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 ac

Question

olga2289 [7]

2 years ago

9

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 ac

id?

Chemistry

2 answers:

inna [77] · Answer 1 · 2023-10-03T10:33:53+03:00

An acidic solution is 0.1M in HCl and 0.2 H2so4. volume is equal to no of moles divided by molarity.
number of moles of HCl is 450ml x 0.1 divided by 1000 which is equal to 0.045 moles
volume of HCl is therefore 0.45 divided by 0.16 which is 2.81 litres

Number of moles of H2so4 is 450ml x 0.2 divided by 1000 which is equal to 0.09 moles
volume of H2SO4 IS 0.09 divided by 0.16 which is equal to 0.56 litres

satela [25.4K] · Answer 2 · 2023-10-03T12:47:18+03:00

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

<h3>Further explanation </h3>

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)