Question

The first question is what I got as an answer and said it was wrong and that my first product has elements in there that aren't supposed to be in there. A

Complete the molecular reaction for the following weak base with a strong acid: NaClO2(aq) + H2SO4(aq) → NaClO2H+ (aq) + HS0.- (aq)

nd then the 2nd question I feel like I am making a calculation error somewhere.

Thanks in advance!

Answer 1

Q1. The balanced molecular reaction is :

2 NaClO₂(aq) + H₂SO₄(aq) $\rightarrow$ 2 HClO₂(aq) + Na₂SO₄(aq)

Q2. pH = 1.52

Explanation

Q2. Concentration HCl = 0.250 M

volume HCl = 60.0 mL

moles HCl = (Concentration HCl) * (volume HCl)

moles HCl = (0.250 M) * (60.0 mL)

moles HCl = 15.0 mmol

moles H⁺ = moles HCl = 15.0 mmol

moles Ca(OH)₂ = (concentration Ca(OH)₂) * (volume Ca(OH)₂)

moles Ca(OH)₂ = (0.150 M) * (40.0 mL)

moles Ca(OH)₂ = 6.00 mmol

moles OH^- = 2 * (moles Ca(OH)₂)

moles OH^- = 2 * (6.00 mmol)

moles OH^- = 12.0 mmol

excess moles H⁺ = (moles H⁺) - (moles OH^-)

excess moles H⁺ = (15.0 mmol) - (12.0 mmol)

excess moles H⁺ = 3.00 mmol

total volume = (volume HCl) + (volume Ca(OH)₂))

total volume = (60.0 mL) + (40.0 mL)

total volume = 100. mL

[H⁺] = (excess moles H⁺) / (total volume)

[H⁺] = (3.00 mmol) / (100. mL)

[H⁺] = 0.0300 M

pH = -log[H⁺]

pH = -log(0.0300 M)

pH = 1.52