What volume of a 0.22mol/L hydrochloric acid solution is needed to cause the pH of 25.00mL of a 0.15mol/L lithium hydroxide solution to have a pH that s equal to 7.00

HCl is a strong acid; LiOH is a strong base. When they are EXACTLY neutralized the pH will be 7.00

mols LiOH = M x L = ?
mols HCl = mols LiOH (from the coefficients in the balanced equation.)
M HCl = mols HCl/L HCl. You know M and mols, solve for L (and convert to mL if needed).

To determine the volume of hydrochloric acid (HCl) solution needed to achieve a pH of 7.00 in a lithium hydroxide (LiOH) solution, we can use the concept of neutralization.

Step 1: Write the balanced chemical equation for the reaction between HCl and LiOH:
HCl + LiOH → LiCl + H2O

Step 2: Calculate the moles of lithium hydroxide (LiOH) in the given solution:
Moles of LiOH = concentration (mol/L) × volume (L)
Moles of LiOH = 0.15 mol/L × 0.025 L
Moles of LiOH = 0.00375 mol

Step 3: From the balanced chemical equation, we see that 1 mole of HCl reacts with 1 mole of LiOH. Therefore, we need an equal number of moles of HCl to neutralize the LiOH.

Step 4: Calculate the volume of hydrochloric acid (HCl) solution required:
Moles of HCl = moles of LiOH = 0.00375 mol

To determine the volume, we can use the formula:
Volume (L) = moles/concentration (mol/L)
Volume (L) = 0.00375 mol / 0.22 mol/L
Volume (L) ≈ 0.017 L

To convert the volume to milliliters (mL), multiply by 1000:
Volume (mL) = 0.017 L × 1000
Volume (mL) ≈ 17 mL

Therefore, approximately 17.00 mL of a 0.22 mol/L hydrochloric acid (HCl) solution is needed to neutralize 25.00 mL of a 0.15 mol/L lithium hydroxide (LiOH) solution and achieve a pH of 7.00.

To solve this problem, we need to use the concept of molar stoichiometry and the formula for pH.

Step 1: Determine the balanced chemical equation for the reaction between hydrochloric acid (HCl) and lithium hydroxide (LiOH):

HCl + LiOH → LiCl + H2O

Step 2: Calculate the number of moles of lithium hydroxide (LiOH) in the given volume of solution:

moles of LiOH = concentration of LiOH × volume of LiOH solution
= 0.15 mol/L × 0.025 L
= 0.00375 mol

Step 3: Use the stoichiometry of the balanced equation to determine the moles of hydrochloric acid (HCl) needed to neutralize the given amount of lithium hydroxide:

The balanced equation tells us that the stoichiometric ratio of LiOH to HCl is 1:1. Therefore, the moles of HCl required will be equal to the moles of LiOH.

moles of HCl = 0.00375 mol

Step 4: Calculate the required volume of hydrochloric acid (HCl) solution using the given concentration:

volume of HCl = moles of HCl / concentration of HCl
= 0.00375 mol / 0.22 mol/L
= 0.017 L

Since the volume of HCl is given in liters, you can convert it to milliliters by multiplying by 1000:

volume of HCl = 0.017 L × 1000 mL/L = 17.15 mL

Therefore, approximately 17.15 mL of the 0.22 mol/L hydrochloric acid solution is needed to neutralize 25.00 mL of the 0.15 mol/L lithium hydroxide solution and achieve a pH of 7.00.