CHEM 1R03 Lecture Notes - Lecture 21: Litmus, Sodium Bicarbonate, Conjugate Acid
27 Apr 2018
School
Department
Course
Professor
lecture 21
properties of acids
-sour taste
-change the colours of various vegetables dyes
-react with active metals such as Al, Zn, Fe, but not Cu, Ag, or Au
-example reaction between Zn and HCl
-corrosive
-they react with carbonates to produce carbon dioxide
-for example marble, chalk, and baking soda (CaCO3 + 2HCl --> CaCl2 + CO2 + H2O)
-reactive with bases to form ionic salts and water
properties of bases
-also known as alkalis
-taste bitter and they feel slippery because they react with the oils on our skin
-change the colours of vegetables dyes, different colour than acids
-the litmus paper turns blue
-reactive with acids to form ionic salts and water
Arrhenius theory
-acids ionize in water to H+ ions and anions
-bases ionize in water to OH- ions and cations
-a neutralization reaction involve the combination of H+ and OH- to form water
-however some problems of this theory is that this theory only applies to aqueous
solutions
-the general definition of the theory also does not explain why liquid ammonia
solutions are basic
-ammonia turns litmus blue or in other words basic without OH- ions
Bronsted-Lowry theory
-an acid is a H+ donor while a base is a H+ acceptor
Document Summary
Change the colours of various vegetables dyes. React with active metals such as al, zn, fe, but not cu, ag, or au. They react with carbonates to produce carbon dioxide. For example marble, chalk, and baking soda (caco3 + 2hcl --> cacl2 + co2 + h2o) Reactive with bases to form ionic salts and water properties of bases. Taste bitter and they feel slippery because they react with the oils on our skin. Change the colours of vegetables dyes, different colour than acids. Reactive with acids to form ionic salts and water. Acids ionize in water to h+ ions and anions. Bases ionize in water to oh- ions and cations. A neutralization reaction involve the combination of h+ and oh- to form water. However some problems of this theory is that this theory only applies to aqueous solutions. The general definition of the theory also does not explain why liquid ammonia solutions are basic.
