Answer Happy

Redo #1: You have an unknown base with a mass of 0.3 g. This is titrated against 0.125MHCl to the equivalence point and the volume titrated is 12 mL. a) From the molarity of the HCL and its volume (in L), how many moles of acid titrated the base? b) Using the fundamental equality of titrated acid and base, how may moles of base were titrated? c) From the moles of base, the grams of base, and the definition of equivalent mass, what is the apparent equivalent mass of the base?
Acidic or Basic Salts The underlying fact determining whether a salt makes acldic or basic solutions in water is whether the cation from the dissolved salt reacts with water, the anion of the salt reacts with water, or the cation has a charge of +3 or greater. Acidic cations are weak acids: For NaCl vs., NH4​Cl complete the following equations for aqueous solutions NaCl(s)H2​O​NH4​ClH2​O​​ You should have Cl−,Na+, and NH4+​ions on the right-hand side. a) Which of the cations is a weak acid? Write down its reaction with water b) How strong is the conjugate base formed from this reaction? c) Given your answer from (b) and the reaction in (a), will hydroxide ions be formed? d) Given your answer, with this make the solution basic, acidic, or stay neutral? Basic anions are weak bases a) Write down the anions formed by dissolving NaCl,NaF, and NaC2​H3​O2​ in water b) Which, if any, of these is the conjugate base of a weak acid?
c) For the ones which are weak bases, write down the equation for its reaction with water d) Will any of these reactions favor products? If so, what will the pH of the solution be acidic neutral?