because there were, A:Arrhenius acid/base concept :- Q:State whether 0.1 M solutions of each of the following salts are acidic, basic, or neutral. Acid = CH3COOH As we discussed earlier shows a standing wave on a string. https://en.wikipedia.org/wiki/Base_(chemistry), https://en.wikipedia.org/wiki/Salt_(chemistry), https://en.wikipedia.org/wiki/Neutralization_(chemistry). (b) What is the ionization constant, Ka, for the acid? b. EtH TLDR: Ball 111 HS. Chapter 16 Flashcards | Quizlet undergone, Q:Say whether the following salt solutions would be acidic, basic or neutral. To be honest, it is a tricky question, but to answer it in one line, I would say it is as acidic or basic as water. I suggest you write them even though you think neither anion nor cation is hydrolyzed. b.) The reaction is: We are given two of three equilibrium concentrations and asked to find the missing concentration. Which of the following are expected to act as a Lewis acid? The reaction, [latex]{\text{CaCO}}_{3}\left(s\right)+2\text{HCl}\left(aq\right)\rightleftharpoons {\text{aCl}}_{2}\left(aq\right)+{\text{H}}_{2}\text{O}\left(l\right)+{\text{CO}}_{2}\left(g\right)[/latex]. Making statements based on opinion; back them up with references or personal experience. The way to tell if salt is acidic or not is by using the pH scale. However, the acetate ion, the conjugate base of acetic acid, reacts with water and increases the concentration of hydroxide ion: [latex]{\text{CH}}_{3}{\text{CO}}_{2}{}^{\text{-}}\left(aq\right)+{\text{H}}_{2}\text{O}\left(l\right)\rightleftharpoons {\text{CH}}_{3}{\text{CO}}_{2}\text{H}\left(aq\right)+{\text{OH}}^{\text{-}}\left(aq\right)[/latex]. These reactions are best explained . Using a Lewis approach, the Na + ion can be viewed as an acid because it is an electron . This is known as a hydrolysis reaction. 2003-2023 Chegg Inc. All rights reserved. If Ka is stronger soln is acid. We have difine a increasing acidic order. However, the ammonium ion, the conjugate acid of ammonia, reacts with water and increases the hydronium ion concentration: [latex]{\text{NH}}_{4}{}^{\text{+}}\left(aq\right)+{\text{H}}_{2}\text{O}\left(l\right)\rightleftharpoons {\text{H}}_{3}{\text{O}}^{\text{+}}\left(aq\right)+{\text{NH}}_{3}\left(aq\right)[/latex], The equilibrium equation for this reaction is simply the ionization constant.
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