Which combinations will produce a precipitate

What is the relative density of silver? What is the dominant chemical present in vinegar? A Ethanol. B Ethylene glycol. C Sodium bicarbonate. D Sulphuric acid. A Uzbekistan. B USA. C India. D Kazakhstan.

A Perchloryl fluoride. B Phosphorus pentafluoride. C Phosphine. D Phosgene. A JJ Thomson. The net ionic equation only shows the precipitation reaction. A net ionic equation must be balanced on both sides not only in terms of atoms of elements, but also in terms of electric charge.

Precipitation reactions are usually represented solely by net ionic equations. If all products are aqueous, a net ionic equation cannot be written because all ions are canceled out as spectator ions. Therefore, no precipitation reaction occurs. Precipitation reactions are useful in determining whether a certain element is present in a solution. If a precipitate is formed when a chemical reacts with lead, for example, the presence of lead in water sources could be tested by adding the chemical and monitoring for precipitate formation.

In addition, precipitation reactions can be used to extract elements, such as magnesium from seawater. Precipitation reactions even occur in the human body between antibodies and antigens; however, the environment in which this occurs is still being studied.

Second, consult the solubility rules to determine if the products are soluble. The resulting equation is the following:. Third, separate the reactants into their ionic forms, as they would exist in an aqueous solution.

Be sure to balance both the electrical charge and the number of atoms:. Lastly, eliminate the spectator ions the ions that occur on both sides of the equation unchanged. In this case, they are the sodium and chlorine ions. The final net ionic equation is:. After balancing, the resulting equation is as follows:. Separate the species into their ionic forms, as they would exist in an aqueous solution. Balance the charge and the atoms. Cancel out all spectator ions those that appear as ions on both sides of the equation.

This particular example is important because all of the reactants and the products are aqueous, meaning they cancel out of the net ionic equation. There is no solid precipitate formed; therefore, no precipitation reaction occurs.

Write the net ionic equation for the potentially double displacement reactions. Make sure to include the states of matter and balance the equations.

After dissociation, the ionic equation is as follows:. The ionic equation is after balancing :. This means that both the products are aqueous i. According to the solubility rules , all silver salts are insoluble in water with the exception of silver nitrate, silver acetate and silver sulfate.

Therefore, AgBr will precipitate out. The other compound Mg NO 3 2 will remain in solution because all nitrates, NO 3 - , are soluble in water. KNO 3 will remain in solution since all nitrates are soluble in water. Chlorides are soluble in water with the exception of silver, lead and mercury. This means PbCl 2 is insoluble and form a precipitate.

There are many other factors that can affect solubility, but these rules are a good first step to determine the outcome of aqueous solution reactions. The key to predicting a precipitate is to learn the solubility rules. Pay particular attention to compounds listed as "slightly soluble" and remember that temperature affects solubility.

For example, a solution of calcium chloride is typically considered soluble in water, yet if the water is cold enough, the salt doesn't readily dissolve. Transition metal compounds may form a precipitate under cold conditions, yet dissolve when it's warmer.

Also, consider the presence of other ions in a solution. This can affect solubility in unexpected ways, sometimes causing a precipitate to form when you didn't expect it. Actively scan device characteristics for identification. Use precise geolocation data. Select personalised content. Create a personalised content profile.

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