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question_answer1) What mass of \[{{N}_{2}}{{H}_{4}}\] can be oxidized to \[{{N}_{2}}\] by 24.0 gm of \[{{K}_{2}}Cr{{O}_{4}},\] which is reduced to\[Cr\left( OH \right)_{4}^{-}\]?
question_answer2) It requires 40 ml of 0.5 (M) \[C{{e}^{4+}}\] to titrate 10 ml of 1(M) \[S{{n}^{2+}}\] to \[S{{n}^{4+}}\]. What is the oxidation state of cerium in the reduction product?
question_answer3) A sample of 2.5 moles of \[{{N}_{2}}{{H}_{4}}\] loses 25 moles of electrons on being converted to a new compound 'X'. Assuming that there is no loss of nitrogen in the formation of the new compound, what is the oxidation number of nitrogen in compound 'X'?
question_answer4) What volume of \[{{H}_{2}}\] at NTP is needed to reduce 125 gm. of \[Mo{{O}_{3}}\] to metal?
question_answer5) In acting as a reducing agent, a piece of metal M weighing 16 grams gives up \[2.25\,\,\times \,\,{{10}^{23}}\] electrons, what is the equivalent weight of the metal
question_answer6) When the ion \[C{{r}_{2}}O_{7}^{2-}\] acts as an oxidant in acidic aqueous solution the ion \[C{{r}^{3+}}\] is formed. How many moles of \[S{{n}^{2+}}\] would be oxidised to \[S{{n}^{4+}}\]by one mole of \[C{{r}_{2}}O_{7}^{2-}\] ions −
question_answer7) A solution of \[KCl\]and \[KOH\]was neutralized with 120 ml of 0.12 (N) \[HCl.\] What is the amount of KOH in the mixture −
question_answer8) \[{{H}_{3}}P{{O}_{4}}\] is a tribasic acid and one of its salt is \[Na{{H}_{2}}P{{O}_{4}}.\]What volume of 1 (M) \[NaOH\] solution should be added to 12 gm of \[Na{{H}_{2}}P{{O}_{4}}\] to convert it into \[N{{a}_{3}}P{{O}_{4}}\]?
question_answer9) What is the strength in gm/litre of a solution of \[{{H}_{2}}S{{O}_{4}},\] 12 ml of which neutralizes 15 ml of N/10 \[NaOH\] solution?
question_answer10) The volume of 0.1 M \[{{H}_{2}}S{{O}_{4}}\] solution required to neutralise 50 ml of 0.2 M \[NaOH\]solution is −
question_answer11) If 20 ml of 0.4 N \[NaOH\]solution completely neutralises 40 ml of a dibasic acid, the molarity of the acid solution is -
question_answer12) If 25.8 ml of 0.101 M \[{{K}_{2}}C{{r}_{2}}{{O}_{7}}\] are required to titrate 10.0 ml of a liquid iron supplement calculate the concentration of iron in vitamin solution (Take valency factor of \[Fe\,\,=\,\,1\])
question_answer13) 10 ml of \[{{H}_{2}}{{O}_{2}}\] solution when reacted with \[KI\]solution produced 0.5 g of iodine. Calculate % of purity of \[{{H}_{2}}{{O}_{2}}\] (by volume).
question_answer14) Among the following, the number of elements showing only one non-zero oxidation state is \[O,\,\,\,\,Cl,\,\,\,\,F,\,\,\,\,N.\,\,\,\,P,\,\,\,\,Sn,~\,\,\,\,Tl,\,\,\,\,~Na,\,\,\,\,Ti\]
question_answer15) Reaction of \[B{{r}_{2}}\] with \[N{{a}_{2}}C{{O}_{3}}\] in aq. solution gives sodium bromide and sodium bromate with evolution of \[C{{O}_{2}}\] gas. The number of sodium bromide molecules involved in the balanced chemical equation is.
question_answer16) The difference in the oxidation numbers of the two types of sulphur atoms in \[N{{a}_{2}}{{S}_{4}}{{O}_{6}}\] is.
question_answer17) In neutral or faintly alkaline solution, 8 moles of permanganate anion quantitatively oxidize thiosulphate anions to produce X moles of a sulphur containing product. The magnitude of \[X\] is.
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