Answer:
vol 0.05M H₂SO₄ = 0.200 ml
Explanation:
H₂SO₄ + 2NaOH => NaCl + 2 H₂O
moles = Molarity X Volume
From balanced equation 1 mole H₂SO₄ neutralizes 2 moles NaOH.
Using neutralization equation
Moles NaOH neutralized = 2 x Moles H₂SO₄ used
∴ 1(Molarity x Volume Base) = 2(Molarity x Volume Acid)
=> Volume of Acid needed = Molarity x Volume of Base / 2 x Molarity of Acid
=> Volume of Acid needed = (0.001M x 20 ml) / (2 x 0.05M) = 0.20 ml Acid
Answer:
we need 0.2 mL of a 0.0500M H2SO4 solution
Explanation:
Step 1: Data given
Molarity of H2SO4 = 0.0500 M
Volume of NaOH = 20.0 mL = 0.020 L
Molarity of NaOH = 1.00 * 10^-3 M
Step 2: The balanced equation
2NaOH + H2SO4 → Na2SO4 + 2H2O
Step 3: Calculate the volume of H2SO4
b*Ca*Va = a*Cb*Vb
⇒with b = the coefficient of H2SO4 = 1
⇒with Ca = the concentration of NaOH = 1.00 * 10^-3 M
⇒with Va = the volume of NaOH = 0.020 L
⇒with a = the coefficent of NaOH = 2
⇒with Cb = the concentration of H2SO4 = 0.0500 M
⇒with Vb = the volume of H2SO4 = TO BE DETERMINED
1*10^-3 * 0.020 = 2*0.0500 * Vb
Vb = 0.0002 L = 0.2 mL
we need 0.2 mL of a 0.0500M H2SO4 solution
