Is salt a neutral acid or alkali

Big Bang HTL 2, textbook

Inorganic Technology and Ecology (2nd year, 4th semester) 97 Acids and Bases 7 Neutral salt solutions are formed when strong acids and strong bases react. The resulting conjugated acids and bases show no tendency to release the absorbed H + ions again or, conversely, to take up released ones again. They mainly consist of the following ions: cations z. E.g .: alkali and alkaline earth ions (except Be +2) anions e.g. For example: Cl -, Br -, I - NO 3 - acidic salt solutions arise when the cation tries to give up H + ions because it was created from a weak base. In addition, small, strongly positively charged metal cations are acidic. They pull so strongly on the binding electrons in their hydration water that this releases H + ions. Cations e.g. B .: NH 4 +, Al 3+ Basic salt solutions are obtained from anions of weak acids, because these, as bases, tend to take up H + again. Anions e.g. B.: NO 2 -, CO 3 2–, CH 3 COO -, F -, OH - F27 Summary Acid and basic solutions react with each other in the so-called neutralization reaction. However, the resulting salt solutions are not always neutral. As a general rule: Salt from ... solution reacts ... strong acid + strong base neutral strong acid + weak base acidic weak acid + strong base basic If, however, weak acids react with weak bases, the salts can depending on the strength of the acids and bases react acidic, basic or neutral. Z Answer the following questions using the information from the book! Find the formulas of the following salts: a) calcium sulfate b) lithium hydrogen phosphate c) ammonium sulfite d) magnesium cyanide e) iron (III) nitrite f) aluminum carbonate L Determine for each of the following salts whether it forms a neutral, acidic or basic solution and name it Salt. a) Ba (NO 3) 2 b) NH 4 I c) K2CO 3 d) Ca (CH 3 COO) 2 e) AlCl 3 f) NaCl L 30ml of a nitric acid are titrated with 13.2ml of a 0.1M sodium hydroxide solution to the equivalence point . Calculate the concentration of the acid! L 7.4 F28 A1 F29 A1 F30 7.5 So that everything stays as it is Buffer The definition of the term buffer from the Duden is: "Spring device on the front and back of a rail vehicle to absorb bumps" Adding base changes the pH value dramatically: For example: 1 l water (pH = 7) + 10 ml hydrochloric acid (c = 0.1 mol / l) with c = n __ V ® n = 0.001 mol HCl addition per Liters of water ® c H3O + = 0.001mol / l ® pH = 3 A buffer is a solution that keeps the pH value largely constant when small amounts of acid or base are added! So it cushions strong pH changes. This is e.g. B. vital in our blood. Info: Buffer System of the Blood An acid must be present in a buffer in order to neutralize OH - ions that are released when a base is added. In addition, a base is required to absorb H + ions that are released by added acids. However, the acids and bases must not neutralize one another. Therefore, one uses mixtures of weak acids and their conjugate bases (i.e. salts) such as. B. acetic acid and sodium acetate. Q31 Summary Buffers consist of mixtures of weak acids and their conjugate bases. They keep the pH value of a solution constant within a certain range despite the addition of acids or bases. What does a chemist understand by the term “buffer”? How does our body keep the pH of the blood constant? F31 F32 Fig. 7.20: Z For testing purposes only - property of the publisher öbv

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