what is the ph of a koh solution that has h+=1.87×10−13 m? round to the nearest tenth. what is the poh of a…

what is the ph of a koh solution that has h+=1.87×10−13 m? round to the nearest tenth. what is the poh of a koh solution that has oh−=5.81×10−3m? round to the nearest hundredth. what is the ph of a solution of nacl that has h+=1.00×10−7 m? round to the nearest hundredth.

what is the ph of a koh solution that has h+=1.87×10−13 m? round to the nearest tenth. what is the poh of a koh solution that has oh−=5.81×10−3m? round to the nearest hundredth. what is the ph of a solution of nacl that has h+=1.00×10−7 m? round to the nearest hundredth.

Answer

Answer:

  1. For the pH of KOH solution with $[H^+]=1.87\times 10^{-13}\ M$: 12.7
  2. For the pOH of KOH solution with $[OH^-]=5.81\times 10^{-3}\ M$: 2.24
  3. For the pH of NaCl solution with $[H^+]=1.00\times 10^{-7}\ M$: 7.00

Explanation:

Step1: Recall pH formula

$pH = -\log[H^+]$ For the KOH solution with $[H^+]=1.87\times 10^{-13}\ M$, $pH=-\log(1.87\times 10^{-13})$. Using a calculator, $pH = 12.73$. Rounding to the nearest tenth gives 12.7.

Step2: Recall pOH formula

$pOH=-\log[OH^-]$ For the KOH solution with $[OH^-]=5.81\times 10^{-3}\ M$, $pOH = -\log(5.81\times 10^{-3})$. Using a calculator, $pOH=2.236$. Rounding to the nearest hundred - th gives 2.24.

Step3: Calculate pH of NaCl solution

For the NaCl solution with $[H^+]=1.00\times 10^{-7}\ M$, using the formula $pH = -\log[H^+]$, $pH=-\log(1.00\times 10^{-7}) = 7.00$.