What is the ph of an aqueous solution with the hydronium ion concentration [h3o+] = 2 x 10-14 m ? make sure that your answer has the correct number of signi?

The pH of an aqueous solution with the hydronium ion concentration [H₃O+] of 2 × 10^-14 M is 13.699.

Further Explanation: pH and pOH pH and pOH measures the acidity or alkalinity of a substance.pH is the measure hydrogen ion concentration in a substance while pOH measures the concentration of hydroxyl ions. Acids and bases Acids Acids are substances that react with bases to form salt and water as the only products.Acids have a pH less than 7, with strong acids having a pH range of 1-3 while weak acids have a pH range of 4-6.The pOH of acids on the other hand is greater than 7.BasesBases are substances that react with acids to form salt and water as the only product.Bases have a pH greater than 7, with strong bases having a pH range of 12-14 and weak bases having a pH range of 8-11.Bases have a pOH less than 7.Calculation of pH and pOH pH is calculated as the negative logarithm of hydrogen ion concentration.

That is;

pH = -Log [H+]

pOH on the other hand is calculated as the negative logarithm of hydroxyl ion concentration.

That is;

pOH =-Log[OH-] Additionally;pH + pOH = 14 In the Question:

We are given [H₃O+] = 2 × 10^-14 M

But; pH = -Log[H+] =-Log [H₃o+]

Therefore;

pH = - log[2 × 10^-14 M]

    = 13.699

Therefore; The pH of an aqueous solution with the hydronium ion concentration [H₃O+] of 2 × 10^-14 M is 13.699.

Keywords: Acids, bases, pH, pOH Learn more about:pH :linkpOH : linkExample of a question on pH: linkExample of a question on pOH: link

Level; High school

Subject: Chemistry

Topic: Acids and bases

Sub-topic; pH and pOH

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Naoh + hbr -> nabr (salt) + h2o ca (oh)2 + 2hbr - - - > ca (br)2 + 2h2o