25.0 mL of nitrous acid (HNO2) is titrated with a 1.235 M solution of KOH. The equivalence point (stoichiometric point) is observed after 9.

Question

25.0 mL of nitrous acid (HNO2) is titrated with a 1.235 M solution of KOH. The equivalence point (stoichiometric point) is observed after 9.26 mL of base is added. What is the original concentration of the acid

in progress 0
Phúc Điền 1 week 2021-07-22T06:12:49+00:00 1 Answers 0 views 0

Answers ( )

    0
    2021-07-22T06:14:19+00:00

    Answer:

    0.456 M

    Explanation:

    Step 1: Write the balanced neutralization equation

    HNO₂ + KOH ⇒ KNO₂ + H₂O

    Step 2: Calculate the reacting moles of KOH

    9.26 mL of 1.235 M KOH react.

    0.00926 L × 1.235 mol/L = 0.0114 mol

    Step 3: Calculate the reacting moles of HNO₂

    The molar ratio of HNO₂ to KOH is 1:1. The reacting moles of HNO₂ are 1/1 × 0.0114 mol = 0.0114 mol.

    Step 4: Calculate the initial concentration of HNO₂

    0.0114 moles of HNO₂ are in 25.0 mL of solution.

    [HNO₂] = 0.0114 mol / 0.0250 L = 0.456 M

Leave an answer

Browse

Giải phương trình 1 ẩn: x + 2 - 2(x + 1) = -x . Hỏi x = ? ( )