[填空题]
20.0$cm^3$ of 0.100 mol $dm^{-3}$ NaOH were slowly added to a 10.0 $cm^3$ sample of 0.100mol $dm^{-3}$ HCl, and the pH was measured throughout the addition.
The equation for the reaction is as follows:NaOH$_{(aq)}$+HCl$_{(aq)}$$\rightarrow$NaCl$_{(aq)}$+$H_2O(l)$
The ionic product constant of water at $25^{\circ}C$ is $1.00\times10^{-14}$.
1.Calculate the number of moles of NaOH remaining at the end of the addition. $\times10^{-3} mol$
2.Calculate the concentration of $OH^-$ at the end of the addition. $mol\:dm^{-3}$
3.Using your value for $[OH^-]$ in (b), calculate the pH of the solution at the end of the addition.
