Chem 105, Please help! super confused and lost on these!

Question

1. Calculate the volume of 0.550-M NaOH solution needed to completely neutralize 98.3 mL of a 0.630-M solution of the monoprotic acid HNO₃.
2. 80.96 mL of a solution of the acid H₂C₂O₄ is titrated, and 64.30 mL of 0.8600-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution.
3. A 50.00-mL sample of aqueous Ca(OH)₂ requires 34.66 mL of 0.859 M nitric acid for neutralization. Calculate the concentration (molarity) of the original solution of calcium hydroxide.
4. What volume (mL) of 0.250 M HNO₃ is required to titrate (neutralize) a solution containing 0.266 g of KOH?

Answer 1

Chem 105, Please help! super confused and lost on these!

What volume (mL) of 0.250 M HNO3 is required to titrate (neutralize) a solution containing 0.266 g of KOH?

Hello Makayla,

Just use: n₁M₁V₁ = n₂M₂V₂

where:

n = the number of moles of H⁺ or OH^- found on the reacting pair in the neutralization reactiion:

M = Molarity in Mol/L

V = Volume in Liters

Calculate the volume of 0.550-M NaOH solution needed to completely neutralize 98.3 mL of a 0.630-M solution of the monoprotic acid HNO₃.

n₁M₁V₁ = n₂M₂V₂

1 * 0.55mol/L NaOH *V₁ = 1 * 0.630mol/L HNO₃ * 0.0983L

Solve for V₁:

V₁ = 0.113 L

80.96 mL of a solution of the acid H₂C₂O₄ is titrated, and 64.30 mL of 0.8600-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution.

n₁M₁V₁ = n₂M₂V₂

1 * M₁ H₂C₂O₄  * 0.08096L = 2 * 0.8600mol/L NaOH * 0.06430L

Solve for M₁:

M₁ H₂C₂O₄ = 1.37 mol/L

A 50.00-mL sample of aqueous Ca(OH)2 requires 34.66 mL of 0.859 M nitric acid (HNO₃) for neutralization. Calculate the concentration (molarity) of the original solution of calcium hydroxide.

n₁M₁V₁ = n₂M₂V₂

1 * M₁ Ca(OH)₂ * 0.050L = 2 * 0.859mol/L HNO₃ * 0.03466L

Solve for M₁:

M₁ Ca(OH)₂ = 1.19 mol/L

You try the last one...