Question

each row of the table below describes an aqueous solution at about 25 °c.
complete the table. that is, fill in any missing entries in the second and third columns. be sure each entry you write incluc
digits.

Explanation:

Step1: Calculate pH for solution A

The formula for pH is \(pH = -\log[H_3O^+]\).
For solution A, \([H_3O^+]=2.0\times 10^{-10}\space mol/L\).
\(pH = -\log(2.0\times 10^{-10})=-( \log2+\log10^{-10})=-(0.30 - 10)=9.70\)

Step2: Calculate \([H_3O^+]\) for solution B

Using the formula \([H_3O^+]=10^{-pH}\).
For solution B, \(pH = 7.08\).
\([H_3O^+]=10^{-7.08}=10^{-7}\times10^{-0.08}\approx8.3\times 10^{-8}\space mol/L\)

Step3: Calculate pH for solution C

Using the formula \(pH = -\log[H_3O^+]\).
For solution C, \([H_3O^+]=7.0\times 10^{-6}\space mol/L\).
\(pH = -\log(7.0\times 10^{-6})=-( \log7+\log10^{-6})=-(0.85 - 6)=5.15\)

Answer:

solution	\([H_3O^+]\)	pH
B	\(8.3\times 10^{-8}\space mol/L\)	\(7.08\)
C	\(7.0\times 10^{-6}\space mol/L\)	\(5.15\)