# If Ti(NO3)4 is dissolved in water, what would be the change of pH?

Does this compound exist in nature. I would suppose the salt would dissolve in it's ions (Nitrate and $\ce{Ti+}$). Wouldn't the nitrate react with the hydrogen in the water and give us a acid? And therefore a pH drop?

$\ce{Ti(NO3)4 + H2O -> Ti^{4+} + 4NO3-}$
$\ce{4NO3- + H2O -> HNO3}$

$\ce{HNO3 + H2O -> NO3- + H3O+}$

Or a metal complex as $\ce{Ti(OH)4}$?

$\ce{Ti(NO3)4 + H2O -> Ti(OH)4 + NO3-}$ and hence a basic solution?

I also came up with something along these lines

$\ce{Ti(NO3)4 + H2O -> Ti^{4+} + NO3- + H2O}$

$\ce{Ti^{4+} + NO3- + 2H2O -> TiO2 + 4H+ + NO3-}$

$\ce{TiO2 + 4H+ + 4NO3- + 4H2O -> TiO2 + 4H3O+}$

• Sorry but I don't understand how the equations are balanced as $\ce{H20}$ doesn't make sense for me. – Hexacoordinate-C Jun 28 '18 at 18:54
• Hi Hexa, the questions are not balanced. I just wanted to show how I thought about the problem. I can also see now that I wrote a mistake. "h30+" should be "H3O+" – gidl Jun 28 '18 at 18:58
• I also came up with something along these lines: Ti(NO3)4 + H2O > Ti4+ + NO3- + H2O Ti4+ + NO3- + 2H2O > TiO2 + 4H+ + NO3- TiO2 + 4H+ NO3- + 4 H2O > TiO2 + 4H3O+ (see org. comment) – gidl Jun 28 '18 at 19:03
• Well, all salts of $\ce{Ti^4+}$ will be hydrolyzed to a great extent and hence very acidic, that's for sure. – Ivan Neretin Jun 28 '18 at 20:16
• @MaxW It was also for OP. BTW hydrated forms of Ti(NO3)4 are rather ill-defined. One could just put (H2O)x into formula and call it a day. – Mithoron Jun 28 '18 at 22:53