Chemistry

Problem

A chemist prepares five separate

100.0\,\text{mL}

samples of aqueous solutions at

25\,^{\circ}\text{C}

. The solutes and their initial molarities are given in the table.

Sample	Solute (strong)	$C_0$ (M)
1	$\text{HCl}$	$1.0\times10^{-3}$
2	$\text{HBr}$	$1.0\times10^{-7}$
3	$\text{NaOH}$	$1.0\times10^{-3}$
4	$\text{Ca(OH)}_2$	$5.0\times10^{-4}$
5	Pure water	—

All strong electrolytes dissociate completely. (a) Calculate the pH of each sample, using appropriate significant figures. (b) Identify any sample that can be considered neutral to within

\pm0.05

pH units, and justify your choice. (c) Rank the remaining samples from strongest acid to strongest base, showing how the numerical pH values support your ordering.

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