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If 500 mL of a 5 M solution is diluted to 1500 mL, what will be the molarity of the solution obtained?
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If the concentration of glucose \[\ce{(C6H12O6)}\] in blood is 0.9 g L–1, what will be the molarity of glucose in blood?
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What will be the molality of the solution containing 18.25 g of \[\ce{HCl}\] gas in 500 g of water?
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Sulphuric acid reacts with sodium hydroxide as follows:
\[\ce{H2SO4 + 2NaOH -> Na2SO4 + 2H2O}\]
When 1 L of 0.1 M sulphuric acid solution is allowed to react with 1 L of 0.1 M sodium hydroxide solution, the amount of sodium sulphate formed and its molarity in the solution obtained is:
(i) 0.1 mol L–1
(ii) 7.10 g
(iii) 0.025 mol L–1
(iv) 3.55 g
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Which of the following solutions have the same concentration?
(i) \[\ce{20 g of NaOH in 200 mL of solution}\]
(ii) \[\ce{0.5 mol of KCl in 200 mL of solution}\]
(iii) \[\ce{40 g of NaOH in 100 mL of solution}\]
(iv) \[\ce{20 g of KOH in 200 mL of solution}\]
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Which of the following terms are unitless?
(i) Molality
(ii) Molarity
(iii) Mole fraction
(iv) Mass percent
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What is the difference between molality and molarity?
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If 4 g of \[\ce{NaOH}\] dissolves in 36 g of \[\ce{H2O}\], calculate the mole fraction of each component in the solution. Also, determine the molarity of solution (specific gravity of solution is 1g mL–1).
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Match the following physical quantities with units
| Physical quantity | Unit |
| (i) Molarity | (a) g mL–1 |
| (ii) Mole fraction | (b) mol |
| (iii) Mole | (c) Pascal |
| (iv) Molality | (d) Unitless |
| (v) Pressure | (e) mol L–1 |
| (vi) Luminous intensity | (f) Candela |
| (vii) Density | (g) mol kg–1 |
| (viii) Mass | (h) Nm–1 |
| (i) kg |
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\[\ce{BF3}\] does not have proton but still acts as an acid and reacts with \[\ce{NH3}\]. Why is it so? What type of bond is formed between the two?
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A reaction between ammonia and boron trifluoride is given below: \[\ce{NH3 + BF3 -> H3N : BF3}\] Identify the acid and base in this reaction. Which theory explains it? What is the hybridisation of B and N in the reactants?
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Match the following species with the corresponding conjugate acid:
| Species | Conjugate acid |
| (i) \[\ce{NH3}\] | (a) \[\ce{CO^{2-}3}\] |
| (ii) \[\ce{HCO^{-}3}\] | (b) \[\ce{NH^{+}4}\] |
| iii) \[\ce{H2O}\] | (c) \[\ce{H3O+}\] |
| (iv) \[\ce{HSO^{-}4}\] | (d) \[\ce{H2SO4}\] |
| (e) \[\ce{H2CO3}\] |
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Match the type of mixture of compounds in Column I with the technique of separation/purification given in Column II.
| Column I | Column II |
| (i) Two solids which have different solubilities in a solvent and which do not undergo reaction when dissolved in it. | (a) Steam distillation |
| (ii) Liquid that decomposes at its boiling point | (b) Fractional distillation |
| (iii) Steam volatile liquid | (c) Simple distillation |
| (iv) Two liquids which have boiling points close to each other | (d) Distillation under reduced pressure |
| (v) Two liquids with large difference in boiling points. | (e) Crystallisation |
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Assertion (A): Simple distillation can help in separating a mixture of propan-1-ol (boiling point 97°C) and propanone (boiling point 56°C).
Reason (R): Liquids with a difference of more than 20°C in their boiling points can be separated by simple distillation.
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Two liquids (A) and (B) can be separated by the method of fractional distillation. The boiling point of liquid (A) is less than boiling point of liquid (B). Which of the liquids do you expect to come out first in the distillate? Explain.
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Draw a diagram of bubble plate type fractionating column. When do we require such type of a column for separating two liquids. Explain the principle involved in the separation of components of a mixture of liquids by using fractionating column. What industrial applications does this process have?
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Arrange the following carbanions in order of their decreasing stability.
(A) H3C – C ≡ C–
(B) H – C ≡ C–
(C) \[\ce{H3C - C\overset{-}{H2}}\]
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Which of the following are correct?
(i) \[\ce{CH3 - O - CH^{⊕}2}\] is more stable than \[\ce{CH3 - CH^{⊕}2}\]
(ii) (CH3)2CH⊕ is less stable than \[\ce{CH3 - CH2 - CH^{⊕}2}\]
(iii) \[\ce{CH3 = CH2 - CH^{⊕}2}\] is more stable than \[\ce{CH3 - CH2 - CH^{⊕}2}\]
(iv) \[\ce{CH2 - CH^{⊕}}\] is more stable than \[\ce{CH3 - CH^{⊕}2}\]
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How will you convert benzene into p – nitrobromobenzene
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How will you convert benzene into m – nitrobromobenzene
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