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Questions 36 and 37 refer to the following: During a laboratory activity, a student places 25.0 ml of HCIOaq) of unknown concentration into a flask. The student adds four drops of phenolphthalein to the solution in the flask. The solution is titrated with 0.150 M KOH(aq) until the solution appears faint pink. The volume of KOH(aq) added is 18.5 mL. 36) Complete the equation below for the neutralization reaction that occurs during the given titration. KOH (aq) HCl(aq)- 37o Determine the concentration of the HCI(aq) solution, using the given titration data.

Questions 36 and 37 refer to the following During a laboratory activity a student places 250 ml of HCIOaq of unknown concentration into a flask The student adds class=

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36)  HCl(aq)+KOH(aq)⇒H₂O(l)+KCl(aq)

37)  You can use the equation M₁V₁=M₂V₂
M₁=concentration of acid
V₁=volume of acid in orginal solution
M₂=concentration of base
V₂= the volume of based used to neutralize the acid
M₁=(0.150M KOH x 0.0185L KOH)/0.025L HCl
M₁=0.111M HCl
This equation works since we no based off of the formula in question 36 that 1 mole of KOH will neutralize 1 mole of HCl and M₂V₂ is equal to the moles KOH which means it needs to equal M₁V₁ since that is the number of moles HCl. (if moles HCl did not equal moles KOH the solution would not be neutralized).

(36) The complete equation for the neutralization reaction that occur during the given titration is KOH + HCl → KCl + H₂O. (37) The concentration of the HCl solution is 0.111 M.

What is Neutralization Reaction ?

The reaction in which the acid and a base react with each other that results in an ionic compound and possibly water is known as Neutralization reaction.

Acid + Base → Salt + H₂O

The complete reaction will be

KOH + HCl → KCl + H₂O

How to find the concentration of solution ?

To calculate the concentration of diluted solution it is expressed as

M₁V₁ = M₂V₂

where

M₁ = initial molarity

V₁ = initial volume

M₂ = final molarity

V₂ = final volume

Here we have to find the initial molarity of the solution. Initial volume is given 25.0 ml. Final molarity is given 0.150 M. Final volume is given 18.5 ml.

Now put the values in above equation we get:

M₁V₁ = M₂V₂

M₁ × 25.0 ml = 0.150 M × 18.5 ml

[tex]M_{1} = \frac{0.15 M \times 18.5 mL}{25.0 mL}[/tex]

[tex]M_{1} = \frac{2.775}{25}[/tex]

M₁ = 0.111 M

Thus from the above conclusion we can say that (36) The complete equation for the neutralization reaction that occur during the given titration is KOH + HCl → KCl + H₂O. (37) The concentration of the HCl solution is 0.111 M.

Lean more about the Neutralization reaction here: https://brainly.com/question/203541
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