/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 60 A precipitate may appear when tw... [FREE SOLUTION] | 91影视

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Chapter 8: Problem 60

A precipitate may appear when two completely clear aqueous solutions are mixed. What circumstances are responsible for this event?

Short Answer

Expert verified
Answer: A precipitate forms when two clear aqueous solutions are mixed if the combination of ions in the solutions leads to the formation of an insoluble product as a result of a chemical reaction. Factors contributing to precipitate formation include solubility rules, concentration, temperature, and pH changes.

Step by step solution

01

Understanding precipitate formation

When two clear aqueous solutions are mixed, a precipitate may appear if the combination of ions in the solutions leads to the formation of an insoluble product. This process typically occurs as a result of a chemical reaction taking place between the ions present in the two original solutions.
02

Identifying the key factors contributing to precipitate formation

There are several factors that contribute to the formation of a precipitate when clear aqueous solutions are mixed, including: 1. Solubility Rules: Certain combinations of ions produce insoluble compounds, leading to the formation of a precipitate. These solubility rules are based on empirical observations and allow us to predict whether a particular combination of ions will form a precipitate or not. 2. Concentration: The concentration of the ions in the solutions plays a crucial role in determining whether a precipitate will form. If the concentration of the ions is high enough to exceed the solubility of the insoluble compound, a precipitate will form. 3. Temperature: The solubility of some compounds is temperature-dependent. A precipitate may form if the temperature of the reaction is such that the solubility of the produced compound is decreased. 4. pH: Changes in pH can also lead to precipitate formation as some compounds may become more or less soluble depending on the pH of the solution.
03

Explaining examples of precipitate formation

Here are some examples to illustrate the concept of precipitate formation: 1. Mixing silver nitrate (AgNO3) and sodium chloride (NaCl) solutions: In this case, silver nitrate and sodium chloride react to form insoluble silver chloride (AgCl) and sodium nitrate (NaNO3), which remains dissolved in the solution: AgNO3(aq) + NaCl(aq) 鈫� AgCl(s) + NaNO3(aq) The precipitate formed here is silver chloride (AgCl). 2. Mixing barium chloride (BaCl2) and sodium sulfate (Na2SO4) solutions: In this reaction, the resulting products are barium sulfate (BaSO4), which is insoluble and forms a precipitate, and sodium chloride (NaCl), which remains dissolved in the solution: BaCl2(aq) + Na2SO4(aq) 鈫� BaSO4(s) + 2NaCl(aq) The precipitate formed here is barium sulfate (BaSO4). From the given examples, it can be concluded that a precipitate forms when two completely clear aqueous solutions are mixed if the chemical reaction taking place between the ions present in the solutions produces an insoluble compound.

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Most popular questions from this chapter

A method for determining the quantity of dissolved oxygen in natural waters requires a series of redox reactions. Balance the following chemical equations in that series under the conditions indicated: a. \(\mathrm{Mn}^{2+}(a q)+\mathrm{O}_{2}(g) \rightarrow \mathrm{MnO}_{2}(s)\) (basic solution) b. \(\mathrm{MnO}_{2}(s)+\mathrm{I}^{-}(a q) \rightarrow \mathrm{Mn}^{2+}(a q)+\mathrm{I}_{2}(s)\) (acidic solution) c. \(\mathrm{I}_{2}(s)+\mathrm{S}_{2} \mathrm{O}_{3}^{2-}(a q) \rightarrow\) \(\mathrm{I}^{-}(a q)+\mathrm{S}_{4} \mathrm{O}_{6}^{2-}(a q) \quad\) (neutral solution)

A puddle of coastal seawater, caught in a depression formed by some coastal rocks at high tide, begins to evaporate on a hot summer day as the tide goes out. If the volume of the puddle decreases to \(23 \%\) of its initial volume, what is the concentration of \(\mathrm{Na}^{+}\) after evaporation if it was \(0.449 \mathrm{M}\) initially?

Near Las Vegas, NV, improper disposal of perchlorates used to manufacture rocket fuel contaminated a stream flowing into Lake Mead, the largest artificial lake in the United States and a major supply of drinking and irrigation water for the American Southwest. The U.S. EPA has proposed an advisory range for perchlorate concentrations in drinking water of 4 to \(18 \mu \mathrm{g} / \mathrm{L} .\) The perchlorate concentration in the stream averages \(700.0 \mu \mathrm{g} / \mathrm{L},\) and the stream flows at an average rate of 161 million gallons per day \((1 \text { gal }=3.785\) L) a. What are the formulas of sodium perchlorate and ammonium perchlorate? b. How many kilograms of perchlorate flow from the Las Vegas stream into Lake Mead each day? c. What volume of perchlorate-free lake water would have to mix with the stream water each day to dilute the stream's perchlorate concentration from 700.0 to \(4 \mu \mathrm{g} / \mathrm{L} ?\) d. since \(2003,\) the states of Maryland, Massachusetts, and New Mexico have limited perchlorate concentrations in drinking water to \(0.1 \mu \mathrm{g} / \mathrm{L} .\) Five replicate samples were analyzed for perchlorates by laboratories in each state, and the following data ( \(\mu \mathrm{g} / \mathrm{L}\) ) were collected: $$\begin{array}{ccc} \mathrm{MD} & \mathrm{MA} & \mathrm{NM} \\ 1.1 & 0.90 & 1.2 \\ \hline 1.1 & 0.95 & 1.2 \\ \hline 1.4 & 0.92 & 1.3 \\ \hline 1.3 & 0.90 & 1.4 \\ \hline 0.9 & 0.93 & 1.1 \\ \hline \end{array}$$Which of the labs produced the most precise analytical results?

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A solution of table salt is a good conductor of electricity, but a solution containing an equal molar concentration of table sugar is not. Why?
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