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1. How many milliliters of 0.45M HCl will neutralize 25.0 mL of 1.00M KOH?

Use the molarity to convert the volume of the base to moles of the base. Give your answer to three significant figures.

moles of KOH =
L KOH x [ANSWER 2] M KOH.

Simplify. There are [ANSWER 3] mol KOH



Balance the chemical reaction to find the mole ratio. (Write a coefficient of 1 before compounds which do not need any coefficient.)

Type your answer here.
” HCl + “blank space 5
Type your answer here.
” KOH →“blank space 6
Type your answer here.
” KCl +“blank space 7
Type your answer here.
” H2O

Use the moles of the base and the mole ratio to find the moles of the acid needed to neutralize the base. (Remember to include the units.)



The moles of HCl will be “blank space 8
Type your answer here.
”.



Divide the moles of HCl by the molarity of HCl to calculate the volume of HCl. Give your answer to the correct number of significant figures.



The volume of HCl =“blank space 9
Type your answer here.
” L.



Now write the volume with the correct unit, mL: “blank space 10
Type your answer here.

1 How many milliliters of 045M HCl will neutralize 250 mL of 100M KOH Use the molarity to convert the volume of the base to moles of the base Give your answer t class=
1 How many milliliters of 045M HCl will neutralize 250 mL of 100M KOH Use the molarity to convert the volume of the base to moles of the base Give your answer t class=

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Eduard22sly

Answer:

56mL

Explanation:

We'll begin calculating the number of mole of KOH in the solution. This is illustrated below:

Molarity of KOH = 1 M

Volume of KOH = 25mL = 25/1000 = 0.025L

Mole of KOH =?

Molarity = mole /Volume

Mole = Volume x Molarity

Mole of KOH = 0.025L x 1 M = 0.025 mole.

Therefore, there are 0.025 mole of KOH in the solution.

Next, the balanced equation for the reaction. This is illustrated below:

HCl + KOH —> KCl + H2O

The coefficients are: 1, 1, 1, 1

Next, we shall determine the number of mole of HCl required to react with 0.025 mole of KOH. This is illustrated below:

From the balanced equation above,

1 mole of HCl required 1 mole of KOH.

Therefore, 0.025 mole of HCl will also require 0.025 mole of KOH.

Therefore, the number of mole of HCl in the solution is 0.025 mole.

Next, we shall determine the volume of HCl needed for the reaction. This is illustrated below:

Mole of HCl = 0.025 mole

Molarity of HCl = 0.45 M

Volume of HCl =...?

Volume = mole /Molarity

Volume of HCl = 0.025/0.45

Volume of HCl = 0.056L

Finally, we shall convert 0.056L to mL. This is illustrated below:

1L = 1000mL

Therefore, 0.056L = 0.056 x 1000 = 56mL.

Therefore, the volume of HCl in mL needed for the reaction 56mL.