State whether the reactant shown in bold in each of thefollowing chemical equati

Question

State whether the reactant shown in bold in each of thefollowing chemical equations is acting as an acid or base. a.)   CH3NH2 + H2O -->    CH3NH3 + OH b.)   C6H5OH + H2O -->   C6H5O + H3O c.)   NH3   + H2O   --> NH4 + OH d.)   CH3COOH  +   H2O  --> CHCOO + H3O State whether the reactant shown in bold in each of thefollowing chemical equations is acting as an acid or base. a.)   CH3NH2 + H2O -->    CH3NH3 + OH b.)   C6H5OH + H2O -->   C6H5O + H3O c.)   NH3   + H2O   --> NH4 + OH d.)   CH3COOH  +   H2O  --> CHCOO + H3O

Explanation / Answer

Generally from Lowry Bronsted concepts an acidis a compound that can donate a proton, and a base is acompound that can receive a proton. so here a.)   CH3NH2 + H2O -->    CH3NH3 + OH H2O donates proton to give OH so it is  acid b.)   C6H5OH + H2O -->   C6H5O + H3O H2O accepts a proton to give H3O so it is base c.)   NH3   + H2O   --> NH4 + OH here NH3 accepts a proton to give NH4 so it is base d.)   CH3COOH  +   H2O  --> CH3COO + H3O here CH3COOH donates a proton to give CH3COO so it isacid

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