Student Evaluation Sheet.docx

STUDENT EVALUATION SHEET 1. Note the information below! SO3 + O2- → SO42Which species acts as a Lewis acid? 2. Determine the conjugate base formula of NH4 +? 3. The advantages of Bronsted - Lowry acid base theory, which can explain. . . . 4. Know the reaction: HCl + H2O ==> H3O ++ ClAccording to Bronsted - Lowry Cl- and H3O + ions in these reactions respectively are as. . ..

Answer 1. According to Lewis: • Acid: a substance / compound that can accept electron pairs free from other substances / compounds. • Bases: substances / compounds that can donate free pairs of other substances / compounds.If the reaction above is described by the Lewis formula, then the SO3 compound will act as Lewis acid: 2. Because the requested conjugate base means NH4 + is an acid, then the conjugate base formula is: NH4 + → H + + NH3 (conjugate base) 3. Bronsted Acid - Lowry = binding H + (proton donor) Bonsted Base - Lowry = captures H + (proton acceptor) The specialty of the theory of bronsted lowry acid is that it can explain the nature of acid base in a reversible reaction, as happens in the ionization of CH3COOH weak acids. CH3COOH + H2O <==> H3O + + CH3COOThe above reaction is a reversible reaction where reactants can form products while the product can immediately form reactants. Right reaction CH3COOH + H2O ==> H3O + + CH3COOIn the above reaction, which binds H + to the other is CH3COOH so that it changes to CH3COO- (you can see that 1 CH3COOH atom is lost so it becomes CH3COO-). Then CH3COOH is acidic. Whereas H2O is a species that accepts H + released by acid, so it changes to H3O + (you can see that H H2O atoms increase by one so that it becomes H3O +.

CH3COOH + H2O ==> H3O + + CH3COOBase Acid Conjugated Base Conjugated Acid 1. base acid 1 acid 2 base 2 Leftist reaction H3O + + CH3COO- ==> CH3COOH + H2O In this second reaction, it can be seen that H3O + gives H + to CH3COO - so that it changes to H2O while CH3COO - which receives H + changes to CH3COOH. Then CH3COOH is still acidic and H2O remains the same base when the reaction is right. 4. Because H3O + and Cl- are located in the product, they are both acid and conjugate bases. to determine which acid and conjugate base we will use how to give: 1. Look for pairs of species, namely HCl paired with Cl- and H2O in pairs with H3O +. 2. determine which H + decreases and increases. HCl changes to Cl-, meaning H + from HCl has been donated so that HCl is acid and Cl- is the conjugate base. whereas H2O the number of H + has increased so that it forms H3O +, then H2O is alkaline and H3O + is the conjugate acid.