# Titration Problems

Find the pH of the buffer solution consisting of 0.100 M HONH$_2$ and 0.100 M HONH$_3^+$ (K$_b$ of HONH$_2$ = 1.1 x 10$^{-8}$), after .02 moles HCl is added to the buffer solution? (assume the final volume of the solution is 1 L)

## Related Problems

Rank the following in terms of acidity: HClO, IOH, and HBrO. Explain the trend.

Rank the following in terms of acidity: HClO, HClO$_2$, HClO$_3$, HClO$_4$. Explain the trend.

10.00 mL of an unknown H$_2$CO$_3$ solution is titrated with 0.0500 M NaOH and it requires 15.67 mL to reach the end point. What is the concentration of the H$_2$CO$_3$ ?

H$_2$CO$_3$ + 2 NaOH $\longrightarrow$ Na$_2$CO$_3$ + 2 H$_2$O

Sketch the titration curve for 50.0 mL 0.1 M HCl, K$_a$ = 1.8 x 10$^{-5}$ with 0.1 M NaOH. Include points on your graph for the initial pH, the pH at half way to the equivalence point, the pH at the equivalence point and the pH after the equivalence point.