The ph and poh values were calculated using the formula.
It is given that
[H⁺] of KOH solution = [tex]1.87*10^{-13}[/tex]
[tex]ph = -log[H^{+} ][/tex]
[tex]poh = -log[OH^{-} ][/tex]
So, ph of KOH solution = [tex]-log[1.87*10^{-13} ][/tex]
The ph of KOH solution = 12.72
Similarly, poh of a KOH solution that has [OH⁻] = 5.81 ×10–3m is 2.24.
The ph of NaCl solution that has [H⁺] = 1.00 × 10–7m is 7.
Thus, the ph and poh values were calculated using the formula.
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Answer:
What is the pH of a KOH solution that has [H+] = 1.87 × 10–13 M? Round to the nearest tenth.
12.7
What is the pOH of a KOH solution that has [OH–] = 5.81 ×10–3M? Round to the nearest hundredth.
2.24
What is the pH of a solution of NaCl that has [H+] = 1.00 × 10–7 M? Round to the nearest hundredth.
7.00
Step-by-step explanation:
