The following 0.1 M aqueous solutions are arranged in order of increasing pH, with the highest pH on the far right. $\begin{array} { | l | l | l | l | l | } \hline \mathrm { HClO } _ { 4 } & & \left( \mathrm { CH } _ { 3 } \right) _ { 3 } \mathrm { NHCl } & \mathrm { KBr } & \mathrm { KNO } _ { 2 } \\\hline\end{array}$
Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

Question

The following 0.1 M aqueous solutions are arranged in order of increasing pH, with the highest pH on the far right.

\begin{array} { | l | l | l | l | l | } \hline \mathrm { HClO } _ { 4 } & & \left( \mathrm { CH } _ { 3 } \right) _ { 3 } \mathrm { NHCl } & \mathrm { KBr } & \mathrm { KNO } _ { 2 } \\\hline\end{array}

Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

Quizplus · Accepted Answer

The correct order is based on the nature of the substances: strong acid, weak acid, neutral, weak base, strong base. HCOOH (formic acid) is a weak acid and fits between the strong acid HClO4 and the neutral KBr.

The Following 0 Which One of the Following 0