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Acid salt is a somewhat obscure term for a class of salts formed by the partial neutralization of diprotic or polyprotic acids. Because the parent acid is only partially neutralized, one or more replaceable hydrogen ions remain. Typical acid salts have one or more alkali (alkaline) metal ions as well as one or more protons. Well known examples are sodium bicarbonate (NaHCO3), sodium hydrosulfide (NaHS), sodium bisulfate (NaHSO4), monosodium phosphate (NaH2PO4), and disodium phosphate (Na2HPO4). Often acid salts are used as buffers.
- H2SO4 + NaOH → NaHSO4 + H2O
Acid salts compounds can act either as an acid or a base: addition of a suitably strong acid will restore protons, and addition of a suitably strong base will remove protons. The pH of a solution of an acid salt will depend on the relevant equilibrium constants and the amounts of any additional base or acid. A comparison between the Kb and Ka will indicate this: if Kb > Ka, the solution will be basic, whereas if Kb < 'Ka, the solution will be acidic.
Use in food
Some acid salts are used in baking. They are found in baking powders and are typically divided into low-temperature (or single-acting) and high-temperature (or double-acting) acid salts. Common low-temperature acid salts react at room temperature to produce a leavening effect. They include cream of tartar, calcium phosphate, and citrates. High-temperature acid salts produce a leavening effect during baking and are usually aluminium salts such as calciumaluminium phosphate. Some acid salts may also be found in non-dairy coffee creamers.
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Answers:Are you sure you got the number right for gastric juice? If your teacher really wrote 7.25 on the quiz, then the answer is slightly basic, because anything with a pH greater than 7 is basic. Since 7.25 is just a little bit greater than 7, I would call this slightly basic. However, in reality gastric juice is very acidic with a pH around 2, and it is referred to as both gastric juice and gastric acid. As for why it is basic or acidic, this is based on the definition of these terms. Any solution with a pH greater than 7 is by definition basic, and any solution with a pH less than 7 is by definition acidic. So if your teacher gives you the pH, you just need to determine if it is greater or less than 7, and do not need to know anything else about the solution. Phosphoric acid, H3PO4, has three acidic OH groups, and each one is capable of losing a hydrogen. If you're just talking about dihydrogen phoshpate, then hydrogen is the cation and dihydrogen phoshpate is the anion. A buffer system allows you to maintain the solution at a roughly constant pH even while adding acidic or basic molecules to solution. If you add a few drops of hydrochloric acid to a beaker of pure water, or to a beaker containing an non-buffered aqueous solution, there will be a dramatic change in pH and the solution will become more acidic (how much it changes depends on the exact amount of water and hydrochloric acid you are using). However, if you have a buffer that can act as a base at pH of your solution, it will bind to the hydrogen ions released by hydrochloric acid, there will be no increase in the concentration of "free hydrogen ions" (which are actually hydronium ions, H3O+). If you add too much of an acid or a base, you will overwhelm the buffer and eventually you will be able to change the pH of the solution. Each buffer works over a specific range of pH values. Phosphoric acid/phosphates are excellent buffers because of the three acidic groups. Each hydrogen can bond to or dissociate from its oxygen over a specific range of pH values, but the range is different for each of the three acidic groups. Buffer systems with only one acidic group are effective over a much narrower pH range. To determine which buffer system is appropriate for a given experiment, you need to know the Ka (acid dissociation constant) or pKa for each acidic group in the molecule. Phosphoric acid has three Ka's, one for each of its three acidic groups. When determining which is the cation and which is the anion, it does not make a difference whether or not you are using Arrhenius acid-base theory or Br nsted-Lowry acid-base theory, except some Br nsted-Lowry reactions do not involve ionic reactants or products. The Wikipedia aritcle on acids has a brief description of the three major acid-base theories, and while it does not answer your question directly, the section on Br nsted-Lowry theory gives an example of reactions that do not involve ions, and the entire section discusses how all of the different definitions of an acid (or a base) relate to each other: http://en.wikipedia.org/wiki/Acid#Technical_definitions .
Answers:A SALT HAHAHAH, nah not really its an acid and a base
Answers:acids containds hydrogen so they always have a H infront of it: hydrochloric acid: HCL sulfuric acid: H2SO bases contains hydroxide, so if you see an OH, it is a base: sodium hydroxide: NaOH Calcium Hydroxide: Ca2(OH)2 for salts it depends what kind of salt you're asking. for table salts they are a ionic compound: NaCl hope this helps :)
Answers:17 neutral 18 acidic 19 basic impossible to predict ( Ka and Kb are required)