Question 1 :
$Y$ molal solution of a compound in benzene has mole fraction of solute equal to $0.2$. The value of ?
Question 2 :
A solution of known normality is diluted to two times. Which of the following changes during dilution?
Question 4 :
Measuring molarity of an ionic solution can be accomplished utilizing numerous methods.<br/>Which of the following is the least accurate method for the solution described?
Question 5 :
Semimolar solution contains how many moles of solute in 1L of solution?
Question 6 :
<b></b>Calculate the volume in 10 millimoles of solute present in 0.08 M solution.
Question 7 :
The number of grams of anhydrous $Na_2CO_2$ present in 250 mL of 0.25 M solution is:
Question 8 :
What volume of $0.8M$ solution contains $0.1$ mole of the solute?
Question 9 :
If true enter $1$, else enter $0$.<br/>Normality $=$ Molarity $\times$ Valence factor
Question 10 :
If sea water contains <b>63</b> ppm $NO_{3}^{-}$ and its density is <b>1.01 </b>g/mL, the approximate molarity of sea water is:
Question 12 :
$9.8$ grams of $H_{2}SO_{4}$ is present in two litres of a solution. The molarity of the solution is:<br/>
Question 13 :
The weight ( in-grams) of ${ AgNO }_{ 3 }$ present in 100 ml of 0.25 M solution :
Question 14 : <p class="MsoNormal"> The concentration of the solution is___________. <br/> <span>I) $\dfrac{amount\ of\ solvent}{ amount\ of\ solution}$<br/> II) $\dfrac{amount\ of\ solute}{ amount\ of\ solution}$</span></p>
Question 15 :
In acidic medium which of the following does not change its colour:
Question 16 :
What is the molarity of an aqueous solution of ethyl alcohol ($CH_3CH_2OH$, molar mass $= 46.0$ $g\ mol^{-1}$) which contains 50.0 g of alcohol in 500 mL of the solution?<br/>
Question 17 :
${ 10 }^{ -1 }M$ HCl is diluted to 100 times. Its pH is :
Question 18 : <div><br/><div>$Cl_2(g)+S_2O_3^{2-}\longrightarrow SO_4^{2-}+Cl^-+S$</div><br/></div>If $50.0$ mL of $0.01\ M\ Na_2S_2O_3$ solution and $5\times 10^{-4}$ moles of $Cl_2$ react according to given equation then how many moles of $S_2O_3^{2-}$ are in the above sample?<br/>
Question 19 :
The molarity of $98$ percent $H_{2}SO_{4}$ (density $=1.8\ g/ml$) by weight would be:
Question 20 :
Volume of 0.1M ${ K }_{ 2 }{ Cr }_{ 2 }{ O }_{ 7 }$ required to oxidise 35ml of 0.5M ${ FeSO }_{ 4 }$ solution is:
Question 21 :
Calculate the molarity of pure water using its density to be $1000 kg m^{-3}$.
Question 22 :
Ten grams of sodium hydroxide dissolved in $1 L$ of water makes a solution that is:
Question 23 :
A solution is 0.1 M in each of ${ PO }_{ 4 }^{ 3- },{ SO }_{ 4 }^{ -3 }$ and ${ Cl }^{ - }$ ions. Solid ${ AgNO }_{ 3 }$ is added gradually to this solution which causes no change in volume of the solution. Given ${ K }_{ ap }\left( AgCl \right) =1.8\times { 10 }^{ -10 }$, ${ K }_{ ap }\left({ Ag }_{ 2 }{ SO }_{ 4 } \right) =1.21\times { 10 }^{ -3 }$ and ${ K }_{ ap }\left({ Ag }_{ 3 }{ SO }_{ 4 } \right) =2.7\times { 10 }^{ -18 }$.<br/>The concentrations of first and third ions when the second ion starts precipitating, respectively, are:<br/>
Question 24 :
The molarity of $4\ N\ H_2SO_4$ in the following reaction is $8H^+ +H_2SO_4 + 8e^- \to H_2S +4H_2O$
Question 25 :
A titration is carried out using $0.010\ M\ KMnO_{4}(aq)$, in the presence of excess sulfuric acid, to determine the concentration of iron(II) ion in a solution of iron (II) sulfate, $FeSO_{4}$. The balanced equation for the reaction is<br/>$2KMnO_{4}(aq) + 10FeSO_{4}(aq) + 8H_{2}SO_{4}(aq) \rightarrow 5Fe_{2}(SO_{4})_{3}(aq) + 2MnSO_{4}(aq) +K_{2}SO_{4}(aq) $<br/> $+ 8H_{2}O(l)$<br/>If $25 mL$ of the $FeSO_{4}$ solution requires $37\ mL$ of the permanganate titrant, which of the following expressions CORRECTLY gives the concentration of $Fe^{2+}$, in mol/L, in the iron(II) sulfate solution?<br/>(The molar masses of the reactants and products are: $KMnO_{4}, 158\ g/mol; FeSO_{4}, 152\ g/mol; Fe_{2}(SO_{4})_{3}, 400\ g/mol$; and $MnSO_{4}, 151\ g/mol$.)
Question 26 :
What is the mole fraction of the solute in a 1.00 m aqueous solution?<br>
Question 27 :
The volume of water to be added to 500 ml of 0.25 N hydrochloric acid to make it exactly decinormal is:
Question 28 :
In a laboratory experiment, a student placed sodium hydroxide crystals on a watch glass and assembled the titration equipment. Then he prepared a solution of $0.10$M sulfuric acid. He weighed $4$ grams of sodium hydroxide and added it to enough water to make $1$ liter of solution. What might be a source of error in the results of the titration?
Question 30 :
A $100\ mL$ solution containing $AgNO_3$ was treated with excess $NaCl$ to completely precipitate the silver as $AgCl$. If $5.7\ g\ AgCl$ was obtained, what was the concentration of $Ag^+$ in the original solution? (At. mass of $Ag=108\ g/mol$)
Question 31 :
Assertion: Molarity and molality for very dilute aqueous solution is approximately equal.
Reason: For all aqueous solution, total mass of solvent is approximately equal to total volume of solution.
Question 32 :
A 3.4 g sample of $H_2O_2$ solution containing $x\%\, H_2O_2$ by mass requires x mL of a $KMnO_4$ solution for complete oixidation under acidic condition.The molarity of $KMnO_4$ solution is:
Question 33 :
What is the molarity of a saturated solution of $CaCO_{3}$? $(K_{SP}=2.8\times 10^{-9})$
Question 34 :
$1\ mol$ of iron $(Fe)$ reacts competely with $0.65\ mol\ O_{2}$ to give a mixture of only $FeO$ and $Fe_{2}O_{3}$. Mole ratio ferrous oxide to ferric oxide to ferric oxide is:
Question 36 :
If 98 grams of $\displaystyle { H }_{ 2 }{ SO }_{ 4 }$ is added in sufficient water to make 500 milliliters of solution, then what is the molarity of a solution?
Question 37 :
The volume of water to be added to $100\ cm^{3}$ of $0.5\ N\ H_{2}SO_{4}$ to get decinormal concentration is:
Question 38 :
Number of ions present in 500 ml of 2M ${ Na }_{ 2 }{ SO }_{ 4 }$ solution are:
Question 39 :
What is the molarity if a 500 mL solution contains 20 g of $CaBr_2$?<br>
Question 40 :
What will be the molality of the solution made by dissolving $10\ g$ of $NaOH$ in $100\ g$ of water?
Question 42 :
Molarity of 26% (w/w) ammonia solution, having a density of $0.85\ g/ml$ is:
Question 43 :
20 ml $\dfrac{N}{10}$ $HCl$ is mixed with 40 ml $\dfrac{N}{10}$ NaOH solution. The normality of the resultant acidic/basic solution will be:
Question 44 :
The molarity$(M)$ of $KMnO_4$ solution in the acidic medium is :
Question 45 :
100ml of 0.3N $HNO_{3}$ and 200ml of $0.3M\ H_{2}SO_{4}$ are mixed together. Normality of $H^{+}$ in the resulting solution is:
Question 46 : <p>$500$ ml aqueous solution is prepared by dissolving $2$ moles of $HCl$ in water. What will be the molarity of this solution ? </p>
Question 47 :
In an auto engine with no pollution controls, about 5% of the fuel $(C_{8}H_{18})$ is unburned. Molar ratio of $CO$ and $(C_{8}H_{18})$, emitted in the exhaust gas is:
Question 48 :
$4.0 \,gm$ of $NaOH$ are contained in one decilitre of solution, its molarity would be
Question 49 :
The ratio of the molar amounts of $H_2S$ needed to precipitate the metal ions from 20 ml each of 1M $Cd(NO_3)_2$ and $0.5 M CuSO_4$ is:
Question 50 :
An aqueous solution contains 0.53g of anhydrous ${ { Na }_{ 2 }CO }_{ 3 }$ (Mol. wt. 106) dissolved in 100ml of solution. The molarity of the solution is:
Question 51 :
For a solution of volatile liquids the partial vapour pressure of each component in solution is directly proportional to
Question 53 :
$25\ ml$ of a solution of barium hydroxide on titration with a $0.1$ molar solution of hydrochloric acid gave a titre value of $35\ ml$. The molarity of barium hydroxide solution was:
Question 54 :
One litre of $0.15$ M HCl and one litre of $0.3$ M HCl is given. What is the maximum volume of $0.2$ M HCl which one can make from these two solutions? No water is added.
Question 55 :
Aqueous solution of $HCl$ has the $pH=4$. Its molarity would be:
Question 56 :
$25.0 \,ml$ of $HCl$ solution gave, on reaction with excess $AgNO_3$ solution $2.125g$ of $AgCl$. The molarity of $HCl$ solution is:
Question 57 :
The vapour pressure of a dilute aqueous solution of a non-volatile solute (molar mass $180$ g $mol^{-1}$) at $373$K is $750$ mm $Hg$. Calculate the mole fraction of the solute.
Question 58 :
If $22 gm$ benzene Present in $100 gm\, CCl_4$ then find the $\% W/W$ of benzene in solution:
Question 59 :
2.46 g of sodium hydroxide (molar mass = 40) are dissolved in water and the solution is made to 100 cm$^3$ in a volumetric flask. Calculate the molarity of the solution.
Question 60 :
A $40.0\ mL$ sample of $0.100\ M\ HNO_{3}$ is titrated with $0.200\ M\ NaOH$.<br>Calculate the volume required to reach the equivalence point.
Question 61 :
Find the amount of $98\%$ pure $Na_2CO_3$ required to prepare 5 litres of 2 N solution.
Question 62 :
The specific gravity of sulphuric acid 1.8. What volume of this sample of concentrated H$_2$SO$_4$ is required to prepare 500 ml 0.9 M H$_2$SO$_4$ solution?
Question 63 :
16.0 g of NaOH is present in 100 ml of an aqueous solution. Its density is 1.06 g/ml. Mole fraction of the solute is approximately:
Question 64 :
$252$ gm of oxalic acid with molecular formula $C_2H_2O_4\cdot 2H_2O$ dissolve in water to form $250$ ml. of the solution. Its molarity will be:
Question 65 :
What amount of water is added in 40 ml of NaOH (0.1N) which is neutralised by 50 ml of HCl (0.2N)?
Question 66 :
Which technique would be applied to determine the concentration of an unknown sample of an acid?
Question 68 :
Upon heating a litre of $(N/2)HCl$ solution, $2.675\ g$ of hydrogen chlorine is lost and the volume of the solution shrinks to $750\ mL$. What is the normality of the resultant solution?
Question 69 :
Purple of Cassius is prepared by reducing $ AuCl_{3}$ to colloidal by $ SnCl_{2}.$ A 1 L solution containing 1.97 mg of gold per ml is prepared from 0.05 M solution of $ AuCl_{3}$ by reduction with an appropriate amount of $ 0.05 M\ SnCl_{2}$ solution, the resulting solution being diluted to 1 L with water. The volume of stannous chloride solution required, if its oxidation product is $ SnCl_{4}(aq),$ is (Au = 197)
Question 70 :
If two solution $2$M, $300$ml and $3$M, $200$ml are mixed together then find resultant solution molarity.
Question 71 : A solution of $KMnO_4$ containing $3$ g/L is titrated with a solution of $H_2O_2$ containing $2$ g/L.<div>The volume (in ml) of $KMnO_4$ required to react with $20$ mL $H_2O_2$ solution is: (as nearest integer) </div>
Question 72 : $50$ ml of $0.2$N $K_{2}Cr_{2}O_{7}$ is required to oxidize $40$ ml of $FeSO_{4}$ solution in an acidic medium. <div>The weight of iron present in $1L$ of $FeSO_4$ solution is (atomic weight of iron is $56$):</div>
Question 73 :
A bottle labelled with $\displaystyle 12V\:H_{2}O_{2}$ contain $700$ mL solution. If a student mixes $300$ mL of water in it, the strength, normality and volume strength of final solution are:
Question 75 : The strength of an aqueous NaOH solution is $\text{most accurately}$ determined by titrating:<div> <br/>(Note : consider that an appropriate indicator is used)</div>
Question 76 :
A candle is burnt in a beaker until it extinguishes itself. A sample of gaseous mixture in the beaker contains $6.08\times 10^{20}$ molecules of $N_2, 0.76\times 10^{20}$ molecules of $O_2$, and $0.50\times 10^{20}$ molecules of $CO_2$. The total pressure is 734 mm of Hg. The partial pressure of $O_2$ would be :
Question 77 :
$8\ g\ NaOH$ is dissolved in one litre of solution, the molarity of the solution is:
Question 78 : What is the normality of 0.3 M $ H_3PO_4 $ when it undergoes the reaction?<div><br/><div>$ H_3PO_4 +20H^- \rightarrow HPO^{2-}_3 +2H_2O $</div></div>
Question 79 :
$10$ ml of $NaHC_2O_4$ solution is neutralised by $10$ ml of $0.1\; M \;NaOH$ solution. $10$ ml of same $NaHC_2O_4$ solution is oxidised by $10$ ml of $KMnO_4$ solution in acidic medium. Hence, molarity of $KMnO_4$ is :<br/>
Question 80 :
100 ml of 10V $H_2O_2$ solution is heated. The evolved gas is completely reacted with Ca to form CaO. The aqueous solution of Cao is neutralised by 50 ml of $H_2SO_4$ solution. The molarity of $H_2SO4$ is:
Question 81 :
The volume of water to be added to $400\ mL$ of $N/8\ HCl$ to make it exactly $N/12$, is
Question 82 : Match the List - I with List - II and pick up the correct matching from the codes given below:<br/><table class="wysiwyg-table"><tbody><tr><td>List - I<br/>(Electrochemical Parameter)</td><td>List - II<br/>(Units)</td></tr><tr><td>(I) Ionic mobility</td><td>1. $cm^{-1}$</td></tr><tr><td>(II) Cell constant</td><td>2. $ohm^{-1}\, cm^{-1}$</td></tr><tr><td>(III) Specif conductance </td><td>3. $ohm^{-1}\, cm^{-1}\, mol^{-1}$</td></tr><tr><td>(IV) Molar conductance </td><td>4. $cm^2\, V^{-1}s^{-1}$</td></tr><tr><td><br/></td><td><br/></td></tr></tbody></table>
Question 83 :
In an ideal mixture of liquid A and B the mole fraction of A is 0.25 . If the ratio of $ P^0_A $ to $ P^0_B $ is 7/3. how many repeated distillations would be required as a minimum to obtain a small quantity of distillate which has a mole fraction of A , better than 0.80 ?
Question 84 :
Volume of water needed to mix with $10 \,ml \,10 \,N \,HNO_3$ to get $0.1 \,N \,HNO_3$ is:
Question 85 :
29.2% (w/w) $HCl$ stock solution has a density of $1.25 g \space ml^{-1}$. The molecular weight of $HCl$ is $36.5 g \space mol^{-1}$. The volume (ml) of stock solution required to prepare $200 ml$ solution of $0.4$ M $HCl$ is:
Question 86 : On the basis of the information available from the reaction:<div><br/>$\dfrac {4}{3}Al + O_{2} \rightarrow \dfrac {2}{3} Al_{2}O_{3},\ \Delta G = -827\ kJ\ mol^{-1}$ of $O_{2}$, the minimum emf required to carry out the electrolysis of $Al_{2}O_{3}$ is $[F = 96500\ C\ mol^{-1}]$:</div>
Question 87 :
Two oleum samples $A$ and $B$ have labeling $109%$ and $118%$ respectively. $100\ g$ of $A$ is diluted to an a $1\ L$ solution and $100\ g$ of $B$ is diluted to a $1000\ mL$ solution. If both these solutions are mixed, then normality of $H_{2}SO_{4}$ (approx.) in final solution is:
Question 88 :
How many grams of $NaOH$ should be added to water to prepare 250 ml solution of 2 M $NaOH$?<br/>
Question 89 :
The indicator constant of phenolphthalein is approximately $10 ^ { - 8 }.$ A solution is prepared by adding $100.01 { c.c. }$ of $0.01 { N }$ sodium hydroxide to $100.00 { c.c }$ of $0.01 { N }$ hydrochloric acid. If a few drops of phenolphthalein are now added, what fraction of the indicator is converted to its coloured form ?
Question 90 :
What will be the $H^+$ ion concentration in a solution prepared by mixing 50.0mL of 0.20M NaCl, 25mL of 0.10M NaOH and 25.0mL and 0.30M HCl?
Question 91 :
250 ml of ${ Na }_{ 2 }{ CO }_{ 3 }$ solution contains 2.65 g of ${ Na }_{ 2 }{ CO }_{ 3 }$ .10 ml of this solution is mixed with $X$ ml of water to obtain 0.001 M $\displaystyle { Na }_{ 2 }{ CO }_{ 3 }$ solution. The value of $X$ is:
