1. Salts containing Group I elements are soluble (Li+, Na+, K+, Cs+, Rb+). Exceptions to this rule are rare. Salts containing the ammonium ion (NH4+) are also soluble. Show This offering of solubility rules is in the public domain and may be copied without restriction. The user is encouraged to download it for private use and public distribution in any form, including that of making it available on other Web servers. Send a message to Oliver Seely about this table? --> Start by writing the chemical formulas of the reactants and of the products.
Now, your reaction takes place in aqueous solutions. Three of the four chemical species involved in the reaction will be in the aqueous state, #"(aq)"#, and one, potassium iodide, will be in the solid state, #"(s)"#. The unbalanced chemical equation looks like this
To balance this chemical equation, multiply the potassium iodide by #2# and the potassium nitrate by #2#. You will end up with
If you want, you can write the complete ionic equation by breaking up the soluble compounds, i.e. the ones that are in the aqueous state, into their respective cations and anions
If you eliminate the spectator ions, i.e. the ions that are present on both sides of the equation
you will get the net ionic equation
Lead(II) iodide is a yellow insoluble solid that precipitates out of the solution. A solubility chart is a chart with a list of ions and how, when mixed with other ions, they can become precipitates or remain aqueous. The following chart shows the solubility of multiple independent and various compounds, in water, at a pressure of 1 atm and at room temperature (approx. 25 °C (298.15 K)). Any box that reads "soluble" results in an aqueous product in which no precipitate has formed, while "slightly soluble" and "insoluble" markings mean that there is a precipitate that will form (usually, this is a solid); however, "slightly soluble" compounds such as calcium sulfate may require heat to form its precipitate. Boxes marked "other" can mean that many different states of products can result. For more detailed information of the exact solubility of the compounds, see the solubility table. For compounds with multiple hydrates, the most solubility of the most soluble hydrate is shown in this chart. Some compounds, such as nickel oxalate, will not precipitate immediately even though it is insoluble and requires a few minutes to precipitate out.[1]
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Are halide salts soluble in water?Halides exist in natural water sources, such as rivers, lakes, and streams, due to their high solubility in water.
Are halides generally soluble or insoluble?All NITRATES are soluble; and ALL halides are soluble EXCEPT for those of Pb2+ , Hg2+2 , mercurous ion , and Ag+ in aqueous solution.
Which halide is most soluble?Therefore, the most soluble halide in water is Silver fluoride .
Are most nitrate salts soluble in water?The nitrates, chlorates, and acetates of all metals are soluble in water.
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