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question_answer1) A crystal of common salt of given mass is kept in aqueous solution. After 12 hours, its mass remains the same. Is the crystal in equilibrium with the solution?
question_answer2) Why is there a fizz when a soda water bottle is opened?
question_answer3) Can equilibrium be achieved between water and its vapours in an open vessel? Explain your answer and say what happens eventually.
question_answer4) From the values of the equilibrium constants, indicate in which case, does the reaction go farthest to completion: \[{{K}_{1}}={{10}^{-10}},\,{{K}_{2}}={{10}^{10}},\,{{K}_{3}}={{10}^{5}}\].
question_answer5) The value of the equilibrium constant is less than zero. What does it indicate?
question_answer6) Would you expect equilibrium constant for the reaction \[{{I}_{2}}(g)\rightleftharpoons 2I(g)\] to increase or decrease as temperature increases. Assign reason.
question_answer7) Following equilibrium is set up when \[SC{{N}^{-}}\] ion is added to \[F{{e}^{3+}}\] in aqueous solution : \[\underset{Pale\,yellow}{\mathop{F{{e}^{3+}}}}\,+\underset{Colour\,less}{\mathop{SC{{N}^{-}}}}\,\rightleftharpoons \,\,\underset{Deep\,\,red}{\mathop{\,{{[Fe(SCN)]}^{2+}}}}\,\] When silver nitrate is added to the solution, \[AgSCN\] gets precipitate. What will happen to the equilibrium?
question_answer8) Following reaction occurs in a Blast Furnace: \[F{{e}_{2}}{{O}_{3}}(s)+3CO(g)\rightleftharpoons 2Fe(l)+3C{{O}_{2}}(g)\] Use Le Chatelier's principle to predict the direction of reaction when equilibrium mixture is disturbed by (a) adding \[F{{e}_{2}}{{O}_{3}}\] (b) removing \[C{{O}_{2}}\] (c) removing CO.
question_answer9) Acetic acid is highly soluble in water but still a weak electrolyte. Why?
question_answer10) Discuss the role of \[N{{H}_{4}}OH\] in group III of basic radicals.
question_answer11) How will you account for the following: (a) Clothes dry quicker on a windy day (b) We sweat more on a humid day?
question_answer12) The solubility of\[C{{O}_{2}}\] in water decreases with increase in temperature. Explain.
question_answer13) Will ionic product of water increase or decrease if temperature is increased?
question_answer14) In a chemical reaction under equilibrium, there is no change in moler concentration of products and reactants. Does the reaction stop?
question_answer15) Out of water and silver nitrate solution, in which case silver chloride will dissolve more?
question_answer16) Magnesium is not precipitated from a solution of its salt by \[N{{H}_{4}}OH\] in the presence of\[N{{H}_{4}}Cl\]. Explain.
question_answer17) \[S{{O}_{3}}\] is an acidic oxide while \[N{{a}_{2}}O\] is basic in nature. Support the same with the help of examples.
question_answer18) \[Zn{{(OH)}_{2}}\] is not precipitated when \[N{{H}_{4}}OH\] is added to a zinc salt solution containing some ammonium chloride. Explain.
question_answer19) Will \[pH\] of water be same or different at \[4{}^\circ C\]and \[25{}^\circ C\]? Explain.
question_answer20) Why gas fizzes out when soda water bottle is opened?
question_answer21) Reaction between acetic acid and ethyl alcohol attains a state of equilibrium in an open vessel but decomposition of \[CaC{{O}_{3}}\] does not. Why?
question_answer22) At equilibrium, the mass of each of the reactants and products remains constant. Does it mean that the reaction has stopped? Explain.
question_answer23) If concentrations are expressed in moles \[{{L}^{-1}}\] and pressures in atmospheres, what is the ratio of \[{{K}_{p}}\] to \[{{K}_{c}}\] for the reaction : \[2S{{O}_{2}}(g)+{{O}_{2}}(g)\rightleftharpoons 2S{{O}_{3}}(g)\]at \[25{}^\circ C\]?
question_answer24) The value of equilibrium constant depends on what?
question_answer25) The equilibrium constant for the reactions (i) \[{{N}_{2}}+{{O}_{2}}\rightleftharpoons \,2NO\] and (ii) \[2NO+{{O}_{2}}\rightleftharpoons 2N{{O}_{2}}\] are \[{{K}_{1}}\] and \[{{K}_{2}}\] respectively, then what will be the equilibrium constant for the reaction \[{{N}_{2}}+2{{O}_{2}}\rightleftharpoons 2N{{O}_{2}}?\]
question_answer26) For the reaction \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g),\]at \[400\,K,\,{{K}_{p}}=41\]. Find the value of \[{{K}_{p}}\] for each of the following reactions at the same temperature: (i) \[2N{{H}_{3}}(g)\,\rightleftharpoons {{N}_{2}}(g)+3{{H}_{2}}(g)\] (ii) \[\frac{1}{2}{{N}_{2}}(g)+\frac{3}{2}{{H}_{2}}(g)\rightleftharpoons N{{H}_{3}}(g)\] (iii)\[2{{N}_{2}}(g)+6{{H}_{2}}(g)\rightleftharpoons 4N{{H}_{3}}(g)\]
question_answer27) For an exothermic reaction, what happens to the equilibrium constant if temperature is increased?
question_answer28) The equilibrium constant of a reaction is \[2\times {{10}^{-3}}\] at 25°C and \[2\times {{10}^{-2}}\] at 50°C. Is the reaction exothermic or endothermic?
question_answer29) The equilibrium \[{{H}_{2}}O(l)\rightleftharpoons {{H}_{2}}O(\upsilon )\] is attained in a closed container at 40°C. The aqueous tension of water at 40° C is 23 mm. What is \[{{K}_{p}}\] for the said equilibrium?
question_answer30) The concentration quotient of a reversible reaction is Q, and the equilibrium constant is K. What do you conclude if (i) Q = K (ii) Q > K (iii) Q < K?
question_answer31) What does the equilibrium constant K < 1 indicate?
question_answer32) What qualitative information can you obtain from the magnitude of equilibrium constant?
question_answer33) In which one of the following reactions, the yield of the product will be maximum? \[2A+B\,\rightleftharpoons C,\,K={{10}^{-5}};\,\,C+2D\rightleftharpoons E,\,\,K={{10}^{5}};\,\,D+3B\rightleftharpoons F,\,K={{10}^{3}}\]
question_answer34) For the reaction: \[{{H}_{2}}+{{I}_{2}}\rightleftharpoons 2HI,\] if initially 25 mL of \[{{H}_{2}}\] and 20 mL of \[{{I}_{2}}\] are present in a container and at equilibrium, 30 mL of \[HI\] is formed, then calculate equilibrium constant.
question_answer35) What happens to the equilibrium \[PC{{l}_{5}}(g)\rightleftharpoons PC{{l}_{3}}(g)+C{{l}_{2}}(g),\] if nitrogen gas is added to it (i) at constant volume (ii) at constant pressure? Give reasons.
question_answer36) What two changes on the equilibrium, \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g),\,\,\Delta H=-92.4kJ.\] can keep its state undisturbed?
question_answer37) The following reaction has attained equilibrium \[CO(g)+2{{H}_{2}}(g)\rightleftharpoons C{{H}_{3}}OH(g),\,\Delta {{H}^{{}^\circ }}=-92.0kJmo{{l}^{-1}}\] What will happen if (i) volume of the reaction vessel is suddenly reduced to half? (ii) the partial pressure of hydrogen is suddenly doubled? (iii) an inert gas is added to the system?
question_answer38) The following system is in equilibrium : \[S{{O}_{2}}C{{l}_{2}}+Heat\rightleftharpoons S{{O}_{2}}+C{{l}_{2}}\] What will happen to the temperature of the system if some \[C{{l}_{2}}\] is added into it at constant volume? Give reason.
question_answer39) A reaction \[A(g)+B(g)\rightleftharpoons 2C(g)\] is in equilibrium at a certain temperature. Can we increase the amount of products by (i) adding catalyst (ii) increasing pressure?
question_answer40) Why does ice melt slowly at higher altitudes?
question_answer41) \[2{{N}_{2}}O(g)+{{O}_{2}}(g)\rightleftharpoons 4NO(g);\Delta H>0\] What will be the effect on equilibrium when (i) Volume of the vessel increases? (ii) Temperature decreases?
question_answer42) Some processes are given below. What happens to the process if it is subjected to a change given in the brackets? (i) \[\text{Ice}\overset{M.pt}{\mathop{\rightleftharpoons }}\,Water(Pressure\,is\,increased)\] (ii) Dissolution of \[NaOH\] in water (Temperature is increased) (iii)\[{{N}_{2}}(g)+{{O}_{2}}(g)\rightleftharpoons 2NO(g)-180.7kJ\] (Pressure is increased and temperature is decreased).
question_answer43) How does the degree of ionization of a weak electrolyte vary with concentration? Give exact relationship. What is this law called?
question_answer44) Classify each of the following substances into an acid or base or both and mention the concept/concepts on the basis of which you can do so. (i) \[HCl\,(aq)\] (ii) \[N{{H}_{3}}\,(g)\] (iii) \[N{{a}_{2}}C{{O}_{3}}\,(aq)\] (iv) \[C{{H}_{3}}COOH\,(aq)\] (v) \[C{{O}_{2}}(g)\] (vi)\[B{{F}_{3}}\] (vii) \[A{{g}^{+}}\] (viii) \[C{{N}^{-}}\] (ix) \[{{H}_{2}}O\] (x) \[{{H}_{2}}S{{O}_{4}}\] (xi) \[HCO_{3}^{-}\] (xii) \[Si{{F}_{4}}\]
question_answer45) Write down the conjugate acid and conjugate base of (i) \[{{H}_{2}}O\] (ii) \[HSO_{4}^{-}\] (iii) \[N{{H}_{3}}\] (iv) \[H{{S}^{-}}\]
question_answer46) Out of \[C{{H}_{3}}CO{{O}^{-}}\]and \[O{{H}^{-}}\] which is stronger base and why?
question_answer47) Why is ammonia termed as a base though it does not contain \[O{{H}^{-}}\] ions?
question_answer48) Arrange the given species in order of their increasing basic character : \[{{H}_{2}}O,\,O{{H}^{-}},\,C{{H}_{3}}OH,\,C{{H}_{3}}{{O}^{-}}\]
question_answer49) Between \[N{{a}^{+}}\] and \[A{{g}^{+}}\] which is stronger Lewis acid and why?
question_answer50) How is the degree of dissociation of a weak base related to its molarity?
question_answer51) lonization constants \[{{K}_{a}}\] for formic acid and acetic acid are \[17\cdot \,7\times {{10}^{-5}}\] and \[1\cdot 77\times {{10}^{-5}}\]. Which acid is stronger and how many times the other if equimolar concentrations of the two are taken?
question_answer52) What is the effect of temperature on ionic product of water and why?
question_answer53) What happens to the ionic product of water if some acid is added into water?
question_answer54) What are pH and \[pOH\] values of a neutral solution at a temperature at which \[{{K}_{w}}={{10}^{-13}}\]?
question_answer55) What pH do you expect for \[{{10}^{-8}}\,M\] solution of an acid?
question_answer56) Will the pH of water be same at 4°C and 25°C? Explain.
question_answer57) For an aqueous solution of \[N{{H}_{4}}Cl,\] prove that \[[{{H}_{3}}{{O}^{+}}]\,=\sqrt{{{K}_{h}}C}\].
question_answer58) The pH of an enzyme catalysed reaction has to be maintained between 7 and 8. What indicator should be used to monitor and control the pH?
question_answer59) The\[p{{K}_{\ln }}\] of an indicator is 10.5. For which pH transition range is the indicator most suitable?
question_answer60) Benzoic acid is a monobasic acid. When 1.22 g of its pure sample are dissolved in water and titrated against base, 50 ml of 0.2 M NaOH are used up. Calculate the molar mass of benzoic acid.
question_answer61) A solution gives yellow colour with methyl orange, methyl red and phenol red. What is the pH of the solution?
question_answer62) What is the difference between ionic product and solubility product?
question_answer63) NaCI solution is added to a saturated solution of \[PbC{{l}_{2}}\]. What will happen to the concentration of\[P{{b}^{2+}}\]ions?
question_answer64) When is a precipitate formed when solutions of \[BaC{{l}_{2}}\] and \[N{{a}_{2}}S{{O}_{4}}\] are mixed?
question_answer65) Will \[AgCl\] be more soluble in aqueous solution or \[NaCl\] solution and why?
question_answer66) Why solid \[NaCl\] starts separating out from a saturated solution of \[NaCl\] if \[HCl\] gas is passed through it?
question_answer67) Why common salt is added to precipitate out soap from the solution during its manufacture?
question_answer68) Through a solution containing \[C{{u}^{2+}}\] and \[N{{i}^{2+}},\,{{H}_{2}}S\] gas is passed after adding dil \[HCl,\] which will precipitate out and why?
question_answer69) Why in Group V of qualitative analysis, sufficient \[N{{H}_{4}}OH\] solution should be added before adding\[{{(N{{H}_{4}})}_{2}}C{{O}_{3}}\] solution?
question_answer70) Two sparingly soluble salts AB and \[X{{Y}_{2}}\] have the same solubility product. Which salt will be more soluble? Explain.
question_answer71) The ionization constant of formic acid is \[1.8\times {{10}^{-4}}\]. Around what pH will its mixture with sodium formate give buffer solution of highest capacity?
question_answer72) Blood is a buffer of \[{{H}_{2}}C{{O}_{3}}\] and \[[HCO_{3}^{-}]\]with pH = 7.40. Given \[{{K}_{1}}\] of \[{{H}_{2}}C{{O}_{3}}=4.5\,\times {{10}^{-7}}\]. What will be the ratio of \[[HCO_{3}^{-}]\] to \[[{{H}_{2}}C{{O}_{3}}]\] in the blood?
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