35.0 mL of a 0.250 M solution of KOH is titrated with 0.150 M HCl. After 35.0 mL of the HCl has been added, the resultant solution is:
A) Acidic and after the equivalence point
B) Basic and after the equivalence point
C) Neutral and at the equivalence point
D) Basic and before the equivalence point
E) Acidic and before the equivalence point
So, it should be letter D, basic and before the equivalence point??
millimols HCl = M x L = 0.150 x 35 = 5.25
millimols KOH = M x L = 0.250 x 35 = 8.75
........HCl + KOH ==> KCl + H2O
.......5.25.....8.75
It should be obvious that all of the KOH has not been neutralized by the HCl so the solution will be basic. It will take another 8.75-5.25 = ? mols HCl to finish the neutralization
Well, I gotta say, this titration sounds like a chemistry circus act! Here's the deal: KOH is a strong base, while HCl is a strong acid. When they react, they undergo a neutralization reaction. So, let's break it down.
Initially, you have 35.0 mL of the 0.250 M KOH solution. When you add the 0.150 M HCl solution, they'll start reacting, and the OH- ions from KOH will combine with the H+ ions from HCl to form water (H2O). This reaction will continue until either all the OH- or all the H+ ions are used up. This is known as the equivalence point.
Now, in this case, we have 35.0 mL of the HCl solution added. Since the HCl is of lower concentration than the KOH, it won't be enough to completely neutralize all the OH- ions. Therefore, we still have excess OH- ions left after the reaction.
Since we still have excess OH- ions in the solution, it means that we have a basic solution. So, the resultant solution is Basic and after the equivalence point.
So, the answer is B) Basic and after the equivalence point. Keep clowning around with chemistry!
To determine the resultant solution after 35.0 mL of 0.150 M HCl has been added to 35.0 mL of 0.250 M KOH, we can look at the reaction between the two:
KOH + HCl -> KCl + H2O
The balanced equation shows that the reaction produces potassium chloride (KCl) and water (H2O).
In a neutralization reaction, the moles of acid react with the moles of base at the equivalence point. The balanced equation tells us that the ratio of KOH to HCl is 1:1.
First, we can calculate the number of moles of HCl added:
Volume of HCl = 35.0 mL
Concentration of HCl = 0.150 M
Number of moles of HCl = (Volume of HCl) x (Concentration of HCl)
= (35.0 mL) x (0.150 mol/L) / (1000 mL/L)
= 0.00525 mol
Since KOH and HCl react in a 1:1 ratio, there are also 0.00525 mol of KOH.
Now, let's calculate the moles of KOH before any reaction occurs:
Volume of KOH = 35.0 mL
Concentration of KOH = 0.250 M
Number of moles of KOH = (Volume of KOH) x (Concentration of KOH)
= (35.0 mL) x (0.250 mol/L) / (1000 mL/L)
= 0.00875 mol
Comparing the number of moles of KOH before and after the reaction, we can conclude that:
- The number of moles of HCl added is less than the number of moles of KOH initially present.
- Therefore, there is KOH remaining in the solution.
Since KOH is a strong base and HCl is a strong acid, the remaining KOH makes the solution basic.
In conclusion, the resultant solution is Basic and after the equivalence point.
Therefore, the correct answer is B) Basic and after the equivalence point.
To determine the pH of the resultant solution after the titration, we need to analyze the reaction that occurs between KOH and HCl. The balanced chemical equation for this reaction is:
KOH + HCl -> KCl + H2O
This reaction is a neutralization reaction, where the acid (HCl) reacts with the base (KOH) to form water and a salt (KCl).
In this case, we have added 35.0 mL of the HCl solution to 35.0 mL of the KOH solution, which means the volumes are equal. Since both solutions have the same volume at the equivalence point, we can assume that the number of moles of KOH and HCl are equal.
To calculate the moles of KOH:
Moles of KOH = Volume of KOH solution (L) x Concentration of KOH (mol/L)
= 0.035 L x 0.250 mol/L
= 0.00875 mol
To calculate the moles of HCl:
Moles of HCl = Volume of HCl solution (L) x Concentration of HCl (mol/L)
= 0.035 L x 0.150 mol/L
= 0.00525 mol
Since the moles of KOH and HCl are not equal, it means that we have not reached the equivalence point. Therefore, the solution is not neutral.
To determine whether the solution is acidic or basic, we compare the number of moles of each reactant. In this case, the moles of KOH are higher than the moles of HCl, which means that there is an excess of base (KOH).
Therefore, the resultant solution is basic.
The correct answer is B) Basic and after the equivalence point.