What volume of a 0.160 m solution of koh must be added to 450.0 ml of the acidic solution to completely neutralize all of the acid?

Volume KOH to completely neutralize all of the acid = 1406.25 ml

Titration is a procedure for determining the concentration of a solution by reacting with another solution which is known to be concentrated (usually a standard solution). Determination of the endpoint / equivalence point of the reaction can use indicators according to the appropriate pH range

Titrations can be distinguished including acid-base titration, depositional titration, and redox titration. An acid-base titration is the principle of neutralization of acids and bases is used.

An acid-base titration there will be a change in the pH of the solution.

From this pH change a Titration Curve can be made which is a function of acid / base volume and pH of the solution

Acid-base titration formula

Ma, Mb = acid base concentration

Va, Vb = acid base volume

na, nb = acid base valence

Since the concentration of the acid solution is unknown, we suppose that the solution is:

0.10M in HCl and 0.20 M in H2SO4

1. HCl

Ma Va. na = Mb. Vb. nb

a = HCl, b = KOH

na = valence HCl = 1 (yields 1 H + ion in solution)

nb = valence KOH = 1 (yields 1 OH- ion in solution)

0.10. 450 1 = 0.16. Vb. 1

Vb = 281.25 ml

2. H2SO4

Ma Va. na = Mb. Vb. nb

a = H2SO4, b = KOH

na = valence H2SO4 = 2 (yields 2 H + ions in solution)

nb = valence KOH = 1 (yields 1 OH- ion in solution)

0.20 450 2 = 0.16. Vb. 1

Vb = 1125 ml

Vb tot = 281.25 + 1125 = 1406.25 ml

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