Question 1 :
If $22 gm$ benzene Present in $100 gm\, CCl_4$ then find the $\% W/W$ of benzene in solution:
Question 2 :
100ml of a solution contains $6.02\times { 10 }^{ 22 }$ molecules of oxalic acid. Its normality is:
Question 3 :
What volume of $2M\ { H }_ { 2 }S{ O }_{ 4 }$ is required to form 0.2 N of 100 mL of solution?
Question 4 :
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 5 :
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 6 :
$25\ ml$ 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 7 :
250 ml of sodium carbonate solution contains 2.65g of ${ Na }_{ 2 }{ CO }_{ 3 }$. If 10 ml of the solution is diluted to 1 L. What is the concentration of the resultant solution?
Question 8 :
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 9 :
What volume of $N/2$ and $N/10\ HCl$ should be taken in order to make a $2\ litre$ solution of $N/5$ strength?
Question 10 :
The molarity of a solution obtained by mixing 750 $mL$ of $0.5M \ HCl$ with 250 $mL$ of $2M\ HCl$ will be :<br/>
Question 11 :
250 ml of a sodium carbonate solution contains 2.65 grams of $Na_2CO_3$. If 100 ml of this solution is diluted to one litre, what is the concentration of the resultant solution?
Question 12 :
A solution has a $1:4$ mole ratio of pentane to hexane. The vapour pressures of pure hydrocarbons at $20^o$C are $440$ mm Hg for pentane and $120$ mm Hg for hexane. The mole fraction of pentane in vapour phase would be:
Question 13 :
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 15 :
100 ml of 0.3 N HCl solution is mixed with 200 ml of 0.6 N $H_2SO_4$ solution. What is the normality of $H_2SO_4$ in the final solution?
Question 16 :
The volume of water to be added to 500 ml of 0.25 N hydrochloric acid to make it exactly decinormal is:
Question 17 :
What is the molarity of a saturated solution of $CaCO_{3}$? $(K_{SP}=2.8\times 10^{-9})$
Question 18 :
What is the molarity if a 500 mL solution contains 20 g of $CaBr_2$?<br>
Question 19 :
Number of ions present in 500 ml of 2M ${ Na }_{ 2 }{ SO }_{ 4 }$ solution are:
Question 20 :
$4.0 \,gm$ of $NaOH$ are contained in one decilitre of solution, its molarity would be
Question 21 :
The molarity of $4\ N\ H_2SO_4$ in the following reaction is $8H^+ +H_2SO_4 + 8e^- \to H_2S +4H_2O$
Question 22 :
The volume of $10$ volume H$_2$O$_2$ solution that decolourises $200$ ml of $2$ N KMnO$_4$ solution in acidic medium is:
Question 23 :
A 5 molar solution of ${ H }_{ 2 }S{ O }_{ 4 }$ is diluted form $1 L$ to $10 L$. What is the normality of the solution?
Question 24 :
$1\ mol$ 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 25 :
About how many grams of sodium chloride would be dissolved in water to form a $0.5$ M solution in $500$ mL solution?<br/>
Question 26 :
Find the amount of $98\%$ pure $Na_2CO_3$ required to prepare 5 litres of 2 N solution.
Question 27 : Two solutions of a substance (non-electrolyte) are mixed in the following manner. <div><br/><div>480 ml of 1.5 M first solution + 520 ml of 1.2 M second solution. </div><br/><div>What is the molarity of the final mixture? </div></div>
Question 28 :
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 29 :
The amount of sugar $(C_{12}H_{22}O_{11}$) required to prepare $2L$ of its $0.1 M$ aqueous solution is:
Question 30 :
$10$ mL sample of human urine was found to have $5$ mg of urea on analysis. Calculate the molarity of the given sample with respect to urea (molecular mass $= 60$ g/mol).<br/>
Question 31 :
Essential quantity of ammonium sulphate taken for preparation of 1 molar solution in 2 litres is
Question 32 : <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 34 :
Density of a ${H}_{2}{SO}_{4}$ solution is $1.2\ g/ml$ and it is $40%\ {H}_{2}{SO}_{4}$ by weight. Determine molarity of this solution.
Question 35 :
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 36 :
What is the concentration of an $NaOH$ solution if it takes $12.50\ mL$ of a $0.100\ M\ HCl$ solution to titrate $25.00\ mL$ of the $NaOH$ solution?
Question 37 :
$100\ mL$ of a $0.25\ M\ (Ba(OH)_{2}$ solution was used to titrate $12.5\ mL$ of a $HNO_{3}$ solution to neutralization. What was the concentration of the acid?
Question 38 :
The weight of sodium carbonate required to prepare $500 \,ml$ of a semi- normal solution is
Question 39 :
Find the volume of a 0.2 molar solution of sodium hydroxide, which is used to neutralize 40 liters of a 0.3 molar hydrochloric acid solution.<br/>
Question 40 :
The molarity of $Cl^-$(100 ml) ions in the solution after $0.2$ moles $HCl$ are mixed with $0.1$ moles $CaCl_2$ solution?
Question 41 :
If $500\ ml$ of $0.2M\ NaCl$ solution is mixed with $200\ ml$ of $0.16M\ NaCl$ solution and then diluted to one liter with water, what is the molarity of the resulting solution?
Question 42 :
Concentration terms like mass percentage, ppm, mole fraction and molality do not depend on temperature. However, molarity is a function of temperature because:
Question 43 :
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 44 :
An aqueous solution of 6.3 g oxalic acid dihydrate is made up to 250 mL. The volume of 0.1 N NaOH required to completely neutralize 10 mL of this solution is : <br>
Question 45 :
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 46 :
$25.0 \,ml$ of $HCl$ solution gave, on reaction with excess $AgNO_3$ solution $2.125g$ of $AgCl$. The molarity of $HCl$ solution is:
Question 47 :
A quantity of $1\ kg$ of $2\ m$ urea solution is mixed with $2\ kg$ of $4\ m$ urea solution. The molality of the resulting solution is
Question 48 :
Sulphuric acid is $95.8$% by mass. Calculate mole fraction of $H_{2}SO_{4}$ of density $1.91\ cm^{-3}.$ $(H = 1, S = 32, O = 16 $).
Question 49 :
Which technique would be applied to determine the concentration of an unknown sample of an acid?
Question 50 :
What is the mole fraction of the solute in a 1.00 m aqueous solution?<br>
