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1.520 g of hydroxide of a metal on ignition gave 0.995 g of oxide. The equivalent weight of metal is
Options
(a) 1.52
(b) 0.995
(c) 190
(d) 9
Correct Answer:
9
Explanation:
One equivalent of the metal reacts with one mole of hydroxide, i.e., 17g
Similarly, one equivalent of the metal reacts with 1/2 mole oxygen atoms, i.e., 8g of oxygen atoms.
Let E be the equivalent mass of the metal. And let x be the number of equivalents of metal hydroxide ignited.
Therefore,
x(E+17) = 1.520g and
x(E+8) = 0.995
Eliminating x, we get E=9.06g.
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Difficulty Level: Easy
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Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
- Equal volumes of methanoic acid and sodium hydroxide are mixed, if x is the heat
- K₃[Al (C₂O₄)₃] is called
- Hexoses and pentoses are
- 5 mL of N HCl, 20 mL of N/2 H₂SO₄ and 30 mL of N/3 HNO₃ are mixed together
- For the reaction C₂H₅OH + 3O₂(g) → 2CO₂(g) + 3H₂O which one is true
Question Type: Memory (964)
Difficulty Level: Easy (1008)
Topics: Basic Concepts of Chemistry (94)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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