A25.00 ml sample of an aqueous solution of ba(oh)2 requires 18.45 ml of 0.01500 m hcl (aq) for its neutralization. what is the molarity of the ba(oh)2 solution?

5.54 x 10⁻³ M

Further explanation

Given:

Neutralization reaction between:

25.00 ml of Ba(OH)₂18.45 ml of 0.015 M HCl

Question:

What is the molarity of the Ba(OH)₂ solution?

The Process:

Let us say the molarity of the Ba (OH)₂ solution as x M.

Step-1: prepare moles for each reagent

Step-2: neutralization

We use the ICE table to see how neutralization occurs between acid and base.

Balanced reaction:

                   

Initial:               25x                0.277              -                    -

Change:    - ¹/₂ · (0.277)        -0.277      +¹/₂ · (0.277)     +0.277

Equlibrium:        -                       -           +¹/₂ · (0.277)    +0.277

Neutralization causes no excess of hydrogen or hydroxide ions in solution. In the end, the number of acid and base reactions is balanced. In other words, the two reagents have run out with nothing left.HCl acts as a limiting reagent.

Step-3: calculate the molarity of the Ba(OH)₂ solution.

We consider Ba (OH) from the initial, change, and equilibrium stages.

Thus, the molarity of the Ba(OH)₂ solution is 5.54 x 10⁻³ M.

_ _ _ _ _ _ _ _ _ _

Alternative Steps

Valence of base = the number of OH⁻ ionsValence of acid = the number of H⁺ ions

Neutralization:

Thus the same results were obtained. The molarity of Ba (OH) ₂ solution is 5.54 x 10⁻³ M.

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The answer would be true