Question

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.

Answer 1

To determine the amount of 0.45M HCl needed to neutralize 25.0 mL of 1.00M KOH, calculate the moles of KOH and use the 1:1 molar ratio from the balanced chemical equation. 0.025 mol of KOH requires 0.025 mol of HCl, which corresponds to 55.6 mL of 0.45M HCl solution.

Step-by-step explanation:

To determine how many milliliters of 0.45M HCl will neutralize 25.0 mL of 1.00M KOH, we first calculate the moles of KOH. The formula to convert from liters of KOH to moles is:

moles of KOH = L KOH × M KOH.

For 25.0 mL (0.025 L) of 1.00 M KOH:

moles of KOH = 0.025 L × 1.00 M = 0.025 mol KOH.

The balanced chemical reaction between HCl and KOH is:

HCl + KOH → KCl + H2O

This reaction shows a 1:1 molar ratio between HCl and KOH. Therefore, 0.025 mol of HCl will be needed to neutralize 0.025 mol of KOH.

To find the volume of 0.45M HCl:

Volume of HCl = moles of HCl ÷ molarity of HCl = 0.025 mol ÷ 0.45 M = 0.0556 L

Converting liters to milliliters:

Volume of HCl = 0.0556 L × 1000 mL/L = 55.6 mL

Therefore, 55.6 mL of 0.45M HCl is required to neutralize 25.0 mL of 1.00M KOH.

Answer 2

56mL

Step-by-step 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.