(08.05 MC) What is the hydronium ion concentration of a solution with a pOH of 6.90? (5 points) 6.53 x 10−7 M 6.29 x 10−7 M 7.94 x 10−8 M 7.18 x 10−8 M

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st drop outExplanation:

Step 1: convert the pOH to ph... 6.90 pOH is 7.1 ph.

Step 2: find out what we know, we know that the pH is 7.1

Step 3: What we need:

[ H3O+ ] = ?

[ OH− ] = ?

Step 4: Solve for hydronium ions:

[ H3O+ ] = 10−pH

[ H3O+ ] = 10^−7.1

[ H3O+ ] = 7.94328235 M

Step 5: Solve for hydroxide ions:

Using the ionization constant of water, we can use the concentration of hydronium ions to determine the concentration of hydroxide ions in the solution.

[ H3O+ ] = 10^−7.1

[ H3O+ ] = 7.94328235e-8 × 10^−13 M

[ OH− ] =

1.0 × 10−14 M/7.94 × 10−13 M

[ OH− ] = 1.25944584 × 10^-2 M

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