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question_answer1) Equilibrium constant K for the reaction \[CaC{{O}_{3}}(s)\rightleftharpoons CaO(s)+C{{O}_{2}}(g)\] is 0.82 atm at\[727{}^\circ C\]. If 1 mole of \[CaC{{O}_{3}}\]is placed in a closed container of 20L and heated to this temperature, what amount of \[CaC{{O}_{3}}\] in grams would dissociate at equilibrium?
question_answer2) An amount of solid \[N{{H}_{4}}HS\] is placed in a flask already containing ammonia gas at a certain temperature and 1.0 atm pressure. Ammonium hydrogen sulphide decomposes to yield \[N{{H}_{3}}\] and \[{{H}_{2}}S\] gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 2 atm. What will be the equilibrium constant for \[N{{H}_{4}}HS\] decomposition at this temperature?
question_answer3) Calculate the pH of a solution obtained by diluting 1 mL of 0.10 M weak monoacidic base to 100 mL at constant temperature if \[{{K}_{b}}\] of the base is \[1\times {{10}^{-\,5}}\].
question_answer4) 28 g \[{{N}_{2}}\] and 6.0 g of \[{{H}_{2}}\] are heated over catalyst in a closed one litre flask of \[450{}^\circ C\]. The entire equilibrium mixture 1 required 500 mL of \[\]for neutralisation. Calculate the value of \[{{K}_{c}}\] in \[{{L}^{2}}mo{{l}^{2}}\] for the given reaction. \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g)\]
question_answer5) The equilibrium constant of the reaction of weak acid ha with strong base is \[{{10}^{-7}}\]. Find the pOH of the aqueous solution of 0.1M NaA.
question_answer6) For the reaction \[C(s)+C{{O}_{2}}(g)\to 2CO(g),{{K}_{p}}\] \[=63\,\,atm\,\,\,at\] 1000 K. If at equilibrium: \[{{P}_{CO}}=10\,{{P}_{C{{O}_{2}}}}.\] Find the total pressure (atm) of the gases at equilibrium.
question_answer7) The \[p{{K}_{a}}\] of \[HCOOH\] is 3.8 and \[p{{K}_{b}}\]of \[N{{H}_{3}}\] is 4.8, find the pH of aqueous solution of 1M\[HCOON{{H}_{4}}\].
question_answer8) In the reaction \[AB(g)\rightleftharpoons A(g)+B(g)\] at \[30{}^\circ \text{ }C,\text{ }{{K}_{p}}\] for the dissociation equilibrium is \[1.6\times {{10}^{-3}}\] atm. If the total pressure at equilibrium is 1 atm, then calculate the percentage dissociation of AB.
question_answer9) Calculate the pH at the equivalence point when a solution of 0.01 M \[C{{H}_{3}}COOH\] is titrated with solution of 0.01 M NaOH. \[p{{K}_{a}}\] of \[C{{H}_{3}}COOH\] is 4.74.
question_answer10) The value of \[{{K}_{p}}\] for the equilibrium reaction \[{{N}_{2}}{{O}_{4}}(g)\rightleftharpoons 2N{{O}_{2}}(g)\] is 2. Calculate the percentage dissociation of \[{{N}_{2}}{{O}_{4}}(g)\] at a pressure of 0.5 atm.
question_answer11) A buffer solution is prepared by mixing 10 mL of 1.0 M \[C{{H}_{3}}COOH\] and 20 mL of 0.5 M \[C{{H}_{3}}COONa\] and then diluted to 100 mL with distilled water. If \[p{{K}_{a}}\] of \[C{{H}_{3}}COOH\] is 4.76, what is the pH of the buffer solution?
question_answer12) At a certain temperature and 2 atm pressure equilibrium constant \[({{K}_{p}})\] is 25 for the reaction \[S{{O}_{2}}(g)+N{{O}_{2}}(g)\rightleftharpoons S{{O}_{3}}(g)+NO(g)\] Initially if we take 2 moles of each of the four gases and 2 moles of inert gas, what would be the equilibrium partial pressure of \[N{{O}_{2}}\] in atm?
question_answer13) Find the pH of a 2 litre solution which is 0.1 M each with respect to \[C{{H}_{3}}COOH\] and \[{{(C{{H}_{3}}OO)}_{2}}Ba.\,\,({{K}_{a}}=1.8\times {{10}^{-5}})\]
question_answer14) On addition of increasing amount of \[AgN{{O}_{3}}\]to 0.1 M each of NaCl and NaBr in a solution, what % of \[B{{r}^{-}}\] ion gets precipitated when \[C{{l}^{-}}\] ion starts precipitating? Given: \[{{K}_{sp}}(AgCl)=1.0\times {{10}^{-10}};\] \[{{K}_{sp}}(AgBr)=1\times {{10}^{-13}}\]
question_answer15) What can be the maximum possible molarity of \[C{{o}^{2+}}\] ions in 0.1 M HCl saturated with \[{{H}_{2}}S({{K}_{a}}=4\times {{10}^{-21}})?\] Given that \[{{K}_{sp}}\] for CoS is \[2\times {{10}^{-21}}\] and concentration of saturated \[{{H}_{2}}S=0.1\,M\].
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