Fill in the table below for the type of aqueous system that would result if the

Question

Fill in the table below for the type of aqueous system that would result if the ionic compounds were dissolved in water. Identify each according to these designations. If a solution

Fill in the table below for the type of aqueous system that would result if the ionic compounds were dissolved in water. Identify each according to these designations. If a solution's pH will be affected by more than one component, give TWO identifications for the mixture. (Ka1 for Al(H2O)63+ = 7.9 x10-6, all other K's can be found online) SA = strong acid; SB = strong base; WA = weak acid; WB = weak base; AM = amphiprotic; NS = neutral salt

Explanation / Answer

1) Al(IO3)3 + H2O <------> Al(OH)3 + 3HIO3

while Al(OH)3 is not so basic HIO3 is strongly acidic and hence solution is very acidic

ionic species responsible is Al3+(aq)

2) Na2HAsO4 + H2O <---> 2NaOH + H3AsO4 , clealry NaOH is strong base while H3AsO4 is weaker acid and hence solution is very basic , species responsible is HAsO4-(aq)

3) CsI + 2H2O <---> Cs(OH)2 + 2HI   while Cs(OH)2 is strongly basic HI is strongly acidic , hence solution is neutral , species responsible are Cs+(aq) , I- (aq)

4) CH3COONa + H2O <-----> CH3COOH + NaOH , CH3COOH is weak acid while NaOH is strong base and hence solution is very basic , species responsible is CH3COO-(aq)

5) CH3NH3+ClO4- + H2O <->   HClO4 + CH3NH3OH , HClO4 is stronger acid while CH3NH3OH is weak base and hence solution is very acidic , ion responsible is CH3NH3+(aq)

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