Pg.72]

In this section, you determined the solubility product constant, Kgp, based on solubility data. You obtained your own solubility data and used these data to calculate a value for Kgp. You determined the molar solubility of ionic solutions in pure water and in solutions of common ions, based on their Ksp values. In section 9.3, you will further explore the implications of Le Chatelier s principle. You will use a reaction quotient, Qsp, to predict whether a precipitate forms. As well, you will learn how selective precipitation can be used to identify ions in solution. [Pg.442]

To illustrate your answer, calculate and compare the molar solubility of silver chloride, AgCl (Kgp = 1.8 x 10 ), with silver chromate,... [Pg.442]

Explain how to calculate the molar solubility of a pure substance in water or in a solution of a common ion, given Kgp. [Pg.452]

If the salts are not of the same kind, molar solubilities of each salt must be calculated to compare their solubilities. For example, although the solubility product constant of Ag2Cr04 is smaller than that of AgCl, the former is more soluble than the latter. [Pg.90]

Calculate the molar solubility of CaF2 in each of the following ... [Pg.100]

One of the simplest ways to determine Ksp is to measure the molar solubility of the compound, the molarity of the compound in a saturated solution, but more advanced and accurate methods are also available. Table 11.5 gives some experimental values. In the following calculations, we use s to denote the numerical value of the molar solubility expressed in moles per liter for example, if the molar solubility of a compound is 6.5 X 10 s moFL-1, we write s = 6.5 X 10-5. [Pg.677]

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