Question 1 :
$252$ 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 2 :
What is the correct unit for the following solution?<br/>$0.5\ moles$ of $HCl$ dissolved in $0.25\ L$ of the solution.

Question 3 :
The weight of sodium carbonate required to prepare $500 \,ml$ of a semi- normal solution is

Question 4 :
What is the normality of a $1 \,M$ solution of $H_3PO_4$?

Question 5 :
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 6 :
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 7 :
How many grams of dibasic acid (Mol.wt.=200) should be present in 100ml of its aqueous solution to give deci normal strength?

Question 8 :
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 9 :
$5\ mL$ of $N\ HCl, 20\ mL$ of $N/2\ H_{2}SO_{4}$ and $30\ mL$ of $N/3\ HNO_{3}$ are mixed together and volume made to $1 L$. <br/><div>The normality of the resulting solution is :</div>

Question 10 :
Calculate the molarity of pure water using its density to be $1000 kg m^{-3}$.

Question 11 :
${ 10 }^{ -1 }M$ HCl is diluted to 100 times. Its pH is :

Question 12 :
How many grams of $NaOH$ should be added in $100$ml to get $2$M $NaOH$ aqueous solution?<br/>(Atomic weight of $NaOH$ is $40$ gm/mol).<br/>

Question 13 :
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 14 :
$10\; L$ of $2\;M\; NaCl$ solution is subjected to following changes. Calculate final molarity, if it is diluted by $20\; L$ :<br/>

Question 15 :
$25.0 \,ml$ of $HCl$ solution gave, on reaction with excess $AgNO_3$ solution $2.125g$ of $AgCl$. The molarity of $HCl$ solution is:

Question 16 :
________methods are used for analyzing acids or bases to determine the unknown concentration.

Question 17 :
Molarity of 26% (w/w) ammonia solution, having a density of $0.85\ g/ml$ is:

Question 18 :
$1\ mol$ 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 19 :
$5$ ml of $1N$ HCl, $20$ ml of $\dfrac{N}{2}$ $H_2SO_4$ and $30$ ml of $\dfrac{N}{3}$ $HNO_3$ are mixed together and the volume is made to $1$ L. The normality of the resulting solution is :

Question 20 :
A weak acid, $HA$, has $K_{a}$ of $1.00\times 10^{-5}$. If $0.100$ mole of this acid is dissolved in $1L$ of water, the percentage of acid dissociated at equilibrium is closest to:

Question 21 :
What is the molarity of a saturated solution of $CaCO_{3}$? $(K_{SP}=2.8\times 10^{-9})$

Question 22 :
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 23 :
If $8.3\ ml$ of a sample of $H_{2}SO_{4}(36\ N)$ is diluted by $991.7\ ml$ of water, the approximate normality of the resulting solution is:

Question 25 :
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 26 :
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 27 :
How many moles of electrons are required to electroplate a $0.5$ mole of silver from a nitrate solution?

Question 28 :
What is the molarity of a solution containing $10g$ of $NaOH$ in $500\ mL$ of the solution?

Question 29 :
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 30 :
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 31 :
How many grams of sulphuric acid is to be dissolved to prepare $200 mL$ aqueous solution having concentration of $1 M$ $\left[ { H }_{ 3 }{ O }^{ + } \right] $ ions at ${ 25 }^{ o }C$ temperature?<br>$\left[ H=1,O=16,S=32g{ mol }^{ -1 } \right] $

Question 32 :
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 33 :
A $1$ molal solution of $NaCl$ results when $58.5 g$ of sodium chloride is dissolved in:

Question 34 :
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 36 :
Molarity of a solution prepared by dissolving $75.5 \,g$ of pure $KOH$ in $540 \,ml$ solution is

Question 37 :
Two samples of HCl of $1.0$ M and $0.25$ M are mixed. Find volumes of these samples taken in order to prepare $0.75$ M HCl solution. Assume no water is added.<br/>(I) $20$ mL, $10$ mL (II) $100$ mL, $50$ mL (III) $40$ mL, $20$ mL (IV) $50$ mL, $25$ mL

Question 38 :
Assertion: The normality of $0.3\ M$ aqueous solution of $H_{3} PO_{3}$ is equal to $0.6\ N$. Reason: Equivalent weight of $H_{3} PO_{3} = \dfrac {\text {Molecular weight of} H_{3} PO_{3}}{3}$

Question 39 :
Two litres of $NH_3$ at $3^0C$ and $0.20$ atmosphere is neutralised by $134$ mL of a solution of $H_2SO_4$. If the normality of $H_2SO_4$ is $x$ N then, find the value of $100x$.<br>

Question 40 :
Which technique would be applied to determine the concentration of an unknown sample of an acid?

Question 41 :
Calculate the normality of $250mL$ aqueous solution of ${ H }_{ 2 }{ SO }_{ 4 }$ having $pH=0.00$:

Question 42 :
$10$ 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 44 :
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 45 :
Find the amount of $98\%$ pure $Na_2CO_3$ required to prepare 5 litres of 2 N solution.

Question 46 :
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 47 :
Concentration terms like mass percentage, ppm, mole fraction and molality do not depend on temperature. However, molarity is a function of temperature because:

Question 48 :
What will be the molality of the solution made by dissolving $10\ g$ of $NaOH$ in $100\ g$ of water?

Question 49 :
1.5 litre of solution of normality N and 2.5 litres of 2M HCl are mixed together. The resultant solution has a normality of 5. The value N is:

Question 50 :
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?