a)In a titration, a sample of H 2 SO 4 solution having a volume of 10.69 mL requ

Question

a)In a titration, a sample of H2SO4 solution having a volume of 10.69 mL required 39.25 mL of 0.195 M NaOH solution for complete neutralization.
What is the molarity of the H2SO4 solution?

b)"Stomach acid" is hydrochloric acid. A sample of gastric juice having a volume of 3.74 mL required 12.31 mL of 0.0160 M KOH solution for neutralization in a titration. What was the molar concentration of HCl in this fluid? If we assume a density of 1.00 g mL-1 for the fluid, what was the percentage by weight of HCl?

c)

Explanation / Answer

a)

H2SO4 +2 NaOH -------------> Na2SO4 + 2 H2O

M1 V1 / n1 = M2 V2 / n2

M1 x 10.69 / 1 = 0.195 x 39.25 / 2

M1 = 0.358 M

Molarity of H2SO4 = 0.358 M

b)

HCl + KOH ---------------> KCl + H2O

C1 V1 = C2 V2

C1 x 3.74 = 0.0160 x 12.31

C1 = 0.0527

molar concentration of HCl = 0.0527 M

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